{"id":13629,"date":"2020-11-24T09:06:30","date_gmt":"2020-11-24T09:06:30","guid":{"rendered":"http:\/\/onlineclassesguru.com\/index.php\/2020\/11\/24\/initial-temperature-in-the-calorimeter\/"},"modified":"2020-11-24T09:06:30","modified_gmt":"2020-11-24T09:06:30","slug":"initial-temperature-in-the-calorimeter","status":"publish","type":"post","link":"https:\/\/onlineclassesguru.com\/index.php\/2020\/11\/24\/initial-temperature-in-the-calorimeter\/","title":{"rendered":"Initial temperature in the calorimeter"},"content":{"rendered":"<style type=\"text\/css\"><\/style><p>1. Record the following:<\/p>\n<p>a<br \/>\nInitial\u00a0temperature\u00a0in the calorimeter (C):<br \/>\nb<br \/>\nMaximum temperature\u00a0in the calorimeter from the reaction (C):<\/p>\n<p>c<br \/>\nCalculate deltaT by subtracting (b) from (c)<br \/>\ndeltaT = Tinitial (C):<\/p>\n<p>2. What was the initial heat energy before mixing the cold and\u00a0hot water? To calculate this you need to use the formula :<br \/>\nQinitial = m1*Cp*T(of the hot water) + m2*Cp*T(of the cold water)<br \/>\nwhere Q is the heat energy, m is the mass , Cp is the\u00a0specific heat\u00a0of water 4.184 J\/g*C, and T is the temperature.<\/p>\n<p>3. 3. What was the final heat energy after mixing the cold and hot water? To calculate this you need to use the formula :<br \/>\nQfinal = (m1+m2) * Cp * Tfinal<\/p>\n<p>4. What is the heat energy of the calorimeter? You can calculate the calorimeter heat energy as the difference between the initial and final heat energies. Choose the closest answer.<\/p>\n<p>5. 5. What is the calorimeter\u00a0constant? You can calculate the calorimeter constant, Ccal, per\u00a0degree\u00a0change of the calorimeter by taking the calorimeter heat energy and dividing it by the temperature change undergone by the calorimeter:<\/p>\n<p>Experiment 2<\/p>\n<p>1. Record the following for each of the three trials:<\/p>\n<p>Trial 1<br \/>\na<br \/>\nMass of the empty calorimeter (g):<\/p>\n<p>b<br \/>\nInitial temperature in the calorimeter (C):<\/p>\n<p>c<br \/>\nMaximum temperature in the calorimeter from the reaction (C):<\/p>\n<p>d<br \/>\nCalculate deltaT by subtracting (b) from (c)<br \/>\ndeltaT = Tmaximum \u2013 Tinitial (C):<\/p>\n<p>e<br \/>\nMass of the calorimeter and its contents after the reaction (g):<\/p>\n<p>f<br \/>\nCalculate the mass of the contents of the calorimeter (g): e \u2013 a<br \/>\ng<br \/>\nCalculate the moles of Mg reacted (MW=24.305 g\/mole):<\/p>\n<p>Trial 2<br \/>\na<br \/>\nMass of the empty calorimeter (g):<\/p>\n<p>b<br \/>\nInitial temperature in the calorimeter (C):<\/p>\n<p>c<br \/>\nMaximum temperature in the calorimeter from the reaction (C):<\/p>\n<p>d<br \/>\nCalculate deltaT by subtracting (b) from (c)<br \/>\ndeltaT = Tmaximum \u2013 Tinitial (C):<\/p>\n<p>e<br \/>\nMass of the calorimeter and its contents after the reaction (g):<\/p>\n<p>f<br \/>\nCalculate the mass of the contents of the calorimeter (g): e \u2013 a<br \/>\ng<br \/>\nCalculate the moles of Mg reacted (MW=24.305 g\/mole):<\/p>\n<p>Trial 3<br \/>\na<br \/>\nMass of the empty calorimeter (g):<\/p>\n<p>b<br \/>\nInitial temperature in the calorimeter (C):<\/p>\n<p>c<br \/>\nMaximum temperature in the calorimeter from the reaction (C):<\/p>\n<p>d<br \/>\nCalculate deltaT by subtracting (b) from (c)<br \/>\ndeltaT = Tmaximum \u2013 Tinitial (C):<\/p>\n<p>e<br \/>\nMass of the calorimeter and its contents after the reaction (g):<\/p>\n<p>f<br \/>\nCalculate the mass of the contents of the calorimeter (g): e \u2013 a<br \/>\ng<br \/>\nCalculate the moles of Mg reacted (MW=24.305 g\/mole):<\/p>\n<p>2. Calculate the heat released into the solution for the 3 reactions, according to:<\/p>\n<p>\uffa0 \uffa0 \uffa0 q(reaction) \uffa0 = \uffa0 Ccal * Delta T + mass(contents) * Cp (contents) * deltaT<br \/>\nCp is the specific heat (assume 4.18 J\/goC)<\/p>\n<p>a<br \/>\nTrial 1 (J)<\/p>\n<p>b<br \/>\nTrial 2 (J)<br \/>\nc<br \/>\nTrial 3 (J)<\/p>\n<p>3. Find the\u00a0molar heat\u00a0of reaction for each experiment in units of KiloJoules \/ (mole of Mg) by dividing the heat of reaction (converted to KJ by dividing by 1000) by the moles of Mg used.<\/p>\n<p>a<br \/>\nTrial 1 KJ\/mol<br \/>\nb<br \/>\nTrial 2 KJ\/mol<br \/>\nc<br \/>\nTrial 3 KJ\/mol<\/p>\n<p>4. Calculate and record the average molar heat of reaction from the three results.<\/p>\n<p>Attachment Preview:<\/p>\n<p><center><a href=\"http:\/\/onlineclassesguru.com\/orders\/ordernow\"><img decoding=\"async\" src=\"https:\/\/encrypted-tbn0.gstatic.com\/images?q=tbn:ANd9GcTyj99p60XCLyLk1htB7-1neRt8-2QdnenNlQ&usqp=CAU\"target=\"_http:\/\/onlineclassesguru.com\/orders\/ordernow\"\/><\/center><p>","protected":false},"excerpt":{"rendered":"<p>1. Record the following: a Initial\u00a0temperature\u00a0in the calorimeter (C): b Maximum temperature\u00a0in the calorimeter from the reaction (C): c Calculate deltaT by subtracting (b) from (c) deltaT = Tinitial (C): 2. What was the initial heat energy before mixing the cold and\u00a0hot water? To calculate this you need to use the formula : Qinitial =&#8230;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[],"tags":[],"class_list":["post-13629","post","type-post","status-publish","format-standard","hentry"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v17.0 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Initial temperature in the calorimeter - onlineclassesguru<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"http:\/\/onlineclassesguru.com\/index.php\/2020\/11\/24\/initial-temperature-in-the-calorimeter\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Initial temperature in the calorimeter - onlineclassesguru\" \/>\n<meta property=\"og:description\" content=\"1. Record the following: a Initial\u00a0temperature\u00a0in the calorimeter (C): b Maximum temperature\u00a0in the calorimeter from the reaction (C): c Calculate deltaT by subtracting (b) from (c) deltaT = Tinitial (C): 2. What was the initial heat energy before mixing the cold and\u00a0hot water? 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Record the following: a Initial\u00a0temperature\u00a0in the calorimeter (C): b Maximum temperature\u00a0in the calorimeter from the reaction (C): c Calculate deltaT by subtracting (b) from (c) deltaT = Tinitial (C): 2. What was the initial heat energy before mixing the cold and\u00a0hot water? 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