For the reaction: 2 Cl₂(g)+ 2 H₂O(g)⇌ 4 HCl(g)+ O₂(g),K_p = 6.4 × 10^-6 at 500 K.If a fixed volume is filled with initial concentrations of these gases at 227 °C such that [Cl₂] = 0.5 M,[H₂O] = 0.40 M,[HCl] = 0.5 M,and [O₂] = 0.015 M,in which direction will the reaction proceed? A)The reaction proceeds to the right. B)The reaction proceeds to the left. C)The reaction is already at equilibrium. D)The reaction volume must be specified to answer this question. E)The value of K_p at 25 °C must be specified to answer this question.

Question

Quizplus · Accepted Answer

The reaction quotient can be calculated as:
Q = ([HCl]2[OS]/[Cl2][H2S]) = (0.5)2(0.015)/(0.5)2(0.40) = 0.047

Since Q is less than Kp, the reaction will proceed in the reverse direction to reach equilibrium. Therefore, the reaction will proceed to the left.

For the Reaction: 2 Cl2(g)+ 2 H2O(g)⇌ 4 HCl(g)+ O2(g),Kp

For the Reaction: 2 Cl₂(g)+ 2 H₂O(g)⇌ 4 HCl(g)+ O₂(g),K_p