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Nitromethane (CH3NO2) burns in air to produce significant amounts of heat via the following reaction: 2CH3NO2(l)+32O2(g)→2CO2(g)+3H2O(l)+N2(g)ΔH∘rxn=−1418kJ How much heat is produced by the complete reaction of 3.78 kg of nitromethane?

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Answer:

-43934.8KJ

Explanation:

From the balanced reaction equation:

122g of nitromethane releases -1418000J of heat

3780g of nitromethane will release 3780 × -1418000/122

=-43934.8KJ

The balanced reaction equation must first be obtained before any calculation since the calculation is based on the stoichiometry of the reaction. The mass in kilogrammes must first be converted to grams and the energy expressed in joules before calculations begin.

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