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 6.19 kg of nitromethane?
Answer
71886 kJ of heat is produced
Explanation
2CH3NO2(l) + 3/2O2(g) ------> 2CO2(g) + 3H2O(l) + N2(g)
∆H°rxn = -1418kJ
stoichiometrically , 2moles of CH3NO2 produce 1418kJ of heat
mole = mass/ molar mass
moles of CH3NO2 = 6190g/61.05g/mol = 101.39mol
Heat produced by 101.39 moles of CH3NO2 = ( 1418kJ/2 mol )× 101.39mol = 71886kJ
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...
Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2CH3NO2(l)+3/2O2(g)?2CO2(g)+3H2O(l)+N2(g) ?Horxn = -1418 kJ How much heat is produced by the complete reaction of 5.81kg of nitromethane? Express your answer to three significant figures and include the appropriate units.
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Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 4 CH3NO2 (l) + 3 O2 (g) → 4 CO2 (g) + 6 H2O (l) + 2 N2 (g) , ΔHorxn = -2836 kJ If 1,327 kJ of heat are produced from the burning of nitromethane, how many grams of nitromethane were burned? Enter your numerical answer in units of grams.
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