Consider the reaction : $Cl_2(aq) + H_2S(aq) \to S(s) + 2H^{+}(aq) + 2Cl^{–} (aq)$ The rate equation for this reaction is rate $= k [Cl_2] [H_2S]$ Which of these mechanisms is/are consistent with this rate equation ? <br> (A) $Cl_2 + H_{2}S \to H^+ + Cl^- + Cl^+ + HS^- \;$ (slow) $Cl^{+} + HS^{–} \to H^+ + Cl^- + S (fast)$ <br> $(B)\; H_2S \Leftrightarrow H^+ + HS^- $(fast equilibrium) $Cl_2 + HS^{–} \to 2Cl^{–} +H^+ + S$ (slow)

Question

( A ) A only
( B ) Both A and B
( C ) B only
( D ) Neither A nor B