Problem: 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.

FREE Expert Solution

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: 

H°rxn=H°f,products- H°f,reactants



We are given with the following information:

  • 2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g)                ΔH˚rxn = –1418 kJ
  • Enthalpy of combustion of 1 mole of nitromethane: -709.2 kJ/mol
89% (222 ratings)
View Complete Written Solution
Problem Details

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.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Enthalpy of Formation concept. You can view video lessons to learn Enthalpy of Formation. Or if you need more Enthalpy of Formation practice, you can also practice Enthalpy of Formation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Abbasi's class at BC.