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]
Create a free account to view solution
View Solution FreeTopic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions
More Chemical Kinetics and Nuclear Chemistry Questions
A reaction involving two different reactants can never be...The movement of colloidal particles, under applied electric current is known as :...Half life is independent of the concentration of A. After 10 min volume of N2 gas is 10 L and after complete reaction is...For the second-order reaction A + B → Products, the rate constant k, is given as$k = \frac{2.303}{(a - b)t}\log\frac{b(a...Increasing order of stability of the +2 oxidationstate of the ions :-...