The equilibrium constant for the dissociation of molecular iodine, I₂(g) ⇌ 2 I(g), at 800 K is K_c = 3.1 × 10^–5. (a) Which species predominates at equilibrium I₂ or I?

검증된 단계별 안내

Understand the equilibrium expression for the reaction: I2(g) ⇌ 2 I(g). The equilibrium constant, Kc, is given for this reaction.

Write the expression for the equilibrium constant Kc:

K_{c} = \frac{{[I]}^{2}}{[I2]}

. This expression relates the concentrations of the products and reactants at equilibrium.

Consider the value of Kc = 3.1 × 10^–5. A small Kc value indicates that the equilibrium position favors the reactants over the products.

Analyze the equilibrium position: Since Kc is much less than 1, the concentration of I2(g) is greater than the concentration of I(g) at equilibrium.

Conclude which species predominates: Given the small value of Kc, I2(g) predominates at equilibrium over I(g).

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주요 개념

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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 dissociation of I2, Kc = [I]^2 / [I2]. A small Kc value, like 3.1 × 10^–5, indicates that at equilibrium, the concentration of reactants (I2) is much greater than that of the products (I), suggesting that the reaction favors the formation of 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 to counteract the change and restore a new equilibrium. In the context of the dissociation of I2, if the concentration of I is increased or the temperature is altered, the equilibrium will shift to either the right (producing more I) or the left (producing more I2) to minimize the disturbance.

Predominance of Species at Equilibrium

To determine which species predominates at equilibrium, one must compare the concentrations of the reactants and products using the equilibrium constant. A Kc value significantly less than 1 indicates that the reactants are favored, meaning that at equilibrium, the concentration of I2 will be much higher than that of I, confirming that I2 predominates in this reaction.

The equilibrium constant for the dissociation of molecular iodine, I2(g) ⇌ 2 I(g), at 800 K is Kc = 3.1 × 10–5. (a) Which species predominates at equilibrium I2 or I?