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 1.5880 g sample of fumaric acid (C4H404) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.380x10³ g of water. During the combustion the temperature increases from 21.68 to 24.27 °C. The heat capacity of water is 4.184 ) g1¹ec1. The heat capacity of the calorimeter was determined in a previous experiment to be 954.8 1/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of fumaric acid based on these data. C₂H4O4(s) + 30₂(g) 2 H₂O(l) + 4 CO₂(g) + Energy Molar Heat of Combustion = kJ/mol

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 1.5880 g sample of fumaric acid (C4H404) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.380x10³ g of water. During the combustion the temperature increases from 21.68 to 24.27 °C. The heat capacity of water is 4.184 ) g1¹ec1. The heat capacity of the calorimeter was determined in a previous experiment to be 954.8 1/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of fumaric acid based on these data. C₂H4O4(s) + 30₂(g) 2 H₂O(l) + 4 CO₂(g) + Energy Molar Heat of Combustion = kJ/mol

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 88QAP: A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is...

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