# 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?

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###### 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.

87% (55 ratings)
###### 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?

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 Thermochemical Equations concept. You can view video lessons to learn Thermochemical Equations Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems .

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What professor is this problem relevant for?

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

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