Consider the reaction : Cl_(2)(aq)+H_(2)S(aq)toS(s)+2H^(+)(aq)+2Cl^(-)(aq) The rate equation for this reaction is rate =k[Cl_(2)][H_(2)S] Which of these mechanisms is/are consistent with this rate equation ? A. Cl_(2)+H_(2)StoH^(+)+Cl^(-)+Cl^(+)+HS^(-)("slow"),Cl^(+)+HS^(-)toH^(+)+Cl^(-)+S("fast") B. H_(2)SiffH^(+)+H^(+)HS^(-)("fast equilibrium"),Cl_(2)+HS^(-)to2Cl^(-)+H^(+)+S("slow")

Consider the reaction : Cl_(2)(aq)+H_(2)S(aq)toS(s)+2H^(+)(aq)+2Cl^(-)

1.	Consider the reaction : Cl_(2)(aq)+H_(2)S(aq)toS(s)+2H^(+)(aq)+2Cl^(-)(aq) The rate equation for this reaction is rate =k[Cl_(2)][H_(2)S] Which of these mechanisms is/are consistent with this rate equation ? A. Cl_(2)+H_(2)StoH^(+)+Cl^(-)+Cl^(+)+HS^(-)("slow"),Cl^(+)+HS^(-)toH^(+)+Cl^(-)+S("fast") B. H_(2)SiffH^(+)+H^(+)HS^(-)("fast equilibrium"),Cl_(2)+HS^(-)to2Cl^(-)+H^(+)+S("slow")
Answer» Neither A nor B A only B only Both A and B Solution :(b) : Rate depends upon the slow step. THUS, slow step should involve 1 molecule of `Cl_(2)` and 1 molecule of `H_(2)S`. Hence, A is the CORRECT mechanism.