{"id":87,"date":"2017-12-14T21:25:36","date_gmt":"2017-12-14T21:25:36","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/other-units-temperature-and-density\/"},"modified":"2023-02-09T15:52:33","modified_gmt":"2023-02-09T15:52:33","slug":"other-units-temperature-and-density","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/other-units-temperature-and-density\/","title":{"raw":"2.5 Density and Temperature","rendered":"2.5 Density and Temperature"},"content":{"raw":"<div id=\"ball-ch02_s05\" class=\"section\" lang=\"en\">\r\n<div id=\"ball-ch02_s05_n01\" class=\"learning_objectives editable block\">\r\n<div class=\"bcc-box bcc-highlight\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Define density.<\/li>\r\n \t<li>Calculate density from experimental results.<\/li>\r\n \t<li>Use density as a conversion factor.<\/li>\r\n \t<li>Learn about the various temperature scales that are commonly used in chemistry.<\/li>\r\n \t<li>Convert units of temperature<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<h3>Density<\/h3>\r\nWe use the mass and volume of a substance to determine its density. Thus, the units of density are defined by the base units of mass and length.\r\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large Density = \\frac{mass}{volume}[\/latex]<\/span><\/p>\r\nThe <strong>density<\/strong> of a substance is the ratio of the mass of a sample of the substance to its volume. The SI unit for density is the kilogram per cubic meter (kg\/m<sup>3<\/sup>). For many situations, however, this as an inconvenient unit, and we often use grams per cubic centimeter (g\/cm<sup>3<\/sup>) for the densities of solids and liquids, and grams per liter (g\/L) for gases. Common units for density include g\/mL, g\/cm<sup class=\"superscript\">3<\/sup>, g\/L, or kg\/L. Although there are exceptions, most liquids and solids have densities that range from about 0.7 g\/mL (the density of gasoline) to 19 g\/mL (the density of gold). The density of air is about 1.2 g\/L. Table 1 shows the densities of some common substances.\r\n<table summary=\"This table reports the density of solids, liquids, and gases in grams per centimeters cubed. The values for solids are ice 0.92, oak wood 0.60 to 0.90, iron 7.9, copper 9.0, lead 11.3, silver 10.5, and gold 19.3. The values for liquids are water 1.0, ethanol 0.79, acetone 0.79, glycerin 1.26, olive oil 0.92, gasoline 0.70 to 0.77, and Mercury 13.6. The values for gases, which were measured when the gas was at 25 degrees Celsius and 1 atmosphere, are dry air 1.20, oxygen 1.31, nitrogen 1.14, carbon dioxide 1.80, helium 0.16, neon 0.83, and radon 9.1.\">\r\n<thead>\r\n<tr>\r\n<th style=\"text-align: center;\" colspan=\"3\">Table 1. Densities of Common Substances<\/th>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<th style=\"text-align: center;\">Solids<\/th>\r\n<th style=\"text-align: center;\">Liquids<\/th>\r\n<th style=\"text-align: center;\">Gases (at 25 \u00b0C and 1 atm)<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">ice (at 0 \u00b0C) 0.92 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">water 1.0 g\/mL<\/td>\r\n<td style=\"text-align: center;\">dry air 1.20 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">oak (wood) 0.60\u20130.90 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">ethanol 0.79 g\/mL<\/td>\r\n<td style=\"text-align: center;\">oxygen 1.31 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">iron 7.9 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">acetone 0.79 g\/mL<\/td>\r\n<td style=\"text-align: center;\">nitrogen 1.14 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">copper 9.0 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">glycerin 1.26 g\/mL<\/td>\r\n<td style=\"text-align: center;\">carbon dioxide 1.80 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">lead 11.3 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">olive oil 0.92 g\/mL<\/td>\r\n<td style=\"text-align: center;\">helium 0.16 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">silver 10.5 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">gasoline 0.70\u20130.77 g\/mL<\/td>\r\n<td style=\"text-align: center;\">neon 0.83 g\/L<\/td>\r\n<\/tr>\r\n<tr valign=\"top\">\r\n<td style=\"text-align: center;\">gold 19.3 g\/cm<sup>3<\/sup><\/td>\r\n<td style=\"text-align: center;\">mercury 13.6 g\/mL<\/td>\r\n<td style=\"text-align: center;\">radon 9.1 g\/L<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nWhile there are many ways to determine the density of an object, perhaps the most straightforward method involves separately finding the mass and volume of the object, and then dividing the mass of the sample by its volume. In the following example, the mass is found directly by weighing, but the volume is found indirectly through length measurements.\r\n<div class=\"textbox examples\">\r\n<h3>Example 1:\u00a0Calculation of Density<\/h3>\r\nGold\u2014in bricks, bars, and coins\u2014has been a form of currency for centuries. In order to swindle people into paying for a brick of gold without actually investing in a brick of gold, people have considered filling the centers of hollow gold bricks with lead to fool buyers into thinking that the entire brick is gold. It does not work: Lead is a dense substance, but its density is not as great as that of gold, 19.3 g\/cm<sup>3<\/sup>. What is the density of lead if a cube of lead has an edge length of 2.00 cm and a mass of 90.7 g?\r\n\r\n[reveal-answer q=\"528993\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"528993\"]\r\n\r\nThe density of a substance can be calculated by dividing its mass by its volume. The volume of a cube is calculated by cubing the edge length.\r\n\r\n[latex]\\large\\text{volume of lead cube}=2.00\\text{ cm}\\times 2.00\\text{ cm}\\times 2.00\\text{ cm}={8.00\\text{ cm}}^{3}[\/latex]\r\n\r\n[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{90.7\\text{g}}{{8.00\\text{ cm}}^{3}}=\\frac{11.3\\text{g}}{{1.00\\text{ cm}}^{3}}={11.3\\text{g\/cm}}^{3}[\/latex]\r\n\r\n(We will discuss the reason for rounding to the first decimal place in the next section.)\r\n\r\n[\/hidden-answer]\r\n<h4>Check Your Learning<\/h4>\r\n<ol>\r\n \t<li>To three decimal places, what is the volume of a cube (cm<sup>3<\/sup>) with an edge length of 0.843 cm?<\/li>\r\n \t<li>If the cube in part 1 is copper and has a mass of 5.34 g, what is the density of copper to two decimal places?<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"513756\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"513756\"]\r\n<ol>\r\n \t<li>0.599 cm<sup>3<\/sup><\/li>\r\n \t<li>8.91 g\/cm<sup>3<\/sup><\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<div class=\"textbox\">To learn more about the relationship between mass, volume, and density, use this <a href=\"https:\/\/phet.colorado.edu\/sims\/density-and-buoyancy\/density_en.html\" target=\"_blank\" rel=\"noopener noreferrer\">PhET Density Simulator<\/a>\u00a0to explore the density of different materials, like wood, ice, brick, and aluminum.<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Example 2:\u00a0Using Displacement of Water to Determine Density<\/h3>\r\nThis <a href=\"https:\/\/phet.colorado.edu\/sims\/density-and-buoyancy\/density_en.html\" target=\"_blank\" rel=\"noopener noreferrer\">PhET simulation<\/a> illustrates another way to determine density, using displacement of water. Determine the density of the red and yellow blocks.\r\n\r\n[reveal-answer q=\"573648\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"573648\"]\r\n\r\nWhen you open the density simulation and select Same Mass, you can choose from several 5.00-kg colored blocks that you can drop into a tank containing 100.00 L water. The yellow block floats (it is less dense than water), and the water level rises to 105.00 L. While floating, the yellow block displaces 5.00 L water, an amount equal to the weight of the block. The red block sinks (it is more dense than water, which has density = 1.00 kg\/L), and the water level rises to 101.25 L.