Is Ammonia synthesized according to the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) with Kp = 5.3 * 10^-5 at 725K?

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Identify the reaction: \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \).

Understand that \( K_p \) is the equilibrium constant for the reaction in terms of partial pressures, given as \( 5.3 \times 10^{-5} \) at 725K.

Write the expression for \( K_p \) for the reaction: \( K_p = \frac{{(P_{NH_3})^2}}{{(P_{N_2})(P_{H_2})^3}} \).

Determine the partial pressures of \( N_2 \), \( H_2 \), and \( NH_3 \) at equilibrium if not provided, or assume initial conditions to calculate them.

Substitute the partial pressures into the \( K_p \) expression to check if the calculated \( K_p \) matches the given \( 5.3 \times 10^{-5} \).

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For gaseous reactions, Kp is calculated using partial pressures. A small Kp value, like 5.3 * 10^-5, indicates that at equilibrium, the concentration of reactants is much greater than that of products, suggesting that the reaction favors the reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle helps predict how changes in concentration, pressure, or temperature will affect the position of equilibrium in a reaction, such as the synthesis of ammonia from nitrogen and hydrogen.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in a reaction, not just at equilibrium. It is calculated using the same formula as Kp but with the current concentrations or partial pressures. By comparing Q to Kp, one can determine the direction in which the reaction will proceed to reach equilibrium: if Q < Kp, the reaction will shift to the right (toward products), and if Q > Kp, it will shift to the left (toward reactants).

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