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

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The equilibrium constant (K_eq) for the reaction can be calculated using the Nernst equation:$$K_{eq} = \frac{[Cl^-]^2[Br_2]}{[Cl_2][Br^-]^2}$$At 25°C, the standard reduction potentials for the Cl₂/Cl^- and Br₂/Br^- couples are:$$E°(Cl_2/Cl^-) = 1.36 V$$$$E°(Br_2/Br^-) = 1.09 V$$Using the Nernst equation, we can calculate the equilibrium constant:$$K_{eq} = \frac{[Cl^-]^2[Br_2]}{[Cl_2][Br^-]^2} = \frac{10^{-2(1.36 V)}}{10^{-2(1.09 V)}} = 6.3 * 10^9$$Therefore, the equilibrium constant (K_eq) at 25°C for the reaction is 6.3 * 10⁹.

Determine the Equilibrium Constant (Keq)at 25°C for the Reaction Cl2(g) →\rarr→

Determine the Equilibrium Constant (K_eq)at 25°C for the Reaction Cl₂(g) $\rarr$