Calculate the equilibrium constant Kp for the reaction given below if ΔG^∘=-10.632 kJ at 300 K

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Calculate the equilibrium constant Kp for the reaction given...

Calculate the equilibrium constant $K_{\mathrm{p}}$ for the reaction given below if $\Delta G^{\circ}=-10.632 \mathrm{~kJ}$ at $300 \mathrm{~K}$ $$ \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} $$

Calculate the equilibrium constant $K_{\mathrm{p}}$ for the reaction given below if $\Delta G^{\circ}=-10.632 \mathrm{~kJ}$ at $300 \mathrm{~K}$
$$
\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}
$$

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Key Concepts

Standard Gibbs Free Energy Change

This concept refers to the change in Gibbs free energy (?G°) under standard conditions, which indicates the spontaneity of a reaction. A negative ?G° implies that the reaction is spontaneous under standard conditions, and it is used to predict the direction of the reaction's equilibrium.

Equilibrium Constant (Kp)

The equilibrium constant for a reaction, especially in gas-phase reactions, is expressed as Kp and represents the ratio of the partial pressures of the products to that of the reactants at equilibrium. It provides a quantitative measure of the extent to which a reaction will proceed.

Thermodynamic Relationship between ?G° and K

This key concept is the direct relationship defined by the equation ?G° = -RT ln K, where R is the universal gas constant and T is the temperature in Kelvin. This equation bridges thermodynamics and chemical equilibrium, allowing one to calculate the equilibrium constant from the standard Gibbs free energy change.

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