Chemical Kinetics and Nuclear ChemistryHard
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 + H2 → H+ + Cl- + Cl+ + HS- (slow)
Cl+ + HS- → H+ + Cl- + S (fast)
(B) H2S → H+ + HS- (fast equilibrium)
Cl2 + HS- → 2Cl- + H+ + S (slow)
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 + H2 → H+ + Cl- + Cl+ + HS- (slow)
Cl+ + HS- → H+ + Cl- + S (fast)
(B) H2S → H+ + HS- (fast equilibrium)
Cl2 + HS- → 2Cl- + H+ + S (slow)
Options
A.B only
B.Both A and B
C.Neither A nor B
D.A only
Solution
Rate equation is to be derived wrt slow
Step ∴ from mechanism (A)
Rate = k [Cl2] [H2S]
Step ∴ from mechanism (A)
Rate = k [Cl2] [H2S]
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