The mechanism for the overall reaction is A2 - B - C A2 - 2A slow 2A - B - C fastIf a catalyst d changes the mechanism to A2 - D - A2D slow A2D - 2A - D fast 2A - B - C fastWhich is the rate expression for the reaction with and without a catalyst -

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Nucleophilic Substitution Reaction

The mechanism...

Question

The mechanism for the overall reaction is
$A_{2} + B \to C$
$A_{2} \to 2 A$ (slow)
$2 A + B \to C$ (fast)
If a catalyst d changes the mechanism to
$A_{2} + D \to A_{2} D$ (slow)
$A_{2} D \to 2 A + D$ (fast)
$2 A + B \to C$ (fast)
Which is the rate expression for the reaction with and without a catalyst ?

r = k^{'} [A_{2}] [D], r = k [A_{2}]

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r = k [A_{2}], r = k^{'} [A_{2}] [D]

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r = k^{'} [A_{2} D], r = k [A_{2}] [B]

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r = k [A_{2}] [B], r = k^{'} [A_{2} D]

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Solution

The correct option is A $r = k^{'} [A_{2}] [D], r = k [A_{2}]$
i. Slow step in the reaction with catalyst is
$A_{2} + D \to A_{2} D (s l o w)$
Hence, r = $k^{'} [A_{2}] [D]$
ii. Slow step in the reaction without catalyst is
$A_{2} \to 2 A (s l o w)$
Hence, r = $k [A_{2}]$

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Similar questions

A reaction : $A_{2} + B \to$ Products, involves the following mechanism :
$A_{2} ⇌ 2 A (f a s t)$ (A being the intermediate)
$A + B \to k_{2} (s l o w)$ .The rate law consistent to this mechanism is :

Q. The reaction

A_{2} + B_{2} \to 2 AB

, is bound to obey the following mechanism

A_{2}_{1} A + A (fast)

A + B_{2}_{2} AB + B (slow)

A + B \to AB (fast)

The order of overall reaction is

Q. The reaction,

2 A + B \to

Products, follows the mechanism:

2 A ⇋ A_{2}

(at equilibrium)

A_{2} + B \to

Products (slow)

The order of the reaction is:

Q. A reaction:

A_{2} + B \to

Products, involves the following mechanism:

A_{2} ⇌ 2 A

(fast)
(

A

being the intermediate)

A + B - \to k_{2}

Products (slow).

The rate law consistent to this mechanism is:

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The mechanism for the overall reaction is A2+B→CA2→2A (slow)2A+B→C (fast)If a catalyst d changes the mechanism toA2+D→A2D (slow)A2D→2A+D (fast)2A+B→C (fast)Which is the rate expression for the reaction with and without a catalyst ?

The correct option is A r=k′[A2][D],r=k[A2]i. Slow step in the reaction with catalyst isA2+D→A2D(slow)Hence, r = k′[A2][D]ii. Slow step in the reaction without catalyst isA2→2A(slow)Hence, r = k[A2]

The correct option is A $r = k^{'} [A_{2}] [D], r = k [A_{2}]$
i. Slow step in the reaction with catalyst is
$A_{2} + D \to A_{2} D (s l o w)$
Hence, r = $k^{'} [A_{2}] [D]$
ii. Slow step in the reaction without catalyst is
$A_{2} \to 2 A (s l o w)$
Hence, r = $k [A_{2}]$