heat evolved per mole of.........?

Question

A 2.885 g sample of methanol, CH3OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 11.38 K. If the heat capacity of the bomb is 727.1 J/K and it contains 1.200 kg of water, what is the heat evolved per mole of methanol combusted? The specific heat capacity of water is 4.184 J/g·K and the molar mass of methanol is 32.04 g/mol.

a.-726.5 kJ/mol
b.-634.5 kJ/mol
c.-91.89 kJ/mol
d.-1.019 × 106 kJ/mol
e.-65.41 kJ/mol

Answer 1

This may take a while, so be patient:

First, calculate the heat absorbed by the bomb and the water:

Bomb:
11.38 K X 727.1 J/K = 8274 J
Water:
1200 g X 4.184 J/g-K X 11.38 K = 57137 J

Total heat absorbed = 65411 J

Total heat released = -65.41 kJ

Now, convert the heat released by the combustion into kJ/mol

2.885 g/32.04 g/mol = 0.09004 mol methanol

-65.41 kJ/0.09004 mol = -726.5 kJ/mol

Answer 2

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Answer 3

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