\r\n\r\nThe red block therefore displaces 1.25 L water, an amount equal to the volume of the block. The density of the red block is:\r\n\r\n[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{\\text{5.00 kg}}{\\text{1.25 L}}=4.00 kg\/L[\/latex]\r\n\r\nNote that since the yellow block is not completely submerged, you cannot determine its density from this information. But if you hold the yellow block on the bottom of the tank, the water level rises to 110.00 L, which means that it now displaces 10.00 L water, and its density can be found:\r\n\r\n[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{\\text{5.00 kg}}{10.00 L}=\\text{0.500 kg\/L}[\/latex]\r\n\r\n[\/hidden-answer]\r\n<h4>Check Your Learning<\/h4>\r\nRemove all of the blocks from the water and add the green block to the tank of water, placing it approximately in the middle of the tank. Determine the density of the green block.\r\n\r\n[reveal-answer q=\"422855\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"422855\"]2.00 kg\/L[\/hidden-answer]\r\n\r\n<\/div>\r\n<p id=\"ball-ch02_s05_p15\" class=\"para editable block\">Because of how it is defined, density can act as a conversion factor for switching between units of mass and volume. For example, suppose you have a sample of aluminum that has a volume of 7.88 cm<sup class=\"superscript\">3<\/sup>. How can you determine what mass of aluminum you have without measuring it? You can use the volume to calculate it. If you multiply the given volume by the known density (2.7 g\/cm<sup>3<\/sup>), the volume units will cancel and leave you with mass units, telling you the mass of the sample:<\/p>\r\n\r\n<div id=\"ball-ch02_s05\" class=\"section\" lang=\"en\">\r\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large 7.88\\cancel{{ cm^{3}}}\\times\\frac{2.7{\\text{ g}}}{1\\cancel{cm^{3}}}=21\\text{ g of Al}[\/latex]<\/span><\/p>\r\n<p id=\"ball-ch02_s05_p17\" class=\"para editable block\">where we have limited our answer to two significant figures.<\/p>\r\n\r\n<div class=\"textbox examples\">\r\n<h3>Example 3:\u00a0 Using Density as a Conversion factor<strong>\r\n<\/strong><\/h3>\r\nWhat is the mass of 44.6 mL of mercury? Mercury has a density of 13.6 g\/mL.\r\n\r\n[reveal-answer q=\"798794\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798794\"]\r\n\r\n<span class=\"informalequation block\">[latex]\\large 44.6\\cancel{ mL}\\times\\frac{13.6{\\text{ g}}}{1\\cancel{ mL}}=607 \\text{ g of Hg}[\/latex]<\/span>\r\n\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nWhat is the mass of 25.0 cm<sup class=\"superscript\">3<\/sup> of iron? Density of iron can be found in Table 1.\r\n\r\n[reveal-answer q=\"798795\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798795\"]197 g Fe[\/hidden-answer]\r\n\r\n<\/div>\r\n<p id=\"ball-ch02_s05_p23\" class=\"para editable block\">Density can also be used as a conversion factor to convert mass to volume\u2014but care must be taken. We have already demonstrated that the number that goes with density normally goes in the numerator when density is written as a fraction. Take the density of gold, for example:<\/p>\r\n<p style=\"text-align: center;\">[latex]\\large \\text{density of Au} =19.3\\text{ g\/mL}=\\frac{19.3{\\text{ g}}}{1\\text{ mL}}[\/latex]<\/p>\r\nThat is, the density value tells us that we have 19.3 grams for every 1 milliliter of volume, and the 1 is an exact number. When we want to use density to convert from mass to volume, the numerator and denominator of density need to be switched. For example, if we want to know the volume of 45.9 g of gold, we would set up the conversion as follows:\r\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large 45.9\\cancel{ g}\\times\\frac{1{\\text{ mL}}}{19.3\\cancel{ g}}=2.38\\text{ mL of Au}[\/latex]<\/span><\/p>\r\n<p id=\"ball-ch02_s05_p27\" class=\"para editable block\">Note how the mass units cancel, leaving the volume unit, which is what we\u2019re looking for.<\/p>\r\n\r\n<div class=\"textbox examples\">\r\n<h3>Example 4: Using Density as a Conversion factor<\/h3>\r\nA cork stopper from a bottle of wine has a mass of 3.78 g. If the density of cork is 0.22 g\/mL, what is the volume (in mL) of the cork?\r\n\r\n[reveal-answer q=\"798796\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798796\"]\r\n\r\n<span class=\"informalequation block\">[latex]\\large 3.78\\cancel{ g}\\times\\frac{1{\\text{ mL}}}{0.22\\cancel{ g}}=17.2\\text{ mL}[\/latex]<\/span>\r\n\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nWhat is the volume (in mL) of 3.78 g of glycerin? Density of glycerin can be found in Table 1.\r\n\r\n[reveal-answer q=\"798797\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798797\"]3.00 mL[\/hidden-answer]\r\n\r\n<\/div>\r\n<p id=\"ball-ch02_s05_p33\" class=\"para editable block\">Care must be used with density as a conversion factor. Make sure the mass units are the same, or the volume units are the same, before using density to convert to a different unit. Often, the unit of the given quantity must be first converted to the appropriate unit before applying density as a conversion factor (see Example 7).<\/p>\r\n\r\n<div class=\"textbox examples\">\r\n<h3>Example 5: Using Density as a Conversion factor<\/h3>\r\nAcetone has a density of 0.79 g\/mL, what is the volume (in L) of the 25.0 g of acetone?\u00a0 Hint: 1 L = 10<sup>3<\/sup> mL\r\n\r\n[reveal-answer q=\"79879226\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"79879226\"]\r\n<div id=\"q79879226\" class=\"hidden-answer\">\r\n\r\n<span class=\"informalequation block\"><span class=\"CCbrackets underline\">We start with what is given, 25.0 g and use the density to convert grams to mL, making sure the 0.79 g is in the denominator. Next we convert to L by using 1 L = 10<sup>3<\/sup> mL as a conversion factor.\r\n[latex]\\large 25.0\\cancel{ g}\\times\\frac{1{\\cancel{ mL}}}{0.79\\cancel{ g}}\\times\\frac{1\\text{ L}}{10^{3}\\cancel{ mL}}=0.032\\text{ mL}[\/latex]<\/span><\/span>\r\n\r\nThe final answer requires two significant figures because the density used (0.79 g\/mL).\r\n\r\n<\/div>\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nWhat is the mass (in grams) of 0.050 L of olive oil? Density of olive oil can be found in Table 1. (1 L = 10<sup>3<\/sup> mL)\r\n\r\n[reveal-answer q=\"798797\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798797\"]46 g[\/hidden-answer]\r\n\r\n<\/div>\r\n<div id=\"ball-ch02_s05_n06\" class=\"callout block\">\r\n<h3>Measurement of Temperature (temperature scales)<\/h3>\r\nThere are other units in chemistry that are important, and we will cover others in the course of the entire book. One of the fundamental quantities in science is temperature.<strong> Temperature<\/strong> is a measure of the average amount of energy of motion, or <em class=\"emphasis\">kinetic energy<\/em>, a system contains. Temperatures are expressed using scales that use units called <strong>degrees<\/strong>, and there are several temperature scales in use. In the United States, the commonly used temperature scale is the <em class=\"emphasis\">Fahrenheit scale<\/em> (symbolized by \u00b0F and spoken as \u201cdegrees Fahrenheit\u201d). On this scale, the freezing point of liquid water (the temperature at which liquid water turns to solid ice) is 32 \u00b0F, and the boiling point of water (the temperature at which liquid water turns to steam) is 212 \u00b0F.