{"id":780,"date":"2018-03-20T15:55:49","date_gmt":"2018-03-20T15:55:49","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-orgbiochemistry\/?post_type=chapter&#038;p=780"},"modified":"2018-09-19T14:49:41","modified_gmt":"2018-09-19T14:49:41","slug":"8-3-gases-and-pressure","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/chapter\/8-3-gases-and-pressure\/","title":{"raw":"8.3 Gases and Pressure","rendered":"8.3 Gases and Pressure"},"content":{"raw":"<div id=\"navbar-top\" class=\"navbar\"><\/div>\r\n<div id=\"book-content\">\r\n<div id=\"gob-ch08_s03\" class=\"section\" xml:lang=\"en\">\r\n<div id=\"gob-ch08_s03_n01\" class=\"learning_objectives editable block\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3 class=\"title\">Learning Objective<\/h3>\r\n<ol id=\"gob-ch08_s03_l01\" class=\"orderedlist\">\r\n \t<li>Describe the gas phase.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<p id=\"gob-ch08_s03_p01\" class=\"para editable block\">The gas phase is unique among the three states of matter in that there are some simple models we can use to predict the physical behavior of all gases\u2014independent of their identities. We cannot do this for the solid and liquid states. In fact, the development of this understanding of the behavior of gases represents the historical dividing point between alchemy and modern chemistry. Initial advances in the understanding of gas behavior were made in the mid 1600s by Robert Boyle, an English scientist who founded the Royal Society, one of the world\u2019s oldest scientific organizations.<\/p>\r\n<p id=\"gob-ch08_s03_p02\" class=\"para editable block\">How is it that we can model all gases independent of their chemical identity? The answer is in a group of statements called the <span class=\"margin_term\"><strong><span class=\"glossterm\">kinetic molecular theory of gases<\/span><\/strong><\/span>:<\/p>\r\n\r\n<ul id=\"gob-ch08_s03_l02\" class=\"itemizedlist editable block\">\r\n \t<li>Gases are composed of tiny particles that are separated by large distances.<\/li>\r\n \t<li>Gas particles are constantly moving, experiencing collisions with other gas particles and the walls of their container.<\/li>\r\n \t<li>The velocity of gas particles is directly proportional to the absolute temperature of a gas.<\/li>\r\n \t<li>Gas particles do not experience any force of attraction or repulsion with each other.<\/li>\r\n<\/ul>\r\n<p id=\"gob-ch08_s03_p03\" class=\"para editable block\">Notice that none of these statements relates to the identity of the gas. This means that all gases should behave similarly. A gas that follows these statements perfectly is called an <em class=\"emphasis\">ideal gas<\/em>. Most gases show slight deviations from these statements and are called <em class=\"emphasis\">real gases<\/em>. However, the existence of real gases does not diminish the importance of the kinetic theory of gases.<\/p>\r\nThe kinetic theory also states that there is no interaction between individual gas particles. Although we know that there are, in fact, intermolecular interactions in real gases, the kinetic theory assumes that gas particles are so far apart that the individual particles don\u2019t \u201cfeel\u201d each other. Thus, we can treat gas particles as tiny bits of matter whose identity isn\u2019t important to certain physical properties.\r\n<p id=\"gob-ch08_s03_p04\" class=\"para editable block\">One of the statements of the kinetic theory mentions collisions. As gas particles are constantly moving, they are also constantly colliding with each other and with the walls of their container. There are forces involved as gas particles bounce off the container walls (<a class=\"xref\" href=\"#gob-ch08_s03_f01\">Figure 8.9 \"Gas Pressure\"<\/a>). The force generated by gas particles divided by the area of the container walls yields <strong><span class=\"margin_term\"><span class=\"glossterm\">pressure<\/span><\/span><\/strong>. Due to the large amount of empty space between molecules in a gas, gases are compressible, so the pressure must be specified when other measurements are reported for gases.\u00a0 Solids and liquids also experience and exert pressures,\u00a0 but under everyday conditions, pressure does not affect their properties.<\/p>\r\n\r\n<div id=\"gob-ch08_s03_f01\" class=\"figure large medium-height editable block\">\r\n\r\n<img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20155338\/fbdf37a85ccf2788ba9d689d1ee777ff.jpg\" alt=\"image\" width=\"1078\" height=\"1078\" \/><em><em>Figure 8.9 Gas Pressure.