At constant volume, the heat of combustion of a particular compound is –3547.0 kJ/mol. When 1.239 g of this compound (molar mass = 196.58 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.539 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

Answer 1

q = heat combustion
q = heat capacity x delta T
q = Cp x 8.539
delta H = 3547.0 kJ/mol so
q = 3547.0 kJ x (1.239/196.58) = ?
Substitute and solve for Cp.