\r\n<p id=\"ball-ch02_s05_p02\" class=\"para editable block\">Science also uses other scales to express temperature. The Celsius scale (symbolized by \u00b0C and spoken as \u201cdegrees Celsius\u201d) is a temperature scale where 0 \u00b0C is the freezing point of water and 100 \u00b0C is the boiling point of water; the scale is divided into 100 divisions between these two landmarks and extended higher and lower. By comparing the Fahrenheit and Celsius scales, a conversion between the two scales can be determined:<\/p>\r\n<p style=\"text-align: center;\">[latex]\\large ^{o}C =(^{o}F-32)\\times\\frac{5}{9}[\/latex]\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [latex]\\large ^{o}F =(^{o}C\\times\\frac{9}{5})+ 32[\/latex]<\/p>\r\n<p id=\"ball-ch02_s05_p03\" class=\"para editable block\">Using these formulas, we can convert from one temperature scale to another. The number 32 in the formulas is exact and does not count in significant figure determination.<\/p>\r\n\r\n<div class=\"textbox examples\">\r\n<h3>Example 6: Celsius\/Fahrenheit temperature Conversions<strong>\r\n<\/strong><\/h3>\r\n1. T<span class=\"st\">he average internal temperature of a human is 98.6 <em>\u00b0<\/em>F. What is this temperature in <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C?<\/span>\r\n\r\n2. Room temperature is typically considered to be 25.0 \u00b0C. What is this temperature in \u00b0F?\r\n\r\n[reveal-answer q=\"798792\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798792\"]\r\n\r\n1. [latex]\\large ^{o}C =(98.6 - 32)\\times\\frac{5}{9}= 37.0\\ ^{o}C[\/latex]\r\n\r\n2. [latex]\\large ^{o}F =(25.0\\times\\frac{9}{5})+ 32= 77.0\\ ^{o}F[\/latex]\r\n\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\n1. The average temperature during the month of January at the summit of Mount Everest is -36 <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C. <span class=\"ui_qtext_rendered_qtext\">What is this temperature in\u00a0\u00b0F?<\/span>\r\n\r\n2. The warmest month for Rochester, New York is July with an average high temperature of 83.2 \u00b0F. <span class=\"st\">What is this temperature in <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C?<\/span>\r\n\r\n[reveal-answer q=\"798791\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798791\"] 1. -33 <span class=\"ui_qtext_rendered_qtext\">\u00b0F, 2. 28.4 <span class=\"st\">\u00b0C<\/span><\/span>[\/hidden-answer]\r\n\r\n<\/div>\r\n<p id=\"ball-ch02_s05_p04\" class=\"para editable block\">The fundamental unit of temperature (another fundamental unit of science, bringing us to four) in SI is the <strong>Kelvin<\/strong> (K). The Kelvin temperature scale (note that the name of the scale capitalizes the word <em class=\"emphasis\">Kelvin<\/em>, but the unit itself is lowercase) uses degrees that are the same size as the Celsius degree, but the numerical scale is shifted up by 273.15 units. That is, the conversion between the Kelvin and Celsius scales is as follows:<\/p>\r\n<p style=\"text-align: center;\">[latex]\\large K =\\ ^{o}C + 273.15[\/latex]\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [latex]\\large \\ ^{o}C =K - 273.15[\/latex]<\/p>\r\n<p id=\"ball-ch02_s05_p05\" class=\"para editable block\">For most purposes, it is acceptable to use 273 instead of 273.15. Note that the Kelvin scale does not use the word <em class=\"emphasis\">degrees<\/em>; a temperature of 295 K is spoken of as \u201ctwo hundred ninety-five kelvins\u201d and not \u201ctwo hundred ninety-five degrees Kelvin.\u201d<\/p>\r\n<p id=\"ball-ch02_s05_p06\" class=\"para editable block\">The reason that the Kelvin scale is defined this way is because there exists a minimum possible temperature called <strong>absolute zero<\/strong>. The Kelvin temperature scale is set so that 0 K is absolute zero, and temperature is counted upward from there. Normal room temperature is about 295 K, as seen in the following example.<\/p>\r\n\r\n<div class=\"textbox examples\">\r\n<h3>Example 7: Celsius\/Kelvin Temperature conversions<strong>\r\n<\/strong><\/h3>\r\nIn Denver, Colorado which has an elevation of approximately 1 mile, water boils at about 95 <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C.\u00a0 What is this temperature in Kelvin?\r\n\r\n[reveal-answer q=\"798793\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"798793\"]\r\n\r\n[latex]\\large K =95 + 273.15 = 368 K[\/latex]\r\n<p id=\"ball-ch02_s05_p13\" class=\"para editable block\">[\/hidden-answer]<\/p>\r\n\r\n<\/div>\r\n<p class=\"para editable block\">Figure 1. compares the three temperature scales. Note that science uses the Celsius and Kelvin scales almost exclusively; virtually no practicing chemist expresses laboratory-measured temperatures with the Fahrenheit scale. (In fact, the United States is one of the few countries in the world that still uses the Fahrenheit scale on a daily basis. The other two countries are Liberia and Myanmar [formerly Burma].<\/p>\r\n\r\n<div id=\"ball-ch02_s05_f01\" class=\"figure large editable block\">\r\n<p class=\"title\"><span class=\"title-prefix\">\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 Figure 1. <\/span>Fahrenheit, Celsius, and Kelvin Temperatures<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Temperatures.png\"><img class=\"aligncenter wp-image-4622\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14212527\/Temperatures-1.png\" alt=\"Temperatures\" width=\"444\" height=\"394\" \/><\/a><\/p>\r\n\r\n<\/div>\r\n<h3 class=\"title\">Food and Drink App: Cooking Temperatures<\/h3>\r\n<p id=\"ball-ch02_s05_p78\" class=\"para\">Because degrees Fahrenheit is the common temperature scale in the United States, kitchen appliances, such as ovens, are calibrated in that scale. A cool oven may be only 150\u00b0F, while a cake may be baked at 350\u00b0F and a chicken roasted at 400\u00b0F. The broil setting on many ovens is 500\u00b0F, which is typically the highest temperature setting on a household oven.<\/p>\r\n<p id=\"ball-ch02_s05_p79\" class=\"para\">People who live at high altitudes, typically 2,000 ft above sea level or higher, are sometimes urged to use slightly different cooking instructions on some products, such as cakes and bread, because water boils at a lower temperature the higher in altitude you go, meaning that foods cook slower. For example, in Cleveland water typically boils at 212\u00b0F (100\u00b0C), but in Denver, the Mile-High City, water boils at about 200\u00b0F (93.3\u00b0C), which can significantly lengthen cooking times. Good cooks need to be aware of this.<\/p>\r\n<p id=\"ball-ch02_s05_p80\" class=\"para\">At the other end is pressure cooking. A pressure cooker is a closed vessel that allows steam to build up additional pressure, which increases the temperature at which water boils. A good pressure cooker can get to temperatures as high as 252\u00b0F (122\u00b0C); at these temperatures, food cooks much faster than it normally would. Great care must be used with pressure cookers because of the high pressure and high temperature. (When a pressure cooker is used to sterilize medical instruments, it is called an <em class=\"emphasis\">autoclave<\/em>.)<\/p>\r\n<p id=\"ball-ch02_s05_p81\" class=\"para\">Other countries use the Celsius scale for everyday purposes. Therefore, oven dials in their kitchens are marked in degrees Celsius. It can be confusing for US cooks to use ovens abroad\u2014a 425\u00b0F oven in the United States is equivalent to a 220\u00b0C oven in other countries. These days, many oven thermometers are marked with both temperature scales.<\/p>\r\n\r\n<div id=\"ball-ch02_s05_qs01\" class=\"qandaset block\">\r\n<div class=\"bcc-box bcc-success\">\r\n<h3>Key Takeaways<\/h3>\r\n<ul id=\"ball-ch02_s05_l06\" class=\"itemizedlist\">\r\n \t<li>Density relates a substance\u2019s mass and volume.<\/li>\r\n \t<li>Density is a derived unit and can be used as a conversion factor to calculate volume from a given mass or mass from a given volume.<\/li>\r\n \t<li>Chemistry uses the Celsius and Kelvin scales to express temperatures.<\/li>\r\n \t<li>A temperature on the Kelvin scale is the Celsius temperature plus 273.15.<\/li>\r\n \t<li>The minimum possible temperature is absolute zero and is assigned 0 K on the Kelvin scale.