Consider the reaction: SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g) K_c = 2.99⨉10^-7 at 227 °C If a reaction mixture initially contains 0.175 M SO₂Cl₂, what is the equilibrium concentration of Cl₂ at 227 °C?

검증된 단계별 안내

Step 1: Write the expression for the equilibrium constant (Kc) for the reaction. For the reaction SO2Cl2(g) ⇌ SO2(g) + Cl2(g), the expression is Kc = [SO2][Cl2] / [SO2Cl2].

Step 2: Set up an ICE (Initial, Change, Equilibrium) table to track the concentrations of reactants and products. Initially, [SO2Cl2] = 0.175 M, and [SO2] = [Cl2] = 0 M.

Step 3: Let 'x' be the change in concentration of SO2Cl2 that reacts to reach equilibrium. At equilibrium, [SO2Cl2] = 0.175 - x, [SO2] = x, and [Cl2] = x.

Step 4: Substitute the equilibrium concentrations into the Kc expression: Kc = (x)(x) / (0.175 - x).

Step 5: Solve the equation for x, which represents the equilibrium concentration of Cl2.

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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 concentration. Understanding this concept is crucial for analyzing equilibrium constants and predicting the behavior of reactions.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction SO2Cl2(g) ⇌ SO2(g) + Cl2(g), Kc = [SO2][Cl2]/[SO2Cl2]. A small Kc value, like 2.99 * 10^-7, indicates that at equilibrium, the concentration of reactants is much greater than that of products, suggesting that the reaction favors the reactants.

ICE Table (Initial, Change, Equilibrium)

An ICE table is a tool used to organize the initial concentrations, changes in concentrations, and equilibrium concentrations of reactants and products in a chemical reaction. By setting up an ICE table for the given reaction, one can systematically determine the equilibrium concentrations based on the initial conditions and the equilibrium constant. This method simplifies the calculations needed to find unknown concentrations at equilibrium.

Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99⨉10-7 at 227 °C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?