Question

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g) ΔHorxn = -1418 kJ How much heat is produced by the complete reaction of 4.35 kg of nitromethane?

Answer 1

Molar mass of CH3NO2,

MM = 1*MM(C) + 3*MM(H) + 1*MM(N) + 2*MM(O)

= 1*12.01 + 3*1.008 + 1*14.01 + 2*16.0

= 61.044 g/mol

mass(CH3NO2)= 4.35 Kg

= 4350 g

number of mol of CH3NO2,

n = mass of CH3NO2/molar mass of CH3NO2

=(4350.0 g)/(61.044 g/mol)

= 71.26 mol

The given reaction is:

2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g) ΔHorxn = -1418 kJ

from this reaction,

when 2 mol of CH3NO2 reacts, heat produced = 1418 kJ

so,

when 71.26 mol of CH3NO2 reacts, heat produced = 1418*71.26/2

= 50523 kJ

Answer: 50523 kJ