Question

Methanol is burned in a bomb calorimeter. Liquid water is formed as a product. If 34.0 g of methanol reacts, what is the expected temperature change in a calorimeter with a heat capacity of 6.75 kJ/C

Answer 1

2CH₃OH+ 3O₂ = 2CO₂ + 4H₂O
∆H = 4(-285.8 kJ/mol) + 2(-393.510 kJ/mol) – (2(-201.0 kJ/mol)) = -1528.22 kJ/mol
n(CH₃OH) = 34 g / 32g/mol = 1.0625mol
Q = ∆H*n
Q = 1528.22 kJ/mol* 1.0625mol = 1623.73 kJ
∆t = Q/C
∆t = 1623.73 kJ / 6.75kJ/C = 240.5 C