At constant volume, the heat of combustion of a particular compound, compound A, is - 3568.0 kJ/mol. When 1.411 g of compound A (molar mass = 115.27 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 3.379 °

c. Using this data, what is the heat capacity (calorimeter constant) of the calorimeter?

Question

Madelyn Christensen

Chemistry

19 October, 05:31

At constant volume, the heat of combustion of a particular compound, compound A, is - 3568.0 kJ/mol. When 1.411 g of compound A (molar mass = 115.27 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 3.379 °

c. Using this data, what is the heat capacity (calorimeter constant) of the calorimeter?

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Answers (1)

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Logan Hall · Answer 1

-3568.0 kJ/mol * 1.411 g / 115.27 g/mol = - 43.67 kJ

Heat capacity of the calorimeter: - 43.67 kJ / 3.379 ° = - 12.92 kJ/deg C

Not 100% sure about my answer