At 700 K, the reaction 2SO₂(g)+ O₂(g) 2SO₃(g)has the equilibrium constant K_c = 4.3 * 10⁶, and the following concentrations are present: [SO₂] = 0.010 M; [SO₃] = 10.M; [O₂] = 0.010 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium?

Question

Quizplus · Accepted Answer

To determine if the mixture is at equilibrium, we need to calculate the reaction quotient (Qc) and compare it to the equilibrium constant (Kc). Qc = [SO₃]^2/[O₂] = (10 M)^2 / (0.010 M) = 10,000 M Since Qc < Kc, the reaction is not at equilibrium and will proceed in the direction to reach equilibrium. To determine the direction, we compare the Qc and Kc values. Qc < Kc, so the reaction needs to form more products to reach equilibrium. Therefore, the reaction will proceed from left to right. So, the correct answer is C.

At 700 K, the Reaction 2SO2(g)+ O2(g)

At 700 K, the Reaction 2SO₂(g)+ O₂(g)