At 218°C, 𝐾_𝑐= 1.2×10⁻⁴ for the equilibrium NH₄SH(𝑠) ⇌ NH₃(𝑔) + H₂S(𝑔) (a) Calculate the equilibrium concentrations of NH₃ and H₂S if a sample of solid NH₄SH is placed in a closed vessel at 218°C and decomposes until equilibrium is reached.

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Identify the equilibrium expression for the reaction: NH_4SH(s) ⇌ NH_3(g) + H_2S(g). Since NH_4SH is a solid, it does not appear in the equilibrium expression. Therefore, K_c = [NH_3][H_2S].

Let x be the equilibrium concentration of NH_3 and H_2S. Since the stoichiometry of the reaction is 1:1, [NH_3] = x and [H_2S] = x at equilibrium.

Substitute the equilibrium concentrations into the equilibrium expression: K_c = x * x = x^2.

Set the equilibrium constant equal to the expression: 1.2 \(\times\) 10^{-4} = x^2.

Solve for x by taking the square root of both sides to find the equilibrium concentrations of NH_3 and H_2S.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) 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 the reaction NH₄SH(s) ⇌ NH₃(g) + H₂S(g), Kc = [NH₃][H₂S] / [NH₄SH]. Since NH₄SH is a solid, its concentration does not appear in the expression, simplifying the calculation of equilibrium concentrations.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. In this case, the introduction of solid NH₄SH will shift the equilibrium position to favor the formation of NH₃ and H₂S until the concentrations stabilize according to the Kc value.

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. For the decomposition of NH₄SH, the stoichiometry indicates that one mole of NH₄SH produces one mole of NH₃ and one mole of H₂S. This relationship is crucial for calculating the equilibrium concentrations based on the initial amount of solid NH₄SH and the changes that occur as the system reaches equilibrium.

At 218°C, 𝐾𝑐 = 1.2×10−4 for the equilibrium NH4SH(𝑠) ⇌ NH3(𝑔) + H2S(𝑔) (a) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218°C and decomposes until equilibrium is reached.