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercise<\/h3>\r\n<strong>Calculating Density from Experimental Results<\/strong>\r\n<div class=\"question\">\r\n<ol>\r\n \t<li id=\"ball-ch02_s05_qs01_p13\" class=\"para\">The length, height, and width of an unknown block of metal was found to be 4.53 cm by 13.62 cm by 6.00 cm.\u00a0 The mass of the block was determined to be 3.330 \u00d7 10<sup class=\"superscript\">3<\/sup> g.\u00a0 Determine the density of the block and identify the metal using Table 1.<\/li>\r\n \t<li id=\"ball-ch02_s05_qs01_p13\" class=\"para\">An unknown metal is weighed in a 150 mL beaker, giving a total mass of 125.476 g.\u00a0 The mass of the empty beaker was 61.439 g. The metal was then placed into a graduated cylinder with an initial volume of 26.5 mL.\u00a0 The volume was displaced to give a final volume of 29.8 mL.\u00a0 Determine the density of the unknown metal and identify the metal using Table 1.<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"79879888\"]Show Answers to Select Questions[\/reveal-answer]\r\n[hidden-answer a=\"79879888\"]\r\n<ol>\r\n \t<li>volume of block = 4.53 cm \u00d7 13.62 cm \u00d7 6.00 cm = 370. cm<sup>3<\/sup>. Density = [latex]\\frac{\\text{3.33}\\times10^{3}\\text{ }\\text{g}}{\\text{370. }cm^{3}}=\\text{9.00} \\text{ g}\/cm^{3}[\/latex]. The metal appears to be copper (Cu).<\/li>\r\n \t<li>The mass of the unknown metal is 64.037 g (calculated by subtracting the mass of the empty beaker from the total mass).\u00a0 The volume is 3.3 mL (subtracting the initial volume from the final displaced volume.\u00a0 Density = [latex]\\frac{\\text{64.037}\\text{g}}{\\text{3.3}\\text{ mL}}=\\text{19} \\text{ g\/mL}[\/latex]. The metal appears to be gold (Au).<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"question\">\r\n\r\n[\/hidden-answer]\r\n\r\n<strong>Using Density as a Conversion Factor<\/strong>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<ol>\r\n \t<li class=\"para\">A sample of iron has a volume of 48.2 cm<sup class=\"superscript\">3<\/sup>. What is its mass (in grams)?<\/li>\r\n \t<li>The volume of an Olympic-sized swimming pool is 2.50 \u00d7 10<sup class=\"superscript\">9<\/sup> cm<sup class=\"superscript\">3<\/sup>. If the pool is filled with alcohol (<em class=\"emphasis\">d<\/em> = 0.789 g\/cm<sup class=\"superscript\">3<\/sup>), what mass (in grams) of alcohol is in the pool?<\/li>\r\n \t<li>Neon, a Noble gas, is commonly used in signs. What is the volume in liters of 222 g of neon if neon has a density of 0.900 g\/L?<\/li>\r\n \t<li>What is the volume in cubic centimeters of 100.0 g of lead if lead has a density of 11.34 g\/cm<sup class=\"superscript\">3<\/sup>?<\/li>\r\n \t<li>A sample of air has a volume of 1,015 mL. What is its mass (in grams)?<\/li>\r\n \t<li class=\"para\">The volume of hydrogen used by the <em class=\"emphasis\">Hindenburg<\/em>, the German airship that exploded in New Jersey in 1937, was 2.000 \u00d7 10<sup class=\"superscript\">8<\/sup> L. If hydrogen gas has a density of 0.0899 g\/L, what mass in kilograms of hydrogen was used by the airship?<\/li>\r\n \t<li>The gas tank of a Reliant Robin automobile holds 7.1 gallons according to the owner\u2019s manual. If the density of gasoline is 0.8206 g\/mL, determine the mass of the fuel in a full tank in pounds.<\/li>\r\n \t<li class=\"para\">A typical engagement ring has 0.77 cm<sup class=\"superscript\">3<\/sup> of gold. What mass (in ounces) of gold is present?<\/li>\r\n \t<li>The density of orange juice is 1.05 g\/mL, what is the volume (in pints) of 9.91 \u00d7 10<sup class=\"superscript\">5<\/sup> mg of juice?<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"798798\"]Show Answers to Select Questions[\/reveal-answer]\r\n[hidden-answer a=\"798798\"]\r\n<ol>\r\n \t<li>\u00a0[latex]\\text{48.2 }\\cancel{cm^{3}}\\times\\frac{\\text{7.9 }\\text{g}}{\\text{ 1 }\\cancel{cm^{3}}}=\\text{ 381}\\text{ g}[\/latex]<\/li>\r\n \t<li>[latex]2.50\\times10^{9}\\text{ }\\cancel{cm^3}\\times\\frac{\\text{0.789}\\text{ g}}{\\text{1 }\\cancel{cm^3}}=\\text{1.97 }\\times10^{9}\\text{ g}[\/latex]<\/li>\r\n \t<li>[latex]\\text{222 }\\cancel{\\text{g}}\\times\\frac{\\text{1 }\\text{L}}{\\text{0.900 }\\cancel{\\text{g}}}=\\text{2.47 }\\times10^{2}\\text{ L}[\/latex]<\/li>\r\n \t<li>[latex]\\text{100.0}\\times\\cancel{\\text{g}}\\times\\frac{\\text{1 } cm^3}{\\text{11.34 }\\cancel{\\text{g}}}=\\text{8.818 }cm^3[\/latex]<\/li>\r\n \t<li>[latex]\\text{1015 }\\cancel{\\text{mL}}\\times\\frac{10^{-3}\\text{ }\\cancel{\\text{L}}}{\\text{ 1 }\\cancel{\\text{mL}}}\\times\\frac{\\text{1.20 }\\text{g}}{\\text{ 1 }\\cancel{\\text{L}}}=\\text{1.2 }\\text{ g}[\/latex]<\/li>\r\n \t<li>[latex]2.000\\times10^{8}\\text{ }\\cancel{\\text{L}}\\times\\frac{\\text{0.0899}\\cancel{\\text{ g}}}{\\text{1 }\\cancel{\\text{L}}}\\times\\frac{\\text{1 }\\text{kg}}{10^{3}\\text{ }\\cancel{\\text{g}}}=\\text{1.80 }\\times10^{4}\\text{ kg}[\/latex]<\/li>\r\n \t<li>[latex]\\text{ 7.1 }\\cancel{\\text{gal}}\\times\\frac{\\text{3.785 }\\cancel{\\text{L}}}{\\text{1 }\\cancel{\\text{gal}}}\\times\\frac{\\text{1 }\\cancel{\\text{mL}}}{10^{-3}\\text{ }\\cancel{\\text{L}}}\\times\\frac{\\text{0.8206 }\\cancel{\\text{g}}}{\\text{1 }\\cancel{\\text{mL}}}\\times\\frac{\\text{1 }\\text{lb}}{\\text{453.59 }\\cancel{\\text{g}}}=\\text{49 lb}[\/latex]<\/li>\r\n \t<li>[latex]\\text{0.77 }\\cancel{cm^{3}}\\times\\frac{\\text{19.3 }\\cancel{\\text{g}}}{\\text{ 1 }\\cancel{cm^{3}}}\\times\\frac{\\text{1 }\\text{oz}}{\\text{28.35 }\\cancel{\\text{g}}}=\\text{0.52}\\text{ oz}[\/latex]<\/li>\r\n \t<li>[latex]\\text{9.91}\\times10^5\\text{ }\\cancel{\\text{mg}}\\times\\frac{10^{-3}\\text{ }\\cancel{\\text{g}}}{\\text{1 }\\cancel{\\text{mg}}}\\times\\frac{\\text{1 }\\cancel{\\text{mL}}}{\\text{1.05 }\\cancel{\\text{g}}}\\times\\frac{\\text{1 }\\text{pt}}{\\text{473.2 }\\cancel{\\text{mL}}}=\\text{1.99 pt}[\/latex]<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"question\">\r\n\r\n[\/hidden-answer]\r\n<div class=\"question\">\r\n\r\n<strong>Converting Units of Temperature\r\n<\/strong>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<ol>\r\n \t<li class=\"para\">Convert 255\u00b0F to degrees Celsius<\/li>\r\n \t<li class=\"para\">Convert\u2212255\u00b0F to degrees Celsius<\/li>\r\n \t<li class=\"para\">Convert 50.0\u00b0C to degrees Fahrenheit<\/li>\r\n \t<li class=\"para\">Convert \u221250.0\u00b0C to degrees Fahrenheit<\/li>\r\n \t<li class=\"para\">Convert 0 K to degrees Celsius. What is the significance of the temperature in degrees Celsius?<\/li>\r\n \t<li class=\"para\">The hottest temperature ever recorded on the surface of the earth was 136\u00b0F in Libya in 1922. What is the temperature in degrees Celsius and in kelvins?<\/li>\r\n \t<li class=\"para\">The coldest temperature ever recorded on the surface of the earth was \u2212128.6\u00b0F in Vostok, Antarctica, in 1983. What is the temperature in degrees Celsius and in kelvins?<\/li>\r\n<\/ol>\r\n<div class=\"question\">\r\n\r\n[reveal-answer q=\"798798881\"]Show Answers to Select Questions[\/reveal-answer]\r\n[hidden-answer a=\"798798881\"]\r\n<div class=\"question\">\r\n<ol>\r\n \t<li>\u00a0124\u00b0C<\/li>\r\n \t<li>\u2212159\u00b0C<\/li>\r\n \t<li>122\u00b0F<\/li>\r\n \t<li>\u221258\u00b0F<\/li>\r\n \t<li>\u2212273\u00b0C. This is the lowest possible temperature in degrees Celsius.<\/li>\r\n \t<li>57.8\u00b0C; 331 K<\/li>\r\n \t<li>\u221289.2\u00b0C; 184 K<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<div class=\"question\">\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div id=\"ball-ch02_s05\" class=\"section\" lang=\"en\">\n<div id=\"ball-ch02_s05_n01\" class=\"learning_objectives editable block\">\n<div class=\"bcc-box bcc-highlight\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Define density.<\/li>\n<li>Calculate density from experimental results.<\/li>\n<li>Use density as a conversion factor.<\/li>\n<li>Learn about the various temperature scales that are commonly used in chemistry.