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
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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:

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)
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.

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