Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g). A reaction mixture is made containing an initial [SO2Cl2] of 0.020 M. At equilibrium, [Cl2] = 1.2*10^-2 M. Calculate the value of the equilibrium constant (Kc).

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Identify the balanced chemical equation: \( \text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g) \).

Write the expression for the equilibrium constant \( K_c \): \( K_c = \frac{[\text{SO}_2][\text{Cl}_2]}{[\text{SO}_2\text{Cl}_2]} \).

Set up an ICE (Initial, Change, Equilibrium) table to determine the equilibrium concentrations of all species.

Use the given initial concentration of \( \text{SO}_2\text{Cl}_2 \) and the equilibrium concentration of \( \text{Cl}_2 \) to find the change in concentration and calculate the equilibrium concentrations of \( \text{SO}_2 \) and \( \text{SO}_2\text{Cl}_2 \).

Substitute the equilibrium concentrations into the \( K_c \) expression to solve for the equilibrium constant.

Key Concepts

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

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. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. A Kc value greater than 1 indicates that products are favored at equilibrium, while a value less than 1 suggests that reactants are favored.

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 chemical reaction.

Stoichiometry of Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the amounts of substances consumed and produced. In the context of equilibrium, stoichiometry is essential for calculating the concentrations of all species involved, which is necessary for determining the equilibrium constant.

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Consider the reaction: 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) K_p = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br₂ is 126 torr. What is the partial pressure of NOBr in this mixture?

Textbook Question

Consider the reaction: SO₂Cl₂(g) ⇌ SO₂(g) + Cl₂(g) K_p = 2.91⨉10³ at 298 K In a reaction at equilibrium, the partial pressure of SO₂ is 137 torr and that of Cl₂ is 285 torr. What is the partial pressure of SO₂Cl₂in this mixture?

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