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

The reaction quotient, Qc, can be calculated as: Qc = [SO₃] / [O₂] [SO₂]^2 Substituting the given values, we get: Qc = (10.) / (0.010)^2 (0.010)^2 = 1000 Since Qc > K_c, the reaction is not at equilibrium and it proceeds in the direction that consumes the excess of SO₃ and produces more O₂ and SO₂. This corresponds to the reverse reaction, i.e., the reaction proceeds right to left, and the answer is C.

At 700 K, the Reaction 2SO2(g)+ O2(g) 2SO3(g)has the Equilibrium

At 700 K, the Reaction 2SO₂(g)+ O₂(g) 2SO₃(g)has the Equilibrium