A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat ofcombustion of fuels and the energy available from foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heatcapacity of the calorimeter. This is known as calibrating the calorimeter.In the laboratory a student burns a 0.971-g sample of dimethyl oxalate (CĄHGO4) in a bombcalorimeter containing 1050. g water. The temperature increases from 25.40 °C to 28.00 °C. Thespecific heat capacity of water is 4.184 J g-1 °C•!.The combustion enthalpy is –1675 kJ/mol dimethyl oxalate.C,H,O4(s) + 7/2 O2(g -→4 CO2(g) + 3 H20(1) A,H° = -1675 kJ/molCalculate the heat capacity of the calorimeter.heat capacity of calorimeter =c* ןנ A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat ofcombustion of fuels and the energy available from foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heatcapacity of the calorimeter. This is known as calibrating the calorimeter.In the laboratory a student burns a 0.459-g sample of decanoic acid (C10H2002) in a bombcalorimeter containing 1120. g water. The temperature increases from 24.70 °C to 27.60 °C. Thespecific heat capacity of water is 4.184 J g-l °C•!.The combustion enthalpy is -6080. kJ/mol decanoic acid.C10H2002(s) + 14 O2(g)→10 CO2(g) + 10 H2O(1) A,H° = -6080. kJ/mol%3DCalculate the heat capacity of the calorimeter.heat capacity of calorimeter =c* ןנ

The heat released in the bomb calorimeter is at constant volume, i.e., change in internal energy and…

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.971-g sample of dimethyl oxalate (C4H,O4) in a bomb calorimeter containing 1050. g water. The temperature increases from 25.40 °C to 28.00 °C. The specific heat capacity of water is 4.184 J g-l °C*!. The combustion enthalpy is –1675 kJ/mol dimethyl oxalate. CĄHGO4(s) + 7/2 O2(g) 4 CO2(g) + 3 H2O(1) A,H° = -1675 k)/mol Calculate the heat capacity of the calorimeter.

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.971-g sample of dimethyl oxalate (C4H,O4) in a bomb calorimeter containing 1050. g water. The temperature increases from 25.40 °C to 28.00 °C. The specific heat capacity of water is 4.184 J g-l °C*!. The combustion enthalpy is –1675 kJ/mol dimethyl oxalate. CĄHGO4(s) + 7/2 O2(g) 4 CO2(g) + 3 H2O(1) A,H° = -1675 k)/mol Calculate the heat capacity of the calorimeter.

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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