Achieve #12 week 3-4

[Maia V 1L]

Can someone explain the steps to figure this problem out? Thank you.

At constant volume, the heat of combustion of a particular compound, compound A, is −3420.0 kJ/mol. When 1.613 g of compound A (molar mass =123.89 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 5.497 ∘C.

What is the heat capacity (calorimeter constant) of the calorimeter?

[Eszter Kovacs 1A]

you know how much heat is released per mole, so you need to calculate n for the compound in order to calculate the amount of heat that was released in the reaction. The amount of heat that was released in the reaction is taken up by the calorimeter, so you know qcal too. In order to get the heat capacity you just need to calculate qcal/delta T.

[Lily Rivas 1H]

It always proves helpful to remember that the heat capacity of the calorimeter, C , is calculated by dividing the amount of heat released in the calorimeter, q, by the calorimeter's change in temperature, ΔT.
C=q/ΔT