The equilibrium constant Kp for the synthesis of ammonia N2(g)+3 H2(g) ⇌2 NH3(g) is 4.3 ×10^-3 a

step 1 Told that the KP, the equilibrium expression, will define it as a partial pressure of NH3 square

The equilibrium constant Kp for the synthesis of ammonia...

The equilibrium constant $K_{\mathrm{p}}$ for the synthesis of ammonia $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$ is $4.3 \times 10^{-3}$ at $300^{\circ} \mathrm{C} .$ What is the value of $K_{\mathrm{p}}$ at $300^{\circ} \mathrm{C}$ for the following equilibrium? $$ \frac{1}{2} \mathrm{N}_{2}(g)+\frac{3}{2} \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{NH}_{3}(g) $$

The equilibrium constant $K_{\mathrm{p}}$ for the synthesis of ammonia
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)
$$
is $4.3 \times 10^{-3}$ at $300^{\circ} \mathrm{C} .$ What is the value of $K_{\mathrm{p}}$ at $300^{\circ} \mathrm{C}$ for the following equilibrium?
$$
\frac{1}{2} \mathrm{N}_{2}(g)+\frac{3}{2} \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{NH}_{3}(g)
$$

Key Concepts

Scaling of Equilibrium Constants in Manipulated Reactions

When a chemical equation is scaled by multiplying all its stoichiometric coefficients by a factor, the equilibrium constant for the modified reaction is obtained by raising the original equilibrium constant to a power equal to that factor. This rule allows one to calculate the equilibrium constant for reactions that are a fraction or multiple of the original balanced reaction, as the exponentiation reflects the proportional change in the mole ratios of the species involved.

Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationship between the reactants and products in a chemical reaction, as determined by the balanced chemical equation. It governs how the concentrations or partial pressures of reactants and products are interrelated, and it is essential when defining the form of the equilibrium constant expression.

Equilibrium Constant

An equilibrium constant is a numerical value that relates the concentrations or pressures of products and reactants at equilibrium for a reversible reaction. For gas-phase reactions under constant temperature, the equilibrium constant expressed in terms of partial pressures (Kp) quantifies the ratio of the product of the pressures of the products to that of the reactants, each raised to the power of their stoichiometric coefficients.

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