In an experiment, a 0.4494 g sample of pyrene ( C16H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.327 × 10³ g of water. During the combustion the temperature increases from 24.64 to 27.30 °C. The heat capacity of water is 4.184 J·g¯¹. C¹. 0 The heat capacity of the calorimeter was determined in a previous experiment to be 801.8 J. ˚C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of pyrene based on these data. C16H10 (8) + (37/2)O2(g) → 5H₂O(1) + 16CO2 (g) + Energy kJ/mol Molar Heat of Combustion =

In an experiment, a 0.4494 g sample of pyrene ( C16H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.327 × 10³ g of water. During the combustion the temperature increases from 24.64 to 27.30 °C. The heat capacity of water is 4.184 J·g¯¹. C¹. 0 The heat capacity of the calorimeter was determined in a previous experiment to be 801.8 J. ˚C-¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of pyrene based on these data. C16H10 (8) + (37/2)O2(g) → 5H₂O(1) + 16CO2 (g) + Energy kJ/mol Molar Heat of Combustion =

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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