The heat capacity of a bomb calorimeter is found to be 5.68 kJ°C⁻¹. When a 1.652 g sample of glucose, C₆H₁₂O₆ (MW = 180 g/mol), is burned in the calorimeter, the temperature of the calorimeter increases from 24.56°C to 29.10°C. Calculate the ΔH for the following reaction:\[ \text{C}_6\text{H}_{12}\text{O}_6(s) + 6 \text{O}_2(g) \rightarrow 6 \text{CO}_2(g) + 6 \text{H}_2\text{O}(g) \]Options:A) -2.81 × 10³ kJ B) -25.8 kJ C) 15.6 kJ D) -42.6 kJ E) 2811 kJ The correct choice indicated is option A.

The heat capacity of a bomb calorimeter is found to be 5.68 kJ °C-1. When a 1.652 g sample of glucose, C6H12O6 (MW= 180 g/mol) is burned in the calorimeter, the temperature of the calorimeter increases from 24.56°C to 29.10°C. Calculate the AH for the following reaction: C6H12O6 (s) +6 02 (g) →6 CO2 (g) + 6 H₂O (g) A)-2.81 x 103 kJ B)-25.8 kJ C) 15.6 kJ D) -42.6 kJ E) 2811 kJ

The heat capacity of a bomb calorimeter is found to be 5.68 kJ °C-1. When a 1.652 g sample of glucose, C6H12O6 (MW= 180 g/mol) is burned in the calorimeter, the temperature of the calorimeter increases from 24.56°C to 29.10°C. Calculate the AH for the following reaction: C6H12O6 (s) +6 02 (g) →6 CO2 (g) + 6 H₂O (g) A)-2.81 x 103 kJ B)-25.8 kJ C) 15.6 kJ D) -42.6 kJ E) 2811 kJ

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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