finding heat capacity using q=cΔT

[Felicia Fong 2G]

This question is from the 2011 Midterm.
Q1a) The enthalpy of combustion of benzoic acid is -3227 kJ/mol. When 1.453g of benzoic acid was burned in a calorimeter, the temp increased by 2.265 degrees C. What is the heat capacity of the calorimeter?

The solution is:
q=CcalΔT
Ccal=-(mol benzoic acid)(-3227 kJ/mol benzoic acid)/2.265 degrees C
=16.95 kJ/degrees C

Why is there a negative in front of the mol of benzoic acid? Why do you multiply the number of moles of benzoic acid by the enthalpy of combustion instead of dividing? I thought the equation with moles is q=nCcalΔT

[Justin Folk 3I]

The heat capacity is defined as ENERGY per TEMPERATURE

[Ethan Vuong 3G]

Since you are looking for the specific heat capacity, you wouldn't be solving for q, but for Ccal. Therefore, you would divide q by delta T. I am unsure of where the negative comes from though.

[Angela 1K]

It is negative because the q of the calorimeter is going to be the negative of the q of the reaction, which is what we use in the equation.

Hope that makes sense.