Consider the reaction CH4+2 O2 ⇌CO2+ 2 H2 O when the reaction occurs at 450 kPa and 3000 K . Det

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Consider the reaction CH4+2 O2 ⇌CO2+ 2 H2 O when the...

Consider the reaction $\mathrm{CH}_{4}+2 \mathrm{O}_{2} \rightleftharpoons \mathrm{CO}_{2}+$ $2 \mathrm{H}_{2} \mathrm{O}$ when the reaction occurs at $450 \mathrm{kPa}$ and $3000 \mathrm{K} .$ Determine the equilibrium partial pressure of the carbon dioxide. The natural logarithms of the equilibrium constant for the reactions $\mathrm{C}+2 \mathrm{H}_{2} \rightleftharpoons \mathrm{CH}_{4}$ and $\mathrm{C}+\mathrm{O}_{2} \rightleftharpoons \mathrm{CO}_{2}$ at $3000 \mathrm{K}$ are 9.685 and $15.869,$ respectively

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in a reversible reaction where the forward and reverse reaction rates are equal, leading to constant concentrations or partial pressures of reactants and products over time. This concept underpins the analysis of reactions in which, after sufficient time, there is no net change in the distribution of species because the system has reached balance.

Equilibrium Constant

The equilibrium constant is a numerical value that relates the concentrations or partial pressures of products and reactants at equilibrium according to the stoichiometry of the balanced chemical equation. It provides a snapshot of the reaction's position at equilibrium and is fundamental in predicting how changes in conditions can shift the equilibrium.

Partial Pressure

Partial pressure is the pressure contributed by an individual gas in a mixture. In chemical equilibrium calculations involving gaseous reactions, partial pressures play a key role, as they are used in the equilibrium expressions to represent the amounts of reactants and products present.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. Understanding stoichiometric coefficients is crucial in equilibrium problems because these coefficients dictate how equilibrium concentrations or partial pressures are related, influencing the equilibrium expression.

Combination of Equilibrium Constants

When an overall reaction can be viewed as the sum of two or more individual reactions, the overall equilibrium constant is obtained by multiplying the equilibrium constants of the individual reactions. This principle, grounded in the laws of thermodynamics and Hess's law, is vital for calculating the equilibrium position of composite reactions using known equilibrium constants.

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