A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.52°C. If the heat capacity of the bomb plus water was 8.75 kJ / °C, calculate the molar heat of combustion of methanol.
Heat = C×(∆T)
q = 8.75×5.52
= 48.3 J
∆U = -q/n
= -48.3×1000×32/1.992
= 776 kJ/mol
A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently,...
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