Assuming steady-state approximation for [Cl] and [COCl], the rate law for the formation of COCl2 is — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

From step (3), d[COCl2]/dt = K5[COCl][$Cl_2$]. Applying SSA on [COCl] gives [COCl] = K3[$CO$][Cl] / (K4 + K5[$Cl_2$]). From the fast equilibrium of $Cl_2$, [Cl] = (K1/K2)^(1/2) [$Cl_2$]^(1/2). Substituting [Cl] and [COCl] yields the rate law in (a).