<\/li>\n<li>Convert units of temperature<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n<h3>Density<\/h3>\n<p>We use the mass and volume of a substance to determine its density. Thus, the units of density are defined by the base units of mass and length.<\/p>\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large Density = \\frac{mass}{volume}[\/latex]<\/span><\/p>\n<p>The <strong>density<\/strong> of a substance is the ratio of the mass of a sample of the substance to its volume. The SI unit for density is the kilogram per cubic meter (kg\/m<sup>3<\/sup>). For many situations, however, this as an inconvenient unit, and we often use grams per cubic centimeter (g\/cm<sup>3<\/sup>) for the densities of solids and liquids, and grams per liter (g\/L) for gases. Common units for density include g\/mL, g\/cm<sup class=\"superscript\">3<\/sup>, g\/L, or kg\/L. Although there are exceptions, most liquids and solids have densities that range from about 0.7 g\/mL (the density of gasoline) to 19 g\/mL (the density of gold). The density of air is about 1.2 g\/L. Table 1 shows the densities of some common substances.<\/p>\n<table summary=\"This table reports the density of solids, liquids, and gases in grams per centimeters cubed. The values for solids are ice 0.92, oak wood 0.60 to 0.90, iron 7.9, copper 9.0, lead 11.3, silver 10.5, and gold 19.3. The values for liquids are water 1.0, ethanol 0.79, acetone 0.79, glycerin 1.26, olive oil 0.92, gasoline 0.70 to 0.77, and Mercury 13.6. The values for gases, which were measured when the gas was at 25 degrees Celsius and 1 atmosphere, are dry air 1.20, oxygen 1.31, nitrogen 1.14, carbon dioxide 1.80, helium 0.16, neon 0.83, and radon 9.1.\">\n<thead>\n<tr>\n<th style=\"text-align: center;\" colspan=\"3\">Table 1. Densities of Common Substances<\/th>\n<\/tr>\n<tr valign=\"top\">\n<th style=\"text-align: center;\">Solids<\/th>\n<th style=\"text-align: center;\">Liquids<\/th>\n<th style=\"text-align: center;\">Gases (at 25 \u00b0C and 1 atm)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">ice (at 0 \u00b0C) 0.92 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">water 1.0 g\/mL<\/td>\n<td style=\"text-align: center;\">dry air 1.20 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">oak (wood) 0.60\u20130.90 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">ethanol 0.79 g\/mL<\/td>\n<td style=\"text-align: center;\">oxygen 1.31 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">iron 7.9 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">acetone 0.79 g\/mL<\/td>\n<td style=\"text-align: center;\">nitrogen 1.14 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">copper 9.0 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">glycerin 1.26 g\/mL<\/td>\n<td style=\"text-align: center;\">carbon dioxide 1.80 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">lead 11.3 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">olive oil 0.92 g\/mL<\/td>\n<td style=\"text-align: center;\">helium 0.16 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">silver 10.5 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">gasoline 0.70\u20130.77 g\/mL<\/td>\n<td style=\"text-align: center;\">neon 0.83 g\/L<\/td>\n<\/tr>\n<tr valign=\"top\">\n<td style=\"text-align: center;\">gold 19.3 g\/cm<sup>3<\/sup><\/td>\n<td style=\"text-align: center;\">mercury 13.6 g\/mL<\/td>\n<td style=\"text-align: center;\">radon 9.1 g\/L<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>While there are many ways to determine the density of an object, perhaps the most straightforward method involves separately finding the mass and volume of the object, and then dividing the mass of the sample by its volume. In the following example, the mass is found directly by weighing, but the volume is found indirectly through length measurements.<\/p>\n<div class=\"textbox examples\">\n<h3>Example 1:\u00a0Calculation of Density<\/h3>\n<p>Gold\u2014in bricks, bars, and coins\u2014has been a form of currency for centuries. In order to swindle people into paying for a brick of gold without actually investing in a brick of gold, people have considered filling the centers of hollow gold bricks with lead to fool buyers into thinking that the entire brick is gold. It does not work: Lead is a dense substance, but its density is not as great as that of gold, 19.3 g\/cm<sup>3<\/sup>. What is the density of lead if a cube of lead has an edge length of 2.00 cm and a mass of 90.7 g?<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q528993\">Show Answer<\/span><\/p>\n<div id=\"q528993\" class=\"hidden-answer\" style=\"display: none\">\n<p>The density of a substance can be calculated by dividing its mass by its volume. The volume of a cube is calculated by cubing the edge length.<\/p>\n<p>[latex]\\large\\text{volume of lead cube}=2.00\\text{ cm}\\times 2.00\\text{ cm}\\times 2.00\\text{ cm}={8.00\\text{ cm}}^{3}[\/latex]<\/p>\n<p>[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{90.7\\text{g}}{{8.00\\text{ cm}}^{3}}=\\frac{11.3\\text{g}}{{1.00\\text{ cm}}^{3}}={11.3\\text{g\/cm}}^{3}[\/latex]<\/p>\n<p>(We will discuss the reason for rounding to the first decimal place in the next section.)<\/p>\n<\/div>\n<\/div>\n<h4>Check Your Learning<\/h4>\n<ol>\n<li>To three decimal places, what is the volume of a cube (cm<sup>3<\/sup>) with an edge length of 0.843 cm?<\/li>\n<li>If the cube in part 1 is copper and has a mass of 5.34 g, what is the density of copper to two decimal places?<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q513756\">Show Answer<\/span><\/p>\n<div id=\"q513756\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>0.599 cm<sup>3<\/sup><\/li>\n<li>8.91 g\/cm<sup>3<\/sup><\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox\">To learn more about the relationship between mass, volume, and density, use this <a href=\"https:\/\/phet.colorado.edu\/sims\/density-and-buoyancy\/density_en.html\" target=\"_blank\" rel=\"noopener noreferrer\">PhET Density Simulator<\/a>\u00a0to explore the density of different materials, like wood, ice, brick, and aluminum.<\/div>\n<div class=\"textbox examples\">\n<h3>Example 2:\u00a0Using Displacement of Water to Determine Density<\/h3>\n<p>This <a href=\"https:\/\/phet.colorado.edu\/sims\/density-and-buoyancy\/density_en.html\" target=\"_blank\" rel=\"noopener noreferrer\">PhET simulation<\/a> illustrates another way to determine density, using displacement of water. Determine the density of the red and yellow blocks.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q573648\">Show Answer<\/span><\/p>\n<div id=\"q573648\" class=\"hidden-answer\" style=\"display: none\">\n<p>When you open the density simulation and select Same Mass, you can choose from several 5.00-kg colored blocks that you can drop into a tank containing 100.00 L water. The yellow block floats (it is less dense than water), and the water level rises to 105.00 L. While floating, the yellow block displaces 5.00 L water, an amount equal to the weight of the block. The red block sinks (it is more dense than water, which has density = 1.00 kg\/L), and the water level rises to 101.25 L.<\/p>\n<p>The red block therefore displaces 1.25 L water, an amount equal to the volume of the block. The density of the red block is:<\/p>\n<p>[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{\\text{5.00 kg}}{\\text{1.25 L}}=4.00 kg\/L[\/latex]<\/p>\n<p>Note that since the yellow block is not completely submerged, you cannot determine its density from this information. But if you hold the yellow block on the bottom of the tank, the water level rises to 110.00 L, which means that it now displaces 10.00 L water, and its density can be found:<\/p>\n<p>[latex]\\large\\text{density}=\\frac{\\text{mass}}{\\text{volume}}=\\frac{\\text{5.00 kg}}{10.00 L}=\\text{0.500 kg\/L}[\/latex]<\/p>\n<\/div>\n<\/div>\n<h4>Check Your Learning<\/h4>\n<p>Remove all of the blocks from the water and add the green block to the tank of water, placing it approximately in the middle of the tank. Determine the density of the green block.