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A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4245g sample of diphenylacetylene (C,4H10) is bumed completely in a bomb calorimeter. The calorimeter is surrounded by 1.397 x 10 g of water. During the combustion the temperature increases from 25.47 to 28.14 °C. The heat capacity of water is 4.184 J g-1°C-.

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4245g sample of diphenylacetylene (C,4H10) is bumed completely in a bomb calorimeter. The calorimeter is surrounded by 1.397 x 10 g of water. During the combustion the temperature increases from 25.47 to 28.14 °C. The heat capacity of water is 4.184 J g-1°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
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A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4245g sample of diphenylacetylene (C,4H10) is bumed completely in a bomb calorimeter. The calorimeter is surrounded by 1.397 x 103 g of water. During the combustion the temperature increases from 25.47 to 28.14 °C. The heat capacity of water is 4.184 J g-oC-!. The heat capacity of the calorimeter was determined in a previous experiment to be 829.3 J/ C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of diphenylacetylene based on these data. C14H,0(5) + (33/2) 0,(g) 5 H,0(1) + 14 CO,(g) + Energy Molar Heat of Combustion = kJ/mol
Transcribed Image Text:A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4245g sample of diphenylacetylene (C,4H10) is bumed completely in a bomb calorimeter. The calorimeter is surrounded by 1.397 x 103 g of water. During the combustion the temperature increases from 25.47 to 28.14 °C. The heat capacity of water is 4.184 J g-oC-!. The heat capacity of the calorimeter was determined in a previous experiment to be 829.3 J/ C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of diphenylacetylene based on these data. C14H,0(5) + (33/2) 0,(g) 5 H,0(1) + 14 CO,(g) + Energy Molar Heat of Combustion = kJ/mol
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 64.34 grams of chromium to 98.72 °C and then drops it into a cup containing 81.95 grams of water at 22.34 °C. She measures the final temperature to be 28.41 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.61 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of chromium. Metal sample Specific Heat (Cr) = J/g°C. %3D 2000 Themman-Brsoks/Col
Transcribed Image Text:In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 64.34 grams of chromium to 98.72 °C and then drops it into a cup containing 81.95 grams of water at 22.34 °C. She measures the final temperature to be 28.41 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.61 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of chromium. Metal sample Specific Heat (Cr) = J/g°C. %3D 2000 Themman-Brsoks/Col
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