Question

To begin the experiment, a bomb calorimeter is filled with 1.11 g CH4 and an excess of oxygen. The heat capacity of the calorimeter, including the bomb and the water, is 4.319 kJ g C⋅°. The initial temperature of the system was 24.85°C, and the final temperature was 35.65°C.
Using the formula ∆H =−M ⋅ C ⋅∆T , solve for the heat of combustion of. 1.11 g CH4.

Answer 1

There are several information's already given in the question. Based on those information's the answer can be easily determined.

M = 1.11 g CH4
C = 4.319 kJ g C⋅°
∆T = 35.65 - 24.85 degree centigrade
     = 10.8 degree centigrade.
Then
∆H =−M ⋅ C ⋅∆T
      = - 1.11 * 4.319 * 10.8
      = - 51.776 kJ/mol

I hope the procedure is clear enough for you to understand.