<\/em><\/em>\r\n<div id=\"gob-ch08_s03_f01\" class=\"figure large medium-height editable block\">\r\n<p class=\"para\">Pressure is what results when gas particles rebound off the walls of their container.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<p id=\"gob-ch08_s03_p05\" class=\"para editable block\">The basic unit of pressure is the newton per square meter (N\/m<sup class=\"superscript\">2<\/sup>). This combined unit is redefined as a <span class=\"margin_term\"><strong><span class=\"glossterm\">pascal\u00a0<\/span><\/strong><\/span>(Pa). One pascal is not a very large amount of pressure. A more useful unit of pressure is the <span class=\"margin_term\"><strong><span class=\"glossterm\">bar<\/span><\/strong><\/span>, which is 100,000 Pa (1 bar = 100,000 Pa). Other common units of pressure are the <span class=\"margin_term\"><strong><span class=\"glossterm\">atmosphere\u00a0<\/span><\/strong><\/span>(atm), which was originally defined as the average pressure of Earth\u2019s atmosphere at sea level; and <span class=\"margin_term\"><strong><span class=\"glossterm\">mmHg (millimeters of mercury)<\/span><\/strong><\/span>, which is the pressure generated by a column of mercury 1 mm high. The unit millimeters of mercury is also called a <span class=\"margin_term\"><strong><span class=\"glossterm\">torr<\/span><\/strong><\/span>, named after the Italian scientist Evangelista Torricelli, who invented the barometer in the mid-1600s. A more precise definition of atmosphere, in terms of torr, is that there are exactly 760 torr in 1 atm. A bar equals 1.01325 atm. Given all the relationships between these pressure units, the ability to convert from one pressure unit to another is a useful skill.<\/p>\r\n\r\n<div id=\"gob-ch08_s03_n02\" class=\"exercises block\">\r\n<h3 class=\"title\">Example 3<\/h3>\r\n<p id=\"gob-ch08_s03_p06\" class=\"para\">Write a conversion factor to determine how many atmospheres are in 1,547 mmHg.<\/p>\r\n<p class=\"simpara\">Solution<\/p>\r\n<p id=\"gob-ch08_s03_p07\" class=\"para\">Because 1 mmHg equals 1 torr, the given pressure is also equal to 1,547 torr. Because there are 760 torr in 1 atm, we can use this conversion factor to do the mathematical conversion:<\/p>\r\n<p style=\"text-align: center\"><span class=\"informalequation\">[latex]1547\\cancel{\\text{ torr}}\\times\\frac{1\\text{ atm}}{760\\cancel{\\text{ torr}}}=2.036\\text{atm}[\/latex]<\/span><\/p>\r\nThe conversion factor 760 torr = 1 atm is exact, so it does not limit the sig figs.\u00a0 The answer is rounded to 4 sig figs because the measured pressure of 1547 torr has 4 sig figs.\r\n\r\n<\/div>\r\n<div id=\"gob-ch08_s03_qs01\" class=\"qandaset block\">\r\n<div class=\"textbox exercises\">\r\n<h3 class=\"title\">Skill-Building Exercise<\/h3>\r\n<ol id=\"gob-ch08_s03_qs01_qd01\" class=\"qandadiv\">\r\n \t<li id=\"gob-ch08_s03_qs01_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs01_p01\" class=\"para\">Write a conversion factor to determine how many millimeters of mercury are in 9.65 atm.<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\r\n<div class=\"textbox exercises\">\r\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\r\n<h3 class=\"title\">Concept Review Exercise<\/h3>\r\n<ol id=\"gob-ch08_s03_qs02_qd01\" class=\"qandadiv\">\r\n \t<li id=\"gob-ch08_s03_qs02_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs02_p01\" class=\"para\">What is pressure, and what units do we use to express it?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<div id=\"gob-ch08_s03_qs02_ans\" class=\"qandaset block\">\r\n<h3 class=\"title\">Answer<\/h3>\r\n[reveal-answer q=\"402174\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"402174\"]1. Pressure is the force per unit area; its units can be pascals, torr, millimeters of mercury, or atmospheres.\u00a0[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox key-takeaways\">\r\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\r\n<h3 class=\"title\">Key Takeaway<\/h3>\r\n<\/div>\r\n<div id=\"gob-ch08_s03_n05\" class=\"key_takeaways editable block\">\r\n<ul id=\"gob-ch08_s03_l03\" class=\"itemizedlist\">\r\n \t<li>The gas phase has certain general properties characteristic of that phase.