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 5.56 kg of nitromethane

From the balanced reaction, we are given that 1418 kJ of heat is released for every 2 moles of nitromethane (CH3NO2) reacted.

So first calculate the moles of CH3NO2:

moles CH3NO2 = 5560 g / (61.04 g/mol)

moles CH3NO2 = 91.1 mol

 

So total heat released is:

total heat = (-1418 kJ / 2mol) * 91.1 mol

total heat = -129,162.52 kJ = -129.16 MJ

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