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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 X(s) + H2O(1)-X(aq) and the temperature of the solution increases to 30.0 "C. 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. Express the change in enthalpy in kilojoules per mole to three significant figures. > View Available Hint(s)

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 X(s) + H2O(1)-X(aq) and the temperature of the solution increases to 30.0 "C. 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. Express the change in enthalpy in kilojoules per mole to three significant figures. > View Available Hint(s)

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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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, G. the equation becomes X(s) + H2O(1)→X(aq) q= Cx 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, qi 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 ΔΗp but it is usually expressed per mole of reactant and with a sign opposite to that of q 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+uw However, at constant volume (as with a bomb calorimeter) w = 0 and so AE= q« ΔΗ- kJ/mol Submit P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use Privacy Pollcy | Permissions I Contact Us chemistry.com/myct/itemView?assignmentProblemID=174388853 7:57 acer
Transcribed Image Text: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, G. the equation becomes X(s) + H2O(1)→X(aq) q= Cx 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, qi 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 ΔΗp but it is usually expressed per mole of reactant and with a sign opposite to that of q 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+uw However, at constant volume (as with a bomb calorimeter) w = 0 and so AE= q« ΔΗ- kJ/mol Submit P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. Terms of Use Privacy Pollcy | Permissions I Contact Us chemistry.com/myct/itemView?assignmentProblemID=174388853 7:57 acer
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