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"gob-ch08_s03_qs03\" class=\"qandaset block\">\r\n<div class=\"textbox exercises\">\r\n<h3>Exercises<\/h3>\r\n<div id=\"book-content\">\r\n<div id=\"gob-ch08_s03\" class=\"section\" xml:lang=\"en\">\r\n<div id=\"gob-ch08_s03_qs03\" class=\"qandaset block\">\r\n<ol id=\"gob-ch08_s03_qs03_qd01\" class=\"qandadiv\">\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p01\" class=\"para\">What is the kinetic theory of gases?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa02\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p03\" class=\"para\">According to the kinetic theory of gases, the individual gas particles are (always, frequently, never) moving.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa03\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p05\" class=\"para\">Why does a gas exert pressure?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa04\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p07\" class=\"para\">Why does the kinetic theory of gases allow us to presume that all gases will show similar behavior?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa05\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p09\" class=\"para\">Arrange the following pressure quantities in order from smallest to largest: 1 mmHg, 1 Pa, and 1 atm.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa06\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p11\" class=\"para\">Which unit of pressure is larger\u2014the torr or the atmosphere?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa07\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p13\" class=\"para\">How many torr are there in 1.56 atm?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa08\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p15\" class=\"para\">Convert 760 torr into pascals.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa09\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p17\" class=\"para\">Blood pressures are expressed in millimeters of mercury. What would be the blood pressure in atmospheres if a patient\u2019s systolic blood pressure is 120 mmHg and the diastolic blood pressure is 82 mmHg? (In medicine, such a blood pressure would be reported as \u201c120\/82,\u201d spoken as \u201cone hundred twenty over eighty-two.\u201d)<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch08_s03_qs03_qd01_qa10\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch08_s03_qs03_p19\" class=\"para\">In weather forecasting, barometric pressure is expressed in inches of mercury (in. Hg), where there are exactly 25.4 mmHg in every 1 in. Hg. What is the barometric pressure in millimeters of mercury if the barometric pressure is reported as 30.21 in. Hg?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<div id=\"gob-ch08_s03_qs03_ans\" class=\"qandaset block\">\r\n<h3 class=\"title\">Answers<\/h3>\r\n[reveal-answer q=\"994271\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"994271\"]\r\n\r\n1. Gases are composed of tiny particles that are separated by large distances. Gas particles are constantly moving, experiencing collisions with other gas particles and the walls of their container. The velocity of gas particles is related to the temperature of a gas. Gas particles do not experience any force of attraction or repulsion with each other.\r\n\r\n3. A gas exerts pressure as its particles rebound off the walls of its container.\r\n\r\n5. 1 Pa, 1 mmHg, and 1 atm\r\n\r\n7. 1,190 torr\r\n\r\n9. 0.158 atm; 0.108 atm \u00a0[\/hidden-answer]\r\n<div class=\"answer\"><\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div id=\"navbar-top\" class=\"navbar\"><\/div>\n<div id=\"book-content\">\n<div id=\"gob-ch08_s03\" class=\"section\" xml:lang=\"en\">\n<div id=\"gob-ch08_s03_n01\" class=\"learning_objectives editable block\">\n<div class=\"textbox learning-objectives\">\n<h3 class=\"title\">Learning Objective<\/h3>\n<ol id=\"gob-ch08_s03_l01\" class=\"orderedlist\">\n<li>Describe the gas phase.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<p id=\"gob-ch08_s03_p01\" class=\"para editable block\">The gas phase is unique among the three states of matter in that there are some simple models we can use to predict the physical behavior of all gases\u2014independent of their identities. We cannot do this for the solid and liquid states. In fact, the development of this understanding of the behavior of gases represents the historical dividing point between alchemy and modern chemistry. Initial advances in the understanding of gas behavior were made in the mid 1600s by Robert Boyle, an English scientist who founded the Royal Society, one of the world\u2019s oldest scientific organizations.