Given the following reaction at equilibrium, if K_c = 1.90 × 10¹⁹at 25.0 °C, K_p = ________. H₂ (g) + Br₂ (g) 2 HBr (g)

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the given reaction is: K_c = [HBr]2/[H₂][Br₂] Since the equilibrium constant for the forward reaction is given, we can use the expression for the equilibrium constant for the reverse reaction to solve for K_p: K_p = 1/K_c Plugging in the given value for K_c: K_p = 1/1.90 × 10¹⁹ K_p = 5.26 × 10^-20 Therefore, the correct answer is (D) 1.90 × 10¹⁹.

Given the Following Reaction at Equilibrium, If Kc = 1

Given the Following Reaction at Equilibrium, If K_c = 1