The reaction of hydrogen and oxygen gases produces 15.0 g of water and releases 48.0 kcal of he

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The reaction of hydrogen and oxygen gases produces 15.0 g...

The reaction of hydrogen and oxygen gases produces $15.0 \mathrm{~g}$ of water and releases 48.0 kcal of heat. How much energy is required to decompose $15.0 \mathrm{~g}$ of water into hydrogen and oxygen gases?

Key Concepts

Reversible Reactions and Energy Sign Reversal

Reversible reactions are those in which the reactants form products and the products can revert back to reactants under certain conditions. When such reactions are reversed, the energy change also reverses; an exothermic reaction (which releases energy) becomes endothermic (requiring energy input) when run in reverse. This principle is important in processes like decomposition, where the energy input required is equal in magnitude to the energy released in the formation process.

Stoichiometry in Thermochemical Calculations

Stoichiometry in thermochemistry involves using the mole ratios from a balanced chemical equation to relate the amounts of reactants and products to the energy changes of the reaction. This concept allows for the calculation of energy changes associated with a specific mass or mole quantity of a substance, ensuring that the energy computations are proportionally accurate according to the chemical reaction involved.

Reaction Enthalpy

Reaction enthalpy is the measure of the total heat change during a chemical reaction at constant pressure. It quantifies the energy released in exothermic reactions or absorbed in endothermic reactions and is essential for understanding the energetic feasibility of chemical processes. In reversible reactions, the magnitude of the enthalpy change remains the same, but its sign is reversed when the reaction direction is inverted.

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