<\/p>\n<p id=\"gob-ch08_s03_p02\" class=\"para editable block\">How is it that we can model all gases independent of their chemical identity? The answer is in a group of statements called the <span class=\"margin_term\"><strong><span class=\"glossterm\">kinetic molecular theory of gases<\/span><\/strong><\/span>:<\/p>\n<ul id=\"gob-ch08_s03_l02\" class=\"itemizedlist editable block\">\n<li>Gases are composed of tiny particles that are separated by large distances.<\/li>\n<li>Gas particles are constantly moving, experiencing collisions with other gas particles and the walls of their container.<\/li>\n<li>The velocity of gas particles is directly proportional to the absolute temperature of a gas.<\/li>\n<li>Gas particles do not experience any force of attraction or repulsion with each other.<\/li>\n<\/ul>\n<p id=\"gob-ch08_s03_p03\" class=\"para editable block\">Notice that none of these statements relates to the identity of the gas. This means that all gases should behave similarly. A gas that follows these statements perfectly is called an <em class=\"emphasis\">ideal gas<\/em>. Most gases show slight deviations from these statements and are called <em class=\"emphasis\">real gases<\/em>. However, the existence of real gases does not diminish the importance of the kinetic theory of gases.<\/p>\n<p>The kinetic theory also states that there is no interaction between individual gas particles. Although we know that there are, in fact, intermolecular interactions in real gases, the kinetic theory assumes that gas particles are so far apart that the individual particles don\u2019t \u201cfeel\u201d each other. Thus, we can treat gas particles as tiny bits of matter whose identity isn\u2019t important to certain physical properties.<\/p>\n<p id=\"gob-ch08_s03_p04\" class=\"para editable block\">One of the statements of the kinetic theory mentions collisions. As gas particles are constantly moving, they are also constantly colliding with each other and with the walls of their container. There are forces involved as gas particles bounce off the container walls (<a class=\"xref\" href=\"#gob-ch08_s03_f01\">Figure 8.9 &#8220;Gas Pressure&#8221;<\/a>). The force generated by gas particles divided by the area of the container walls yields <strong><span class=\"margin_term\"><span class=\"glossterm\">pressure<\/span><\/span><\/strong>. Due to the large amount of empty space between molecules in a gas, gases are compressible, so the pressure must be specified when other measurements are reported for gases.\u00a0 Solids and liquids also experience and exert pressures,\u00a0 but under everyday conditions, pressure does not affect their properties.<\/p>\n<div id=\"gob-ch08_s03_f01\" class=\"figure large medium-height editable block\">\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20155338\/fbdf37a85ccf2788ba9d689d1ee777ff.jpg\" alt=\"image\" width=\"1078\" height=\"1078\" \/><em><em>Figure 8.9 Gas Pressure.<\/em><\/em><\/p>\n<div id=\"gob-ch08_s03_f01\" class=\"figure large medium-height editable block\">\n<p class=\"para\">Pressure is what results when gas particles rebound off the walls of their container.<\/p>\n<\/div>\n<\/div>\n<p id=\"gob-ch08_s03_p05\" class=\"para editable block\">The basic unit of pressure is the newton per square meter (N\/m<sup class=\"superscript\">2<\/sup>). This combined unit is redefined as a <span class=\"margin_term\"><strong><span class=\"glossterm\">pascal\u00a0<\/span><\/strong><\/span>(Pa). One pascal is not a very large amount of pressure. A more useful unit of pressure is the <span class=\"margin_term\"><strong><span class=\"glossterm\">bar<\/span><\/strong><\/span>, which is 100,000 Pa (1 bar = 100,000 Pa). Other common units of pressure are the <span class=\"margin_term\"><strong><span class=\"glossterm\">atmosphere\u00a0<\/span><\/strong><\/span>(atm), which was originally defined as the average pressure of Earth\u2019s atmosphere at sea level; and <span class=\"margin_term\"><strong><span class=\"glossterm\">mmHg (millimeters of mercury)<\/span><\/strong><\/span>, which is the pressure generated by a column of mercury 1 mm high. The unit millimeters of mercury is also called a <span class=\"margin_term\"><strong><span class=\"glossterm\">torr<\/span><\/strong><\/span>, named after the Italian scientist Evangelista Torricelli, who invented the barometer in the mid-1600s. A more precise definition of atmosphere, in terms of torr, is that there are exactly 760 torr in 1 atm. A bar equals 1.01325 atm. Given all the relationships between these pressure units, the ability to convert from one pressure unit to another is a useful skill.