Asked by lea
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
Part A
How much heat is produced by the complete reaction of 4.93 kg of nitromethane?
Express your answer to three significant figures and include the approp
2CH3NO2(l)+32O2(g)→2CO2(g)+3H2O(l)+N2(g)ΔH∘rxn=−1418kJ
Part A
How much heat is produced by the complete reaction of 4.93 kg of nitromethane?
Express your answer to three significant figures and include the approp
Answers
Answered by
DrBob222
You made a typo on the equation. It should be
2CH3NO2(l) + 3/2O2(g)→2CO2(g)+3H2O(l)+N2(g).......ΔH∘rxn=−1418kJ
1418 kJ is produced by 2*molar mass CH3NO2 or
1418 kJ is produced by 122 g so heat produced by 4.93 kg will be
1418 kJ x (4930/122) = ? kJ
2CH3NO2(l) + 3/2O2(g)→2CO2(g)+3H2O(l)+N2(g).......ΔH∘rxn=−1418kJ
1418 kJ is produced by 2*molar mass CH3NO2 or
1418 kJ is produced by 122 g so heat produced by 4.93 kg will be
1418 kJ x (4930/122) = ? kJ
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