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A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.354-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1040. g of water. The temperature increases from 25.10 °C to 27.90 °C. The heat capacity of water is 4.184 J gl°C-!. The molar heat of combustion is –7251 kJ per mole of diphenylacetylene. C14H10(s) + 33/2 0,(g) →14 CO,(g) + 5 H,0(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter J/°C

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.354-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1040. g of water. The temperature increases from 25.10 °C to 27.90 °C. The heat capacity of water is 4.184 J gl°C-!. The molar heat of combustion is –7251 kJ per mole of diphenylacetylene. C14H10(s) + 33/2 0,(g) →14 CO,(g) + 5 H,0(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter J/°C

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.354-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1040. g of water. The temperature increases from 25.10 °C to 27.90 °C. The heat capacity of water is 4.184 J g`I°C•!. The molar heat of combustion is –7251 kJ per mole of diphenylacetylene. C14H10(s) + 33/2 02(g) →14 CO,(g) + 5 H,0(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
Transcribed Image Text:A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.354-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1040. g of water. The temperature increases from 25.10 °C to 27.90 °C. The heat capacity of water is 4.184 J g`I°C•!. The molar heat of combustion is –7251 kJ per mole of diphenylacetylene. C14H10(s) + 33/2 02(g) →14 CO,(g) + 5 H,0(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
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