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q422855\">Show Answer<\/span><\/p>\n<div id=\"q422855\" class=\"hidden-answer\" style=\"display: none\">2.00 kg\/L<\/div>\n<\/div>\n<\/div>\n<p id=\"ball-ch02_s05_p15\" class=\"para editable block\">Because of how it is defined, density can act as a conversion factor for switching between units of mass and volume. For example, suppose you have a sample of aluminum that has a volume of 7.88 cm<sup class=\"superscript\">3<\/sup>. How can you determine what mass of aluminum you have without measuring it? You can use the volume to calculate it. If you multiply the given volume by the known density (2.7 g\/cm<sup>3<\/sup>), the volume units will cancel and leave you with mass units, telling you the mass of the sample:<\/p>\n<div id=\"ball-ch02_s05\" class=\"section\" lang=\"en\">\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large 7.88\\cancel{{ cm^{3}}}\\times\\frac{2.7{\\text{ g}}}{1\\cancel{cm^{3}}}=21\\text{ g of Al}[\/latex]<\/span><\/p>\n<p id=\"ball-ch02_s05_p17\" class=\"para editable block\">where we have limited our answer to two significant figures.<\/p>\n<div class=\"textbox examples\">\n<h3>Example 3:\u00a0 Using Density as a Conversion factor<strong><br \/>\n<\/strong><\/h3>\n<p>What is the mass of 44.6 mL of mercury? Mercury has a density of 13.6 g\/mL.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798794\">Show Answer<\/span><\/p>\n<div id=\"q798794\" class=\"hidden-answer\" style=\"display: none\">\n<p><span class=\"informalequation block\">[latex]\\large 44.6\\cancel{ mL}\\times\\frac{13.6{\\text{ g}}}{1\\cancel{ mL}}=607 \\text{ g of Hg}[\/latex]<\/span><\/p>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>What is the mass of 25.0 cm<sup class=\"superscript\">3<\/sup> of iron? Density of iron can be found in Table 1.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798795\">Show Answer<\/span><\/p>\n<div id=\"q798795\" class=\"hidden-answer\" style=\"display: none\">197 g Fe<\/div>\n<\/div>\n<\/div>\n<p id=\"ball-ch02_s05_p23\" class=\"para editable block\">Density can also be used as a conversion factor to convert mass to volume\u2014but care must be taken. We have already demonstrated that the number that goes with density normally goes in the numerator when density is written as a fraction. Take the density of gold, for example:<\/p>\n<p style=\"text-align: center;\">[latex]\\large \\text{density of Au} =19.3\\text{ g\/mL}=\\frac{19.3{\\text{ g}}}{1\\text{ mL}}[\/latex]<\/p>\n<p>That is, the density value tells us that we have 19.3 grams for every 1 milliliter of volume, and the 1 is an exact number. When we want to use density to convert from mass to volume, the numerator and denominator of density need to be switched. For example, if we want to know the volume of 45.9 g of gold, we would set up the conversion as follows:<\/p>\n<p style=\"text-align: center;\"><span class=\"informalequation block\">[latex]\\large 45.9\\cancel{ g}\\times\\frac{1{\\text{ mL}}}{19.3\\cancel{ g}}=2.38\\text{ mL of Au}[\/latex]<\/span><\/p>\n<p id=\"ball-ch02_s05_p27\" class=\"para editable block\">Note how the mass units cancel, leaving the volume unit, which is what we\u2019re looking for.<\/p>\n<div class=\"textbox examples\">\n<h3>Example 4: Using Density as a Conversion factor<\/h3>\n<p>A cork stopper from a bottle of wine has a mass of 3.78 g. If the density of cork is 0.22 g\/mL, what is the volume (in mL) of the cork?<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798796\">Show Answer<\/span><\/p>\n<div id=\"q798796\" class=\"hidden-answer\" style=\"display: none\">\n<p><span class=\"informalequation block\">[latex]\\large 3.78\\cancel{ g}\\times\\frac{1{\\text{ mL}}}{0.22\\cancel{ g}}=17.2\\text{ mL}[\/latex]<\/span><\/p>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>What is the volume (in mL) of 3.78 g of glycerin? Density of glycerin can be found in Table 1.<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798797\">Show Answer<\/span><\/p>\n<div id=\"q798797\" class=\"hidden-answer\" style=\"display: none\">3.00 mL<\/div>\n<\/div>\n<\/div>\n<p id=\"ball-ch02_s05_p33\" class=\"para editable block\">Care must be used with density as a conversion factor. Make sure the mass units are the same, or the volume units are the same, before using density to convert to a different unit. Often, the unit of the given quantity must be first converted to the appropriate unit before applying density as a conversion factor (see Example 7).<\/p>\n<div class=\"textbox examples\">\n<h3>Example 5: Using Density as a Conversion factor<\/h3>\n<p>Acetone has a density of 0.79 g\/mL, what is the volume (in L) of the 25.0 g of acetone?\u00a0 Hint: 1 L = 10<sup>3<\/sup> mL<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q79879226\">Show Answer<\/span><\/p>\n<div id=\"q79879226\" class=\"hidden-answer\" style=\"display: none\">\n<div id=\"q79879226\" class=\"hidden-answer\">\n<p><span class=\"informalequation block\"><span class=\"CCbrackets underline\">We start with what is given, 25.0 g and use the density to convert grams to mL, making sure the 0.79 g is in the denominator. Next we convert to L by using 1 L = 10<sup>3<\/sup> mL as a conversion factor.<br \/>\n[latex]\\large 25.0\\cancel{ g}\\times\\frac{1{\\cancel{ mL}}}{0.79\\cancel{ g}}\\times\\frac{1\\text{ L}}{10^{3}\\cancel{ mL}}=0.032\\text{ mL}[\/latex]<\/span><\/span><\/p>\n<p>The final answer requires two significant figures because the density used (0.79 g\/mL).<\/p>\n<\/div>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>What is the mass (in grams) of 0.050 L of olive oil? Density of olive oil can be found in Table 1. (1 L = 10<sup>3<\/sup> mL)<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798797\">Show Answer<\/span><\/p>\n<div id=\"q798797\" class=\"hidden-answer\" style=\"display: none\">46 g<\/div>\n<\/div>\n<\/div>\n<div id=\"ball-ch02_s05_n06\" class=\"callout block\">\n<h3>Measurement of Temperature (temperature scales)<\/h3>\n<p>There are other units in chemistry that are important, and we will cover others in the course of the entire book. One of the fundamental quantities in science is temperature.<strong> Temperature<\/strong> is a measure of the average amount of energy of motion, or <em class=\"emphasis\">kinetic energy<\/em>, a system contains. Temperatures are expressed using scales that use units called <strong>degrees<\/strong>, and there are several temperature scales in use. In the United States, the commonly used temperature scale is the <em class=\"emphasis\">Fahrenheit scale<\/em> (symbolized by \u00b0F and spoken as \u201cdegrees Fahrenheit\u201d). On this scale, the freezing point of liquid water (the temperature at which liquid water turns to solid ice) is 32 \u00b0F, and the boiling point of water (the temperature at which liquid water turns to steam) is 212 \u00b0F.<\/p>\n<p id=\"ball-ch02_s05_p02\" class=\"para editable block\">Science also uses other scales to express temperature. The Celsius scale (symbolized by \u00b0C and spoken as \u201cdegrees Celsius\u201d) is a temperature scale where 0 \u00b0C is the freezing point of water and 100 \u00b0C is the boiling point of water; the scale is divided into 100 divisions between these two landmarks and extended higher and lower. By comparing the Fahrenheit and Celsius scales, a conversion between the two scales can be determined:<\/p>\n<p style=\"text-align: center;\">[latex]\\large ^{o}C =(^{o}F-32)\\times\\frac{5}{9}[\/latex]\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [latex]\\large ^{o}F =(^{o}C\\times\\frac{9}{5})+ 32[\/latex]<\/p>\n<p id=\"ball-ch02_s05_p03\" class=\"para editable block\">Using these formulas, we can convert from one temperature scale to another. The number 32 in the formulas is exact and does not count in significant figure determination.