Chemistry - Chemical Kinetics Question with Solution | TestHub

Consider the reaction : ${\mathrm{Cl}}_2(aq)+{\mathrm{H}}_2\mathrm{S}(aq)\to$ $\mathrm{S}(s)+2{\mathrm{H}}^{+}(aq)+2{\mathrm{Cl}}^{-}(aq)$ The rate equation for this reaction is rate $=k\left[{\mathrm{Cl}}_2\right]\left[{\mathrm{H}}_2\mathrm{S}\right]$ Which of these mechanisms is/are consistent with this rate equation? A. ${\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{S}\to {\mathrm{H}}^{+}+{\mathrm{Cl}}^{-}+{\mathrm{Cl}}^{+}+{\mathrm{HS}}^{-}$ (slow) ${\mathrm{Cl}}^{+}+{\mathrm{HS}}^{-}\to {\mathrm{H}}^{+}+{\mathrm{Cl}}^{-}+\mathrm{S}$ B. ${\mathrm{H}}_2\mathrm{S}\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{HS}}^{-}$ (fast equilibrium) ${\mathrm{Cl}}_2+{\mathrm{HS}}^{-}\to 2{\mathrm{Cl}}^{-}+{\mathrm{H}}^{+}+\mathrm{S}$ (Slow)