Sucrose, C₁₂H₂2O(s), is commonly used to sweeten food. In order to determine the molar enthalpy of combustion for sucrose, a technician burns a 0.015 0 mol sample of sucrose using a copper calorimeter that contains 250.0 g of water. The combustion of sucrose is represented by the following equation. C₁2H₂2O(s) + 12 O₂(g) → 12 CO₂(g) + 11 H₂O(g) 6. If the temperature change of the water in the calorimeter is +55.5 °C, then the experimental molar enthalpy of combustion for sucrose is approximately A. -8.72 x 10¹ kJ/mol B. -1.40 x 10¹ kJ/mol C. -5.81 x 10¹ kJ/mol D. -3.88 x 10³ kJ/mol

Sucrose, C₁₂H₂2O(s), is commonly used to sweeten food. In order to determine the molar enthalpy of combustion for sucrose, a technician burns a 0.015 0 mol sample of sucrose using a copper calorimeter that contains 250.0 g of water. The combustion of sucrose is represented by the following equation. C₁2H₂2O(s) + 12 O₂(g) → 12 CO₂(g) + 11 H₂O(g) 6. If the temperature change of the water in the calorimeter is +55.5 °C, then the experimental molar enthalpy of combustion for sucrose is approximately A. -8.72 x 10¹ kJ/mol B. -1.40 x 10¹ kJ/mol C. -5.81 x 10¹ kJ/mol D. -3.88 x 10³ kJ/mol

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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