For the reaction shown here, K_c = 0.513 at 500 K. N₂O₄(g) ⇌ 2 NO₂(g) If a reaction vessel initially contains an N₂O₄concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N₂O₄and NO₂ at 500 K?

검증된 단계별 안내

Set up the initial concentrations of the reactants and products. For N2O4, it is 0.0500 M, and for NO2, it is 0 M since it has not yet formed.

Let x be the change in concentration of N2O4 that reacts to reach equilibrium. The concentration of N2O4 at equilibrium will then be (0.0500 - x) M.

Since the reaction produces 2 moles of NO2 for every 1 mole of N2O4 that reacts, the concentration of NO2 at equilibrium will be (0 + 2x) M.

Write the expression for the equilibrium constant, Kc, in terms of the concentrations of the reactants and products at equilibrium. For the reaction N2O4(g) ⇌ 2NO2(g), Kc = \( \frac{[NO2]^2}{[N2O4]} \).

Substitute the equilibrium concentrations into the Kc expression and solve for x. Use the quadratic formula if necessary. Once x is found, substitute back to find the concentrations of N2O4 and NO2 at equilibrium.

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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 N2O4 ⇌ 2NO2, Kc = [NO2]^2 / [N2O4]. A Kc value less than 1 indicates that at equilibrium, reactants are favored, while a value greater than 1 indicates that products are favored.

ICE Table

An ICE table (Initial, Change, Equilibrium) is a tool used to organize the concentrations of reactants and products at different stages of a chemical reaction. It helps in calculating the changes in concentration as the system reaches equilibrium. By filling in initial concentrations, the changes that occur during the reaction, and the equilibrium concentrations, one can solve for unknown values.

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 is useful in predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in a reaction, such as the one involving N2O4 and NO2.

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2 NO2(g) If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?