Methanol is often used as a model fuel for laboratory combustion studies. The enthalpy of combustion of liquid methanol at constant pressure is ΔHcomb=−726kJ mol−1. A laboratory burner is filled with 15.0g of CH₃OH and burned completely under conditions where heat losses are negligible.
(a) Determine the number of moles of methanol consumed.
(b) Calculate the total enthalpy change q (in kilojoules) associated with the combustion of this sample.
(c) Many energy devices report output in kilowatt-hours (kWh). Convert the magnitude of q from part (b) to kWh. (1 kWh = 3.60×103kJ.)