1. Tardigrade
  2. Question
  3. Chemistry
  4. Consider the reaction: Cl2(aq) + H2S(aq) → S(s) + 2H+(aq) + 2Cl-(aq) The rate equation for this reaction is rate = k [Cl2] [H2S] Which of these mechanisms is/are consistent with this rate equation ? (A) Cl2 + H2S → H+ + Cl- + Cl+ + HS- (slow) Cl+ + HS- → H+ + Cl- + S (fast) (B) H2S leftharpoons H+ + HS- (fast equilibrium) Cl2 + HS- → 2Cl- + H+ + S (slow)

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Q. 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 ?
$\left(A\right) Cl_{2} + H_{2}S \to H^{+} + Cl^{-} + Cl^{+} + HS^{-} $ (slow)
$Cl^{+} + HS^{-} \to H^{+} + Cl^{-} + S $ (fast)
$\left(B\right) H_{2}S \rightleftharpoons H^{+} + HS^{-}$ (fast equilibrium)
$Cl_{2} + HS^{-} \to 2Cl^{-} + H^{+} + S$ (slow)

AIEEEAIEEE 2010Chemical Kinetics

Solution:

Rate equation is to be derived wrt slow
Step $\therefore $ from mechanism (A)
Rate $= k[Cl_2] [H_2S]$