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Ch.7 - Thermochemistry
Chapter 7, Problem 61

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?

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1
Convert the mass of nitromethane (5.56 kg) to grams by multiplying by 1000.
Calculate the number of moles of nitromethane using its molar mass (CH3NO2). The molar mass is the sum of the atomic masses of all atoms in the molecule.
Use the stoichiometry of the balanced chemical equation to determine the relationship between moles of nitromethane and the enthalpy change (ΔH°rxn).
Calculate the total heat produced by multiplying the number of moles of nitromethane by the enthalpy change per mole of reaction (ΔH°rxn).
Ensure the units are consistent and convert the final answer to kilojoules if necessary.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for calculating how much heat is produced when a specific amount of a reactant, like nitromethane, is consumed.
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Enthalpy Change (ΔH)

Enthalpy change (ΔH) represents the heat absorbed or released during a chemical reaction at constant pressure. In this case, the negative value of ΔH indicates that the reaction is exothermic, meaning it releases heat. Understanding ΔH is crucial for calculating the total heat produced from the combustion of nitromethane.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find out how much heat is produced from a given mass of nitromethane, we first need to convert the mass of nitromethane (5.56 kg) into moles using its molar mass, which is essential for applying stoichiometry in the heat calculation.
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Related Practice
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