Heat Capacity

Question

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? 

Answer 1

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!