The reaction below has a K_p value of 3.3 × 10^-5bar.What is the value of K_c for this reaction at 700 K?
$\quad$ $\quad$ 2SO₃(g) ⇌ 2SO₂(g) + O₂(g)

Question

The reaction below has a K_p value of 3.3 × 10^-5bar.What is the value of K_c for this reaction at 700 K? $\quad$$\quad$2SO₃(g)⇌ 2SO₂(g)+ O₂(g)

Quizplus · Accepted Answer

The correct answer is A because Kp = Kc(RT)^Δn, where Δn is the change in the number of moles of gas. In this case, Δn = 2 - 3 = -1, so Kc = Kp/(RT)^Δn = (3.3 × 10^-5 bar)/((0.08314 bar L/mol K)(700 K))^-1 = 5.7 × 10^-7 M.

The Reaction Below Has a Kp Value of 3 \quad \quad

The Reaction Below Has a K_p Value of 3 $\quad$ $\quad$