<\/p>\n<div id=\"gob-ch08_s03_n02\" class=\"exercises block\">\n<h3 class=\"title\">Example 3<\/h3>\n<p id=\"gob-ch08_s03_p06\" class=\"para\">Write a conversion factor to determine how many atmospheres are in 1,547 mmHg.<\/p>\n<p class=\"simpara\">Solution<\/p>\n<p id=\"gob-ch08_s03_p07\" class=\"para\">Because 1 mmHg equals 1 torr, the given pressure is also equal to 1,547 torr. Because there are 760 torr in 1 atm, we can use this conversion factor to do the mathematical conversion:<\/p>\n<p style=\"text-align: center\"><span class=\"informalequation\">[latex]1547\\cancel{\\text{ torr}}\\times\\frac{1\\text{ atm}}{760\\cancel{\\text{ torr}}}=2.036\\text{atm}[\/latex]<\/span><\/p>\n<p>The conversion factor 760 torr = 1 atm is exact, so it does not limit the sig figs.\u00a0 The answer is rounded to 4 sig figs because the measured pressure of 1547 torr has 4 sig figs.<\/p>\n<\/div>\n<div id=\"gob-ch08_s03_qs01\" class=\"qandaset block\">\n<div class=\"textbox exercises\">\n<h3 class=\"title\">Skill-Building Exercise<\/h3>\n<ol id=\"gob-ch08_s03_qs01_qd01\" class=\"qandadiv\">\n<li id=\"gob-ch08_s03_qs01_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs01_p01\" class=\"para\">Write a conversion factor to determine how many millimeters of mercury are in 9.65 atm.<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\n<div class=\"textbox exercises\">\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\n<h3 class=\"title\">Concept Review Exercise<\/h3>\n<ol id=\"gob-ch08_s03_qs02_qd01\" class=\"qandadiv\">\n<li id=\"gob-ch08_s03_qs02_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs02_p01\" class=\"para\">What is pressure, and what units do we use to express it?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<div id=\"gob-ch08_s03_qs02_ans\" class=\"qandaset block\">\n<h3 class=\"title\">Answer<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q402174\">Show Answer<\/span><\/p>\n<div id=\"q402174\" class=\"hidden-answer\" style=\"display: none\">1. Pressure is the force per unit area; its units can be pascals, torr, millimeters of mercury, or atmospheres.\u00a0<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<div id=\"gob-ch08_s03_qs02\" class=\"qandaset block\">\n<h3 class=\"title\">Key Takeaway<\/h3>\n<\/div>\n<div id=\"gob-ch08_s03_n05\" class=\"key_takeaways editable block\">\n<ul id=\"gob-ch08_s03_l03\" class=\"itemizedlist\">\n<li>The gas phase has certain general properties characteristic of that phase.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"gob-ch08_s03_qs03\" class=\"qandaset block\">\n<div class=\"textbox exercises\">\n<h3>Exercises<\/h3>\n<div id=\"book-content\">\n<div id=\"gob-ch08_s03\" class=\"section\" xml:lang=\"en\">\n<div id=\"gob-ch08_s03_qs03\" class=\"qandaset block\">\n<ol id=\"gob-ch08_s03_qs03_qd01\" class=\"qandadiv\">\n<li id=\"gob-ch08_s03_qs03_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p01\" class=\"para\">What is the kinetic theory of gases?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa02\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p03\" class=\"para\">According to the kinetic theory of gases, the individual gas particles are (always, frequently, never) moving.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa03\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p05\" class=\"para\">Why does a gas exert pressure?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa04\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p07\" class=\"para\">Why does the kinetic theory of gases allow us to presume that all gases will show similar behavior?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa05\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p09\" class=\"para\">Arrange the following pressure quantities in order from smallest to largest: 1 mmHg, 1 Pa, and 1 atm.