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
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
1 answer
1 answer