At constant volume, the heat of combustion of a particular compound is -3152.0 kj/mol. When 1.321 of the compound (molar mass = 116.30 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 8.223 C. what is the heat capacity (calorimeter constant) of the calorimeter?
So for this question, you want to use q = m*s*(delta)T.
First change the 1.321g of the compound into moles using the molar mass.
Next use that amount of moles to calculate the energy released using the given heat of combustion (# of moles * kJ/mol)
Knowing that the heat released from the reaction is absorbed by the calorimeter (q(compound)=-q(calorimeter)). We can then use the equation listed above to solve for s (the heat capacity).
Hope this helps!