Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 4 CH3NO2 (1) + 3 O2 (g) → 4 CO2 (g) + 6 H20 (1) + 2 N2 (g) , AH°rxn = -2836 kJ If 1,869 kJ of heat are produced from the burning of nitromethane, how many grams of nitromethane were burned?
Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 4 CH3NO2 (1) + 3 O2 (g) → 4 CO2 (g) + 6 H20 (1) + 2 N2 (g) , AH°rxn = -2836 kJ If 1,869 kJ of heat are produced from the burning of nitromethane, how many grams of nitromethane were burned?
General Chemistry - Standalone book (MindTap Course List)
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.44QP: Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.5000 mol H2S burns...
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First, let's write the data given in the reaction,
4 moles of CH3NO2 burn = -2836
The negative sign of the heat of reaction shows the reaction is heat exothermic that means heat is evolved or produced during the reaction.
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