{"id":6433,"date":"2020-10-23T23:17:17","date_gmt":"2020-10-23T23:17:17","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/?post_type=chapter&#038;p=6433"},"modified":"2021-06-25T20:58:29","modified_gmt":"2021-06-25T20:58:29","slug":"assignment-thermochemistry","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/chapter\/assignment-thermochemistry\/","title":{"raw":"Assignment: Enthalpy, Energy, and Temperature Change","rendered":"Assignment: Enthalpy, Energy, and Temperature Change"},"content":{"raw":"This assignment can be found in Google Docs:\u00a0<a href=\"https:\/\/docs.google.com\/document\/d\/1dgJFphV8D5kFOnZtuvyhb8zH8aYh4Gvc5TcF8ZP19RU\/edit#\" target=\"_blank\" rel=\"noopener\">Chemistry for Majors Assignment: Enthalpy, Energy, and Temperature Change<\/a>\r\n\r\nTo make your own copy to edit:\r\n<ul>\r\n \t<li><strong>If you want a Google Doc<\/strong>: in the file menu of the open document, click \u201cMake a copy.\u201d This will give you your own Google Doc to work from.<\/li>\r\n \t<li><strong>If you want a PDF or Word file<\/strong>: in the file menu of the open document, click \u201cDownload\u201d and select the file type you would like to have (note: depending on the file type you select, the formatting could get jumbled).<\/li>\r\n<\/ul>\r\nComplete the following thermochemistry problems \u2013 show all of your work as you set up equations and make calculations.\r\n<ol>\r\n \t<li style=\"list-style-type: none;\">\r\n<ol>\r\n \t<li style=\"font-weight: 400;\">The Travis Scott promotional meal at McDonald\u2019s had [latex]1180[\/latex] Calories (note the capital letter- this indicates nutritional Calories). Find the amount of energy in Joules.<\/li>\r\n \t<li style=\"font-weight: 400;\">A [latex]9.00[\/latex] g nugget of pure gold absorbed [latex]276[\/latex] J of heat. What was the final temperature of the gold if the initial temperature was [latex]25.0[\/latex]\u00b0 C? The specific heat of gold is [latex]0.129[\/latex] J\/(g \u00b0C).<\/li>\r\n \t<li style=\"font-weight: 400;\">A sample of silver with a mass of [latex]63.3[\/latex] g is heated to a temperature of [latex]384.4[\/latex] K and placed in a container of water at [latex]290.0^{\\circ}[\/latex]K. The final (equilibrium) temperature of the silver and water is [latex]292.4^{\\circ}[\/latex]K. What volume of water is in the container? The specific heat of silver is [latex]0.235[\/latex] J\/(g \u00b0C).<\/li>\r\n \t<li style=\"font-weight: 400;\">NSU Chemistry 101L class conducted an experiment in which a measured amount of [latex]\\text{NaOH}[\/latex] is dissolved in water inside a foam cup calorimeter. A student collected data throughout the experiment. Calculate [latex]\\Delta\\text{H}[\/latex] for the process in kJ\/mol.\r\n<ul>\r\n \t<li>Data table from the experiment:\r\n<table>\r\n<tbody>\r\n<tr>\r\n<td>Mass of NaOH + weigh boat<\/td>\r\n<td>14.13 g<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mass of weigh boat<\/td>\r\n<td>0.70 g<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mass of NaOH<\/td>\r\n<td><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mass of foam cup+water<\/td>\r\n<td>109.85 g<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mass of foam cup<\/td>\r\n<td>10.25 g<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mass of water<\/td>\r\n<td><\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Initial temp of water<\/td>\r\n<td>24.5\u00b0C<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Final temp of water<\/td>\r\n<td>36.8\u00b0C<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Change in temperature (\u0394T)<\/td>\r\n<td><\/td>\r\n<\/tr>\r\n<tr>\r\n<td><\/td>\r\n<td><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/li>\r\n<\/ul>\r\n<\/li>\r\n \t<li>You can light a charcoal grill in about a minute. If the grill is prepared using one [latex]20[\/latex] pound bag of charcoal (primarily carbon) and two [latex]1[\/latex] gallon buckets of liquid oxygen (the density of LOX (liquid oxygen) is [latex]1142[\/latex] kg\/m<sup>3<\/sup>, <em>CRC Handbook of Chemistry and Physics<\/em>.)\r\n<ul>\r\n \t<li>Write a balanced chemical equation describing this reaction.<\/li>\r\n \t<li>Determine the limiting reagent for this reaction.<\/li>\r\n \t<li>Calculate the mass of each product and any remaining reactant.<\/li>\r\n \t<li>Calculate the amount of heat released by this reaction.<\/li>\r\n \t<li>If this heat is used to warm a [latex]500[\/latex] gallon tank of water at [latex]15^{\\circ}[\/latex]C, what is the final temperature?<\/li>\r\n \t<li>If this heat is used to warm [latex]40[\/latex] kg of ice at [latex]200^{\\circ}[\/latex]K, what is the final temperature?<\/li>\r\n<\/ul>\r\n<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>","rendered":"<p>This assignment can be found in Google Docs:\u00a0<a href=\"https:\/\/docs.google.com\/document\/d\/1dgJFphV8D5kFOnZtuvyhb8zH8aYh4Gvc5TcF8ZP19RU\/edit#\" target=\"_blank\" rel=\"noopener\">Chemistry for Majors Assignment: Enthalpy, Energy, and Temperature Change<\/a><\/p>\n<p>To make your own copy to edit:<\/p>\n<ul>\n<li><strong>If you want a Google Doc<\/strong>: in the file menu of the open document, click \u201cMake a copy.