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Calculate the fuel value of CSH12, given that AH comb=-3535 kJ/mol. kJ/g Part 2 How much heat is released during the combustion of 1.29 kg of C5H12? kJ Part 3 How many grams of CSH12 must be burned to heat 1.00 kg of water from 20.6 °C to 93.0°C? Assume that all the heat released during combustion is used to heat the water. gn

Calculate the fuel value of CSH12, given that AH comb=-3535 kJ/mol. kJ/g Part 2 How much heat is released during the combustion of 1.29 kg of C5H12? kJ Part 3 How many grams of CSH12 must be burned to heat 1.00 kg of water from 20.6 °C to 93.0°C? Assume that all the heat released during combustion is used to heat the water. gn

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.52QE
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Lightweight camping stoves typically use white gad,a mixture of C5 and C6 hydrocarbons 

 

Calculate the fuel value of C5H12, given that AH comb=-3535 kJ/mol. kJ/g Part 2 How much heat is released during the combustion of 1.29 kg of C5H12? kJ Part 3 How many grams of C5H12 must be burned to heat 1.00 kg of water from 20.6 °C to 93.0 °C? Assume that all the heat released during combustion is used to heat the water.
Transcribed Image Text:Calculate the fuel value of C5H12, given that AH comb=-3535 kJ/mol. kJ/g Part 2 How much heat is released during the combustion of 1.29 kg of C5H12? kJ Part 3 How many grams of C5H12 must be burned to heat 1.00 kg of water from 20.6 °C to 93.0 °C? Assume that all the heat released during combustion is used to heat the water.
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