Consider the reaction: NH₄HS(s) ⇌ NH₃(g) + H₂S(g) At a certain temperature, K_c = 8.5⨉10^-3. A reaction mixture at this temperature containing solid NH₄HS has [NH₃] = 0.166 M and [H₂S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

검증된 단계별 안내

Identify the reaction and the equilibrium constant expression: NH4HS(s) ⇌ NH3(g) + H2S(g). The equilibrium constant expression is K_c = [NH3][H2S].

Substitute the given concentrations into the equilibrium expression: K_c = (0.166)(0.166).

Calculate the reaction quotient, Q, using the initial concentrations: Q = [NH3][H2S] = (0.166)(0.166).

Compare the calculated Q with the given K_c value (8.5 \(\times\) 10^{-3}).

Determine the direction of the reaction: If Q < K_c, the reaction will proceed to the right, decomposing more solid NH4HS. If Q > K_c, the reaction will proceed to the left, forming more solid NH4HS.

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주요 개념

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Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations. Understanding equilibrium is crucial for predicting how changes in concentration, pressure, or temperature will affect the position of the equilibrium.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their coefficients in the balanced equation. For the reaction NH4HS(s) ⇌ NH3(g) + H2S(g), Kc = [NH3][H2S] / [NH4HS]. A small Kc value, like 8.5 * 10^-3, indicates that at equilibrium, the concentration of products is much lower than that of reactants, suggesting that the reaction favors the formation of reactants.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. In the context of the given reaction, if the concentration of NH3 and H2S is increased, the system will shift to favor the formation of NH4HS, leading to the decomposition of some solid NH4HS to reach equilibrium.

Consider the reaction: NH4HS(s) ⇌ NH3(g) + H2S(g) At a certain temperature, Kc = 8.5⨉10-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Chemical Equilibrium

Equilibrium Constant (Kc)

Le Chatelier's Principle