🤓 Based on our data, we think this question is relevant for Professor Hernandez's class at UCF.
We’re being asked to determine the standard enthalpy change of formation (ΔH˚f) for nitromethane.
Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:
We are given with the following information:
Top fuel dragsters and funny cars burn nitromethane as fuel according to the following balanced combustion equation: 2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g), ΔH˚rxn = –1418 kJ. The standard enthalpy of combustion for nitromethane is –709.2 kJ/mol. Calculate the standard enthalpy of formation (ΔH˚f) for nitromethane.