At constant volume, the heat of combustion of a particular compound is –3350.0 k

Question

At constant volume, the heat of combustion of a particular compound is –3350.0 kJ/mol. When 1.823 g of this compound (molar mass = 146.40 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.563 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

First convert the mass of compound to moles using the molar mass. Next find the amount of heat released by this amount of compound using the heat of combustion. Finally, use the amount of heat (in kilojoules) and the temperature change (in degrees Celsius) to find the calorimeter constant (in kilojoules per degree Celsius).

Explanation / Answer

1.823 g of compound / 146.4 g/mol = 0.0124 mole
amount of heat released by this 0.0124 mole of the compound 0.0124 mole x 3350 kJ/mol = 41.7 kJ
41700 J = ( 6.563 OC ) x Calorimeter constant (J/C)
calorimeter constant = 6356 J/C

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