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.

Question

Chemistry

Leanna Eaton

9 March, 12:35

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.

+2

Answers (1)

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Rodrigo Graves · 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.