\u201d This will give you your own Google Doc to work from.<\/li>\n<li><strong>If you want a PDF or Word file<\/strong>: in the file menu of the open document, click \u201cDownload\u201d and select the file type you would like to have (note: depending on the file type you select, the formatting could get jumbled).<\/li>\n<\/ul>\n<p>Complete the following thermochemistry problems \u2013 show all of your work as you set up equations and make calculations.<\/p>\n<ol>\n<li style=\"list-style-type: none;\">\n<ol>\n<li style=\"font-weight: 400;\">The Travis Scott promotional meal at McDonald\u2019s had [latex]1180[\/latex] Calories (note the capital letter- this indicates nutritional Calories). Find the amount of energy in Joules.<\/li>\n<li style=\"font-weight: 400;\">A [latex]9.00[\/latex] g nugget of pure gold absorbed [latex]276[\/latex] J of heat. What was the final temperature of the gold if the initial temperature was [latex]25.0[\/latex]\u00b0 C? The specific heat of gold is [latex]0.129[\/latex] J\/(g \u00b0C).<\/li>\n<li style=\"font-weight: 400;\">A sample of silver with a mass of [latex]63.3[\/latex] g is heated to a temperature of [latex]384.4[\/latex] K and placed in a container of water at [latex]290.0^{\\circ}[\/latex]K. The final (equilibrium) temperature of the silver and water is [latex]292.4^{\\circ}[\/latex]K. What volume of water is in the container? The specific heat of silver is [latex]0.235[\/latex] J\/(g \u00b0C).<\/li>\n<li style=\"font-weight: 400;\">NSU Chemistry 101L class conducted an experiment in which a measured amount of [latex]\\text{NaOH}[\/latex] is dissolved in water inside a foam cup calorimeter. A student collected data throughout the experiment. Calculate [latex]\\Delta\\text{H}[\/latex] for the process in kJ\/mol.\n<ul>\n<li>Data table from the experiment:<br \/>\n<table>\n<tbody>\n<tr>\n<td>Mass of NaOH + weigh boat<\/td>\n<td>14.13 g<\/td>\n<\/tr>\n<tr>\n<td>Mass of weigh boat<\/td>\n<td>0.70 g<\/td>\n<\/tr>\n<tr>\n<td>Mass of NaOH<\/td>\n<td><\/td>\n<\/tr>\n<tr>\n<td>Mass of foam cup+water<\/td>\n<td>109.85 g<\/td>\n<\/tr>\n<tr>\n<td>Mass of foam cup<\/td>\n<td>10.25 g<\/td>\n<\/tr>\n<tr>\n<td>Mass of water<\/td>\n<td><\/td>\n<\/tr>\n<tr>\n<td>Initial temp of water<\/td>\n<td>24.5\u00b0C<\/td>\n<\/tr>\n<tr>\n<td>Final temp of water<\/td>\n<td>36.8\u00b0C<\/td>\n<\/tr>\n<tr>\n<td>Change in temperature (\u0394T)<\/td>\n<td><\/td>\n<\/tr>\n<tr>\n<td><\/td>\n<td><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/li>\n<\/ul>\n<\/li>\n<li>You can light a charcoal grill in about a minute. If the grill is prepared using one [latex]20[\/latex] pound bag of charcoal (primarily carbon) and two [latex]1[\/latex] gallon buckets of liquid oxygen (the density of LOX (liquid oxygen) is [latex]1142[\/latex] kg\/m<sup>3<\/sup>, <em>CRC Handbook of Chemistry and Physics<\/em>.)\n<ul>\n<li>Write a balanced chemical equation describing this reaction.<\/li>\n<li>Determine the limiting reagent for this reaction.<\/li>\n<li>Calculate the mass of each product and any remaining reactant.<\/li>\n<li>Calculate the amount of heat released by this reaction.<\/li>\n<li>If this heat is used to warm a [latex]500[\/latex] gallon tank of water at [latex]15^{\\circ}[\/latex]C, what is the final temperature?<\/li>\n<li>If this heat is used to warm [latex]40[\/latex] kg of ice at [latex]200^{\\circ}[\/latex]K, what is the final temperature?<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\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-6433\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Original<\/div><ul class=\"citation-list\"><li>Assignment: Enthalpy, Energy, and Temperature Change. <strong>Provided by<\/strong>: Lumen Learning. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em><\/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":17533,"menu_order":11,"template":"","meta":{"_candela_citation":"[{\"type\":\"original\",\"description\":\"Assignment: Enthalpy, Energy, and Temperature Change\",\"author\":\"\",\"organization\":\"Lumen Learning\",\"url\":\"\",\"project\":\"\",\"license\":\"cc-by\",\"license_terms\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-6433","chapter","type-chapter","status-publish","hentry"],"part":3023,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6433","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/users\/17533"}],"version-history":[{"count":12,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6433\/revisions"}],"predecessor-version":[{"id":8177,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6433\/revisions\/8177"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/parts\/3023"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapters\/6433\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/media?parent=6433"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/pressbooks\/v2\/chapter-type?post=6433"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/contributor?post=6433"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/chemistryformajors\/wp-json\/wp\/v2\/license?post=6433"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}