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A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 "C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the solution increases to 30.0 C. At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, gp; that is, Calculate the enthalpy change, AH for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- °C)]. that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. AH = 9, but it is usually expressed per mole of reactant and with a sign opposite to that of g for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and wwork done, w. Express the change in enthalpy in kilojoules per mole to three significant figures. > View Available Hint(s) AE = q+ uo However, at constant volume (as with a bomb calonmeter) ue 0 and so AE=q. ΔΗ- kJ /mol 1 1:20

A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants Periodic Table Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 "C. When 1.70 g of X (a substance with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the solution increases to 30.0 C. At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, gp; that is, Calculate the enthalpy change, AH for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- °C)]. that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the suroundings. AH = 9, but it is usually expressed per mole of reactant and with a sign opposite to that of g for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and wwork done, w. Express the change in enthalpy in kilojoules per mole to three significant figures. > View Available Hint(s) AE = q+ uo However, at constant volume (as with a bomb calonmeter) ue 0 and so AE=q. ΔΗ- kJ /mol 1 1:20

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter9: Energy And Chemistry
Section: Chapter Questions
Problem 9.101PAE
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* Calorimetry 27 of 42 A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants | Periodic Table Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 "C. When 1.70 g of X (a substarce with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the solution increases to 30.0 C. At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, gp; that is Calculate the enthalpy change, AH for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g. °C)]. that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. AH = 9p but it is usually expressed per mole of reactant and with a sign opposite to that of g for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and work done, w: Express the change in enthalpy in kilojoules per mole to three significant figures. • View Available Hint(s) AE =q+ w However, at constant volume (as with a bomb calorimeter) ue 0 and so AE= q.. ΔΗ- kJ/mol 7:20
Transcribed Image Text:* Calorimetry 27 of 42 A calorimeter is an insulated device in which a chemical reaction is contained. By measuring the temperature change, AT, we can calculate the heat released or absorbed during the reaction using the following equation: Constants | Periodic Table Part A q= specific heat x mass x AT A calorimeter contains 30.0 mL of water at 14.0 "C. When 1.70 g of X (a substarce with a molar mass of 76.0 g/mol) is added, it dissolves via the reaction Or, if the calorimeter has a predetermined heat capacity, C, the equation becomes X(s) + H2O(1)→X(aq) q=C x AT and the temperature of the solution increases to 30.0 C. At constant pressure, the enthalpy change for the reaction, AH, is equal to the heat, gp; that is Calculate the enthalpy change, AH for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g. °C)]. that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. AH = 9p but it is usually expressed per mole of reactant and with a sign opposite to that of g for the surroundings. The total internal energy change, AE (sometimes referred to as AU), is the sum of heat, q, and work done, w: Express the change in enthalpy in kilojoules per mole to three significant figures. • View Available Hint(s) AE =q+ w However, at constant volume (as with a bomb calorimeter) ue 0 and so AE= q.. ΔΗ- kJ/mol 7:20
d device in which a ned. By measuring the we can calculate the during the reaction using Part B Consider the reaction Ex mass x AT C12 H22O11 (s) + 1202(g)→12CO2 (g) + 11H20(1) a predetermined heat becomes in which 10.0 g of sucrose, C12 H2O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/"C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE. for this reaction per mole of sucrose. x AT Express the change in internal energy in kilojoules per mole to three significant figures. e enthalpy change for the to the heat, gp, that is, > View Available Hint(s) sed per mole of reactant and that of g for the internal energy change, red to as AU), is the sum of e, w: AE = kJ/mol E= q+ w Submit E volume (as with a bomb and so AE = qo- Next > Provide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions Contact Us E i 1:21
Transcribed Image Text:d device in which a ned. By measuring the we can calculate the during the reaction using Part B Consider the reaction Ex mass x AT C12 H22O11 (s) + 1202(g)→12CO2 (g) + 11H20(1) a predetermined heat becomes in which 10.0 g of sucrose, C12 H2O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/"C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE. for this reaction per mole of sucrose. x AT Express the change in internal energy in kilojoules per mole to three significant figures. e enthalpy change for the to the heat, gp, that is, > View Available Hint(s) sed per mole of reactant and that of g for the internal energy change, red to as AU), is the sum of e, w: AE = kJ/mol E= q+ w Submit E volume (as with a bomb and so AE = qo- Next > Provide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy I Permissions Contact Us E i 1:21
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