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 $\to$ H+ + Cl– + Cl+ + HS– (slow) Cl+ + HS– $\to$ H+ + Cl– + S (fast) (B) H2S $ \Leftrightarrow $ H+ + HS– (fast equilibrium) Cl2 + HS– $\to$ 2Cl– + H+ + S (slow)

Question

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 $\to$ H⁺ + Cl^– + Cl⁺ + HS^– (slow)

Cl⁺ + HS^– $\to$ H⁺ + Cl^– + S (fast)

(B) H₂S $ \Leftrightarrow $ H⁺ + HS^– (fast equilibrium)

Cl₂ + HS^– $\to$ 2Cl^– + H⁺ + S (slow)

B only

Both A and B

Neither A nor B

A only

Solution

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