The enthalpy change for the reaction CH4(g)+2 O2(g) ⟶CO2(g)+2 H2 O(l) is -891 kJ for the reacti

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The enthalpy change for the reaction CH4(g)+2 O2(g)...

The enthalpy change for the reaction $$ \mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ is $-891 \mathrm{~kJ}$ for the reaction as written. a. What quantity of heat is released for each mole of water formed? b. What quantity of heat is released for each mole of oxygen reacted?

The enthalpy change for the reaction
$$
\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)
$$
is $-891 \mathrm{~kJ}$ for the reaction as written.
a. What quantity of heat is released for each mole of water formed?
b. What quantity of heat is released for each mole of oxygen reacted?

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Key Concepts

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a balanced chemical equation. It provides the mole ratios that are essential for determining how much of a reactant is consumed or a product is formed, which in turn allows for the calculation of heat release or absorption on a per mole basis.

Calculating Molar Heat Change

Calculating the molar heat change involves dividing the total reaction enthalpy by the number of moles of a specific reactant or product, as indicated by the stoichiometry of the reaction. This concept is important in thermochemistry because it allows for a standardized comparison of energy changes per mole of a substance, regardless of the overall scaled reaction quantities.

Reaction Enthalpy

Reaction enthalpy refers to the overall heat change that occurs during a chemical reaction under constant pressure. It is a thermodynamic quantity that indicates if a reaction releases heat (exothermic) or absorbs heat (endothermic), and is typically reported in kilojoules for the reaction as a whole.

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