Problem: Nitromethane (CH3NO2) burns in air to produce significant amounts of heat: 2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g); ΔH˚rxn = -1418 kJ.How much heat is produced by the complete reaction of 5.29 kg of nitromethane?

FREE Expert Solution

We are asked how much heat is produced by the complete reaction of 5.29 kg of nitromethane.



We'll use the thermochemical equation to calculate the heat produced.

Molar mass CH3NO2 = 61.05 g/mol

2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g); ΔH˚rxn = -1418 kJ.


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Problem Details

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat: 2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g); ΔH˚rxn = -1418 kJ.

How much heat is produced by the complete reaction of 5.29 kg of nitromethane?

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Based on our data, we think this problem is relevant for Professor Holliman's class at Francis Marion University.