<\/p>\n<div class=\"textbox examples\">\n<h3>Example 6: Celsius\/Fahrenheit temperature Conversions<strong><br \/>\n<\/strong><\/h3>\n<p>1. T<span class=\"st\">he average internal temperature of a human is 98.6 <em>\u00b0<\/em>F. What is this temperature in <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C?<\/span><\/p>\n<p>2. Room temperature is typically considered to be 25.0 \u00b0C. What is this temperature in \u00b0F?<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798792\">Show Answer<\/span><\/p>\n<div id=\"q798792\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. [latex]\\large ^{o}C =(98.6 - 32)\\times\\frac{5}{9}= 37.0\\ ^{o}C[\/latex]<\/p>\n<p>2. [latex]\\large ^{o}F =(25.0\\times\\frac{9}{5})+ 32= 77.0\\ ^{o}F[\/latex]<\/p>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>1. The average temperature during the month of January at the summit of Mount Everest is -36 <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C. <span class=\"ui_qtext_rendered_qtext\">What is this temperature in\u00a0\u00b0F?<\/span><\/p>\n<p>2. The warmest month for Rochester, New York is July with an average high temperature of 83.2 \u00b0F. <span class=\"st\">What is this temperature in <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C?<\/span><\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798791\">Show Answer<\/span><\/p>\n<div id=\"q798791\" class=\"hidden-answer\" style=\"display: none\"> 1. -33 <span class=\"ui_qtext_rendered_qtext\">\u00b0F, 2. 28.4 <span class=\"st\">\u00b0C<\/span><\/span><\/div>\n<\/div>\n<\/div>\n<p id=\"ball-ch02_s05_p04\" class=\"para editable block\">The fundamental unit of temperature (another fundamental unit of science, bringing us to four) in SI is the <strong>Kelvin<\/strong> (K). The Kelvin temperature scale (note that the name of the scale capitalizes the word <em class=\"emphasis\">Kelvin<\/em>, but the unit itself is lowercase) uses degrees that are the same size as the Celsius degree, but the numerical scale is shifted up by 273.15 units. That is, the conversion between the Kelvin and Celsius scales is as follows:<\/p>\n<p style=\"text-align: center;\">[latex]\\large K =\\ ^{o}C + 273.15[\/latex]\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 [latex]\\large \\ ^{o}C =K - 273.15[\/latex]<\/p>\n<p id=\"ball-ch02_s05_p05\" class=\"para editable block\">For most purposes, it is acceptable to use 273 instead of 273.15. Note that the Kelvin scale does not use the word <em class=\"emphasis\">degrees<\/em>; a temperature of 295 K is spoken of as \u201ctwo hundred ninety-five kelvins\u201d and not \u201ctwo hundred ninety-five degrees Kelvin.\u201d<\/p>\n<p id=\"ball-ch02_s05_p06\" class=\"para editable block\">The reason that the Kelvin scale is defined this way is because there exists a minimum possible temperature called <strong>absolute zero<\/strong>. The Kelvin temperature scale is set so that 0 K is absolute zero, and temperature is counted upward from there. Normal room temperature is about 295 K, as seen in the following example.<\/p>\n<div class=\"textbox examples\">\n<h3>Example 7: Celsius\/Kelvin Temperature conversions<strong><br \/>\n<\/strong><\/h3>\n<p>In Denver, Colorado which has an elevation of approximately 1 mile, water boils at about 95 <span class=\"ui_qtext_rendered_qtext\">\u00b0<\/span>C.\u00a0 What is this temperature in Kelvin?<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798793\">Show Answer<\/span><\/p>\n<div id=\"q798793\" class=\"hidden-answer\" style=\"display: none\">\n<p>[latex]\\large K =95 + 273.15 = 368 K[\/latex]<\/p>\n<p id=\"ball-ch02_s05_p13\" class=\"para editable block\"><\/div>\n<\/div>\n<\/div>\n<p class=\"para editable block\">Figure 1. compares the three temperature scales. Note that science uses the Celsius and Kelvin scales almost exclusively; virtually no practicing chemist expresses laboratory-measured temperatures with the Fahrenheit scale. (In fact, the United States is one of the few countries in the world that still uses the Fahrenheit scale on a daily basis. The other two countries are Liberia and Myanmar [formerly Burma].<\/p>\n<div id=\"ball-ch02_s05_f01\" class=\"figure large editable block\">\n<p class=\"title\"><span class=\"title-prefix\">\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 Figure 1. <\/span>Fahrenheit, Celsius, and Kelvin Temperatures<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Temperatures.png\"><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter wp-image-4622\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14212527\/Temperatures-1.png\" alt=\"Temperatures\" width=\"444\" height=\"394\" \/><\/a><\/p>\n<\/div>\n<h3 class=\"title\">Food and Drink App: Cooking Temperatures<\/h3>\n<p id=\"ball-ch02_s05_p78\" class=\"para\">Because degrees Fahrenheit is the common temperature scale in the United States, kitchen appliances, such as ovens, are calibrated in that scale. A cool oven may be only 150\u00b0F, while a cake may be baked at 350\u00b0F and a chicken roasted at 400\u00b0F. The broil setting on many ovens is 500\u00b0F, which is typically the highest temperature setting on a household oven.<\/p>\n<p id=\"ball-ch02_s05_p79\" class=\"para\">People who live at high altitudes, typically 2,000 ft above sea level or higher, are sometimes urged to use slightly different cooking instructions on some products, such as cakes and bread, because water boils at a lower temperature the higher in altitude you go, meaning that foods cook slower. For example, in Cleveland water typically boils at 212\u00b0F (100\u00b0C), but in Denver, the Mile-High City, water boils at about 200\u00b0F (93.3\u00b0C), which can significantly lengthen cooking times. Good cooks need to be aware of this.<\/p>\n<p id=\"ball-ch02_s05_p80\" class=\"para\">At the other end is pressure cooking. A pressure cooker is a closed vessel that allows steam to build up additional pressure, which increases the temperature at which water boils. A good pressure cooker can get to temperatures as high as 252\u00b0F (122\u00b0C); at these temperatures, food cooks much faster than it normally would. Great care must be used with pressure cookers because of the high pressure and high temperature. (When a pressure cooker is used to sterilize medical instruments, it is called an <em class=\"emphasis\">autoclave<\/em>.)<\/p>\n<p id=\"ball-ch02_s05_p81\" class=\"para\">Other countries use the Celsius scale for everyday purposes. Therefore, oven dials in their kitchens are marked in degrees Celsius. It can be confusing for US cooks to use ovens abroad\u2014a 425\u00b0F oven in the United States is equivalent to a 220\u00b0C oven in other countries. These days, many oven thermometers are marked with both temperature scales.<\/p>\n<div id=\"ball-ch02_s05_qs01\" class=\"qandaset block\">\n<div class=\"bcc-box bcc-success\">\n<h3>Key Takeaways<\/h3>\n<ul id=\"ball-ch02_s05_l06\" class=\"itemizedlist\">\n<li>Density relates a substance\u2019s mass and volume.<\/li>\n<li>Density is a derived unit and can be used as a conversion factor to calculate volume from a given mass or mass from a given volume.<\/li>\n<li>Chemistry uses the Celsius and Kelvin scales to express temperatures.<\/li>\n<li>A temperature on the Kelvin scale is the Celsius temperature plus 273.15.<\/li>\n<li>The minimum possible temperature is absolute zero and is assigned 0 K on the Kelvin scale.<\/li>\n<\/ul>\n<\/div>\n<div class=\"bcc-box bcc-info\">\n<h3>Exercise<\/h3>\n<p><strong>Calculating Density from Experimental Results<\/strong><\/p>\n<div class=\"question\">\n<ol>\n<li id=\"ball-ch02_s05_qs01_p13\" class=\"para\">The length, height, and width of an unknown block of metal was found to be 4.53 cm by 13.62 cm by 6.00 cm.\u00a0 The mass of the block was determined to be 3.330 \u00d7 10<sup class=\"superscript\">3<\/sup> g.\u00a0 Determine the density of the block and identify the metal using Table 1.