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa06\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p11\" class=\"para\">Which unit of pressure is larger\u2014the torr or the atmosphere?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa07\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p13\" class=\"para\">How many torr are there in 1.56 atm?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa08\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p15\" class=\"para\">Convert 760 torr into pascals.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa09\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p17\" class=\"para\">Blood pressures are expressed in millimeters of mercury. What would be the blood pressure in atmospheres if a patient\u2019s systolic blood pressure is 120 mmHg and the diastolic blood pressure is 82 mmHg? (In medicine, such a blood pressure would be reported as \u201c120\/82,\u201d spoken as \u201cone hundred twenty over eighty-two.\u201d)<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch08_s03_qs03_qd01_qa10\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch08_s03_qs03_p19\" class=\"para\">In weather forecasting, barometric pressure is expressed in inches of mercury (in. Hg), where there are exactly 25.4 mmHg in every 1 in. Hg. What is the barometric pressure in millimeters of mercury if the barometric pressure is reported as 30.21 in. Hg?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<div id=\"gob-ch08_s03_qs03_ans\" class=\"qandaset block\">\n<h3 class=\"title\">Answers<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q994271\">Show Answer<\/span><\/p>\n<div id=\"q994271\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. Gases are composed of tiny particles that are separated by large distances. Gas particles are constantly moving, experiencing collisions with other gas particles and the walls of their container. The velocity of gas particles is related to the temperature of a gas. Gas particles do not experience any force of attraction or repulsion with each other.<\/p>\n<p>3. A gas exerts pressure as its particles rebound off the walls of its container.<\/p>\n<p>5. 1 Pa, 1 mmHg, and 1 atm<\/p>\n<p>7. 1,190 torr<\/p>\n<p>9. 0.158 atm; 0.108 atm \u00a0<\/p><\/div>\n<\/div>\n<div class=\"answer\"><\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p>&nbsp;<\/p>\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-780\">\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>The Basics of General, Organic, and Biological Chemistry v. 1.0. <strong>Provided by<\/strong>: Saylor Academy. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/\">https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc\/4.0\/\">CC BY-NC: Attribution-NonCommercial<\/a><\/em>. <strong>License Terms<\/strong>: This text was adapted by Saylor Academy under a Creative Commons Attribution-NonCommercial-ShareAlike 3.0 License without attribution as requested by the work&#039;s original creator or licensor.<\/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":44985,"menu_order":4,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"The Basics of General, Organic, and Biological Chemistry v. 1.0\",\"author\":\"\",\"organization\":\"Saylor Academy\",\"url\":\"https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/\",\"project\":\"\",\"license\":\"cc-by-nc\",\"license_terms\":\"This text was adapted by Saylor Academy under a Creative Commons Attribution-NonCommercial-ShareAlike 3.0 License without attribution as requested by the work\\'s original creator or licensor.\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-780","chapter","type-chapter","status-publish","hentry"],"part":753,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/780","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/users\/44985"}],"version-history":[{"count":13,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/780\/revisions"}],"predecessor-version":[{"id":3408,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/780\/revisions\/3408"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/parts\/753"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/780\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/media?parent=780"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=780"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/contributor?post=780"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/license?post=780"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}