At constant volume, the heat of combustion of a particular compound, compound A,

Question

At constant volume, the heat of combustion of a particular compound, compound A, is -3214.0 kJ/mol. When 1.125 g of compound A (molar mass = 108.33 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 3.015 degree C. Using this data, what is the heat capacity (calorimeter constant) of the calorimeter? Suppose a 3.243 g sample of a second compound, compound B, was combusted in the same calorimeter, and the temperature rose from 25.01 degree C to 28.68 degree C. What is the heat of combustion per gram of compound B?

Explanation / Answer

Step1 Heat of combustion for 1.125 g = 3214.0 x 1.125/108.33 = 33.37 kJ

Step2 Heat capacity = 33.37/Rise in temperature = 33.37/3.67 = 9.09 kJ/C

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