<\/li>\n<li id=\"ball-ch02_s05_qs01_p13\" class=\"para\">An unknown metal is weighed in a 150 mL beaker, giving a total mass of 125.476 g.\u00a0 The mass of the empty beaker was 61.439 g. The metal was then placed into a graduated cylinder with an initial volume of 26.5 mL.\u00a0 The volume was displaced to give a final volume of 29.8 mL.\u00a0 Determine the density of the unknown metal and identify the metal using Table 1.<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q79879888\">Show Answers to Select Questions<\/span><\/p>\n<div id=\"q79879888\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>volume of block = 4.53 cm \u00d7 13.62 cm \u00d7 6.00 cm = 370. cm<sup>3<\/sup>. Density = [latex]\\frac{\\text{3.33}\\times10^{3}\\text{ }\\text{g}}{\\text{370. }cm^{3}}=\\text{9.00} \\text{ g}\/cm^{3}[\/latex]. The metal appears to be copper (Cu).<\/li>\n<li>The mass of the unknown metal is 64.037 g (calculated by subtracting the mass of the empty beaker from the total mass).\u00a0 The volume is 3.3 mL (subtracting the initial volume from the final displaced volume.\u00a0 Density = [latex]\\frac{\\text{64.037}\\text{g}}{\\text{3.3}\\text{ mL}}=\\text{19} \\text{ g\/mL}[\/latex]. The metal appears to be gold (Au).<\/li>\n<\/ol>\n<\/div>\n<div class=\"question\">\n<\/div>\n<\/div>\n<p><strong>Using Density as a Conversion Factor<\/strong><\/p>\n<\/div>\n<div class=\"question\">\n<ol>\n<li class=\"para\">A sample of iron has a volume of 48.2 cm<sup class=\"superscript\">3<\/sup>. What is its mass (in grams)?<\/li>\n<li>The volume of an Olympic-sized swimming pool is 2.50 \u00d7 10<sup class=\"superscript\">9<\/sup> cm<sup class=\"superscript\">3<\/sup>. If the pool is filled with alcohol (<em class=\"emphasis\">d<\/em> = 0.789 g\/cm<sup class=\"superscript\">3<\/sup>), what mass (in grams) of alcohol is in the pool?<\/li>\n<li>Neon, a Noble gas, is commonly used in signs. What is the volume in liters of 222 g of neon if neon has a density of 0.900 g\/L?<\/li>\n<li>What is the volume in cubic centimeters of 100.0 g of lead if lead has a density of 11.34 g\/cm<sup class=\"superscript\">3<\/sup>?<\/li>\n<li>A sample of air has a volume of 1,015 mL. What is its mass (in grams)?<\/li>\n<li class=\"para\">The volume of hydrogen used by the <em class=\"emphasis\">Hindenburg<\/em>, the German airship that exploded in New Jersey in 1937, was 2.000 \u00d7 10<sup class=\"superscript\">8<\/sup> L. If hydrogen gas has a density of 0.0899 g\/L, what mass in kilograms of hydrogen was used by the airship?<\/li>\n<li>The gas tank of a Reliant Robin automobile holds 7.1 gallons according to the owner\u2019s manual. If the density of gasoline is 0.8206 g\/mL, determine the mass of the fuel in a full tank in pounds.<\/li>\n<li class=\"para\">A typical engagement ring has 0.77 cm<sup class=\"superscript\">3<\/sup> of gold. What mass (in ounces) of gold is present?<\/li>\n<li>The density of orange juice is 1.05 g\/mL, what is the volume (in pints) of 9.91 \u00d7 10<sup class=\"superscript\">5<\/sup> mg of juice?<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798798\">Show Answers to Select Questions<\/span><\/p>\n<div id=\"q798798\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>\u00a0[latex]\\text{48.2 }\\cancel{cm^{3}}\\times\\frac{\\text{7.9 }\\text{g}}{\\text{ 1 }\\cancel{cm^{3}}}=\\text{ 381}\\text{ g}[\/latex]<\/li>\n<li>[latex]2.50\\times10^{9}\\text{ }\\cancel{cm^3}\\times\\frac{\\text{0.789}\\text{ g}}{\\text{1 }\\cancel{cm^3}}=\\text{1.97 }\\times10^{9}\\text{ g}[\/latex]<\/li>\n<li>[latex]\\text{222 }\\cancel{\\text{g}}\\times\\frac{\\text{1 }\\text{L}}{\\text{0.900 }\\cancel{\\text{g}}}=\\text{2.47 }\\times10^{2}\\text{ L}[\/latex]<\/li>\n<li>[latex]\\text{100.0}\\times\\cancel{\\text{g}}\\times\\frac{\\text{1 } cm^3}{\\text{11.34 }\\cancel{\\text{g}}}=\\text{8.818 }cm^3[\/latex]<\/li>\n<li>[latex]\\text{1015 }\\cancel{\\text{mL}}\\times\\frac{10^{-3}\\text{ }\\cancel{\\text{L}}}{\\text{ 1 }\\cancel{\\text{mL}}}\\times\\frac{\\text{1.20 }\\text{g}}{\\text{ 1 }\\cancel{\\text{L}}}=\\text{1.2 }\\text{ g}[\/latex]<\/li>\n<li>[latex]2.000\\times10^{8}\\text{ }\\cancel{\\text{L}}\\times\\frac{\\text{0.0899}\\cancel{\\text{ g}}}{\\text{1 }\\cancel{\\text{L}}}\\times\\frac{\\text{1 }\\text{kg}}{10^{3}\\text{ }\\cancel{\\text{g}}}=\\text{1.80 }\\times10^{4}\\text{ kg}[\/latex]<\/li>\n<li>[latex]\\text{ 7.1 }\\cancel{\\text{gal}}\\times\\frac{\\text{3.785 }\\cancel{\\text{L}}}{\\text{1 }\\cancel{\\text{gal}}}\\times\\frac{\\text{1 }\\cancel{\\text{mL}}}{10^{-3}\\text{ }\\cancel{\\text{L}}}\\times\\frac{\\text{0.8206 }\\cancel{\\text{g}}}{\\text{1 }\\cancel{\\text{mL}}}\\times\\frac{\\text{1 }\\text{lb}}{\\text{453.59 }\\cancel{\\text{g}}}=\\text{49 lb}[\/latex]<\/li>\n<li>[latex]\\text{0.77 }\\cancel{cm^{3}}\\times\\frac{\\text{19.3 }\\cancel{\\text{g}}}{\\text{ 1 }\\cancel{cm^{3}}}\\times\\frac{\\text{1 }\\text{oz}}{\\text{28.35 }\\cancel{\\text{g}}}=\\text{0.52}\\text{ oz}[\/latex]<\/li>\n<li>[latex]\\text{9.91}\\times10^5\\text{ }\\cancel{\\text{mg}}\\times\\frac{10^{-3}\\text{ }\\cancel{\\text{g}}}{\\text{1 }\\cancel{\\text{mg}}}\\times\\frac{\\text{1 }\\cancel{\\text{mL}}}{\\text{1.05 }\\cancel{\\text{g}}}\\times\\frac{\\text{1 }\\text{pt}}{\\text{473.2 }\\cancel{\\text{mL}}}=\\text{1.99 pt}[\/latex]<\/li>\n<\/ol>\n<\/div>\n<div class=\"question\">\n<\/div>\n<\/div>\n<div class=\"question\">\n<p><strong>Converting Units of Temperature<br \/>\n<\/strong><\/p>\n<\/div>\n<div class=\"question\">\n<ol>\n<li class=\"para\">Convert 255\u00b0F to degrees Celsius<\/li>\n<li class=\"para\">Convert\u2212255\u00b0F to degrees Celsius<\/li>\n<li class=\"para\">Convert 50.0\u00b0C to degrees Fahrenheit<\/li>\n<li class=\"para\">Convert \u221250.0\u00b0C to degrees Fahrenheit<\/li>\n<li class=\"para\">Convert 0 K to degrees Celsius. What is the significance of the temperature in degrees Celsius?<\/li>\n<li class=\"para\">The hottest temperature ever recorded on the surface of the earth was 136\u00b0F in Libya in 1922. What is the temperature in degrees Celsius and in kelvins?<\/li>\n<li class=\"para\">The coldest temperature ever recorded on the surface of the earth was \u2212128.6\u00b0F in Vostok, Antarctica, in 1983. What is the temperature in degrees Celsius and in kelvins?<\/li>\n<\/ol>\n<div class=\"question\">\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q798798881\">Show Answers to Select Questions<\/span><\/p>\n<div id=\"q798798881\" class=\"hidden-answer\" style=\"display: none\">\n<div class=\"question\">\n<ol>\n<li>\u00a0124\u00b0C<\/li>\n<li>\u2212159\u00b0C<\/li>\n<li>122\u00b0F<\/li>\n<li>\u221258\u00b0F<\/li>\n<li>\u2212273\u00b0C. This is the lowest possible temperature in degrees Celsius.<\/li>\n<li>57.8\u00b0C; 331 K<\/li>\n<li>\u221289.2\u00b0C; 184 K<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<div class=\"question\">\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-87\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Introductory Chemistry- 1st Canadian Edition . <strong>Authored by<\/strong>: Jessie A. Key and David W. Ball. <strong>Provided by<\/strong>: BCCampus. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/opentextbc.ca\/introductorychemistry\/\">https:\/\/opentextbc.ca\/introductorychemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc-sa\/4.0\/\">CC BY-NC-SA: Attribution-NonCommercial-ShareAlike<\/a><\/em>. <strong>License Terms<\/strong>: Download this book for free at http:\/\/open.bccampus.ca<\/li><li>Chemistry. <strong>Provided by<\/strong>: OpenStax College. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/openstaxcollege.org\">http:\/\/openstaxcollege.org<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get<\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section>","protected":false},"author":23485,"menu_order":5,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Introductory Chemistry- 1st Canadian Edition \",\"author\":\"Jessie A. 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