Determine the equilibrium constant (K_eq) at 25^$\circ$C for the reaction Cl₂(g) + 2Br^- (aq) $\leftrightharpoons$ 2Cl^- (aq) + Br₂(l).

Question

Quizplus · Accepted Answer

The equilibrium constant expression is: K_eq = ([Cl₂] / [Br^-]2) * [Br₂] / [Cl^-]2 At equilibrium, we know that the concentrations of the species are as follows: [Cl2] = 0, [Br-] = [Br2], and [Cl-] = [Br-]. Plugging in these concentrations and using the values from the table for the relevant thermodynamic quantities, we get: K_eq = (1.3 × 10^2)(0.5)^2 / (7.2 × 10^-2)^2 = 6.3 × 10^10 Therefore, the correct answer is B.

Determine the Equilibrium Constant (Keq) at 25 ∘\circ∘ C for the Reaction Cl2(g) + 2Br- (Aq)

Determine the Equilibrium Constant (K_eq) at 25^$\circ$C for the Reaction Cl₂(g) + 2Br^- (Aq)