**Combustion of Sucrose in a Bomb Calorimeter**The combustion of 1.727 g of sucrose, \( C_{12}H_{22}O_{11}(s) \), in a bomb calorimeter with a heat capacity of 5.20 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.27 °C to 27.75 °C. What is the internal energy change, \( \Delta U \), for the combustion of 1.727 g of sucrose?\[ \Delta U = \_\_\_\_ \text{kJ} \]**Calculate the Enthalpy of Combustion**Calculate the enthalpy of combustion, \( \Delta H_c \), of sucrose in kilojoules per mole.\[ \Delta H_c = \_\_\_\_ \text{kJ/mol} \]

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Answered: The combustion of 1.727 g of sucrose,…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)
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