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 part a how much heat is produced by the complete reaction of 4.68 kg of nitromethane
find the number of moles of nitromethane by dividing the given mass by the molar mass
each mole reacted produces 709 kJ of heat
To determine the amount of heat produced by the complete reaction of 4.68 kg of nitromethane (CH3NO2), we can use the equation you provided along with the given enthalpy change (ΔH°rxn) value (-1418 kJ).
The given balanced equation is:
2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g)
First, we need to convert the mass of nitromethane from kilograms to moles. We can use the molar mass of nitromethane to do this conversion.
Molar mass of CH3NO2:
(1 x Mr of C) + (3 x Mr of H) + (1 x Mr of N) + (2 x Mr of O)
= (1 x 12.01 g/mol) + (3 x 1.01 g/mol) + (1 x 14.01 g/mol) + (2 x 16.00 g/mol)
= 61.04 g/mol
Now, we can calculate the number of moles of nitromethane:
Number of moles = Mass / Molar mass
Number of moles = 4680 g / 61.04 g/mol
Number of moles = 76.62 mol
Next, we can use the stoichiometry of the balanced equation to determine the amount of heat produced.
From the balanced equation:
2 moles of CH3NO2 produce -1418 kJ of heat
So, for 76.62 mol of CH3NO2:
1418 kJ / 2 mol = ΔH°rxn / 76.62 mol
Solving for ΔH°rxn:
ΔH°rxn = (1418 kJ / 2 mol) x 76.62 mol
ΔH°rxn = 71,868 kJ
Therefore, the complete reaction of 4.68 kg of nitromethane produces 71,868 kJ of heat.