Calorimetry problem, not sure how to find heat capacity

A 2.200g sample of quinone (C6H4O2) is burned in a bomb calorimeter. The water surrounding the combustion chamber has a mass of 1.877 kg and a specific heat of 4.18 J g C
The temperature of the water increases from 23.44 C to 30.57 C. What is the combustion per mole of quinone?

The answer is -2.75X10^3 I'm not getting that answer...
I think I have to find the heat capacity first but I'm not sure how to do that

Work out the heat energy change using the equation:
q = mcΔT
q = heat energy change
m = mass
c = specific heat capacity
ΔT = temperature change

q = 1.877 x 4.18 x (30.57 - 23.44) = 55.9409818 kJ

Work out the number of moles of quinone you have using the equation:
n = m / Mr
n = number of moles
m = mass
Mr = molar mass

n = 2.2 / 108.0964 = 0.0203522041 mol

Work out the enthalpy change (combustion per mole) using:
ΔH = -q / n
ΔH = enthalpy change
q = heat energy change (q is negative because combustion is exothermic)
n = number of moles

ΔH = -55.9409818 / 0.0203522041 = -2748.64489 kJ/mol

ΔH = -2.75*10^3 kJ/mol

q = (mass) (temp change) (sp. heat)

q = (1877 g) (7.13) (4.184) = 55994.51384 J

We need to know how many moles of C6H4O2 burned:

2.200 g / 108.0956 g/mol = 0.0203524 mol

The final step:

55994.51384 J / 0.0203524 mol = 2751255 J/mol

-2.75 x 10^3 kJ/mol

I ignore the minus sign (meaning exothermic) until the final answer.