At constant volume, the heat of combustion of a particular compound is –3949.0 kJ/mol. When 1.331 g of this compound (molar mass = 141.44 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 3.837 °C. What is the heat capacity (calorimeter constant) of the calorimeter?

Answer 1

You change the sign of qcombustion rxn so that qcal = -qrxn.
qcal = Ccal x delta T
q = 3949*1.331/141.44 = ?
Then ? = Ccal*delta T. Solve for Ccal.