Given the equation A(g) B(g) + 2C(g). At a particular temperature, K = 1.4 *10 5 .
-Which of the following is true when the equilibrium constant for a reaction is relatively large?

Question

Given the equation A(g)  B(g) + 2C(g). At a particular temperature, K = 1.4 *10 5 .
-Which of the following is true when the equilibrium constant for a reaction is relatively large?

Quizplus · Accepted Answer

When the equilibrium constant for a reaction is relatively large, it means that the products are favored over the reactants at equilibrium. Therefore, the equilibrium lies to the right. The rate of the forward reaction will be relatively fast and the rate of the reverse reaction will be relatively slow. This means that it will take a long time to reach equilibrium because the forward reaction still needs to occur before equilibrium can be reached. Therefore, option B is not correct. Option A is not correct because the rate at which equilibrium is reached is not related to the equilibrium constant. Option C is not correct because a large equilibrium constant indicates that the products are favored, so the equilibrium cannot lie to the left. Therefore, the correct answer is D.

Given the Equation A(g) B(g) + 2C(g)