The reaction 2NO2 Cl - 2NO2 -Cl2 follows the rate law-Rate - k-NO2 Cl- The mechanism is-1st step- NO2 Cl k1- NO2 -Cl2nd step- NO2 Cl - Clk2- NO2 -Cl2Which is the rate determining step-

The correct option is D 1st stepThe rate law expression is = k[NO_2 Cl] . #160;This does not contain the term corresponding to the concentration of Cl. ...

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Standard XII

Chemistry

Activation Energy

The reaction ...

Question

The reaction $2 N O_{2} C l \to 2 N O_{2} + C l_{2}$ follows the rate law,
Rate $= k [N O_{2} C l]$

The mechanism is,
1st step: $N O_{2} C l_{1} N O_{2} + C l$
2nd step: $N O_{2} C l + C l_{2} N O_{2} + C l_{2}$

Which is the rate determining step?

2nd step

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1st step

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Both steps

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None of the above

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Solution

The correct option is D 1st step
The rate law expression is $= k [N O_{2} C l]$ . This does not contain the term corresponding to the concentration of Cl. Hence, the second step is not the rate determining step. The first step is the rate determining step.

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Similar questions

Q. Reaction between NO and

O_{2}

to form

N O_{2} + O_{2} \to 2 N O_{2}

follows the following mechanism:

First step :

N O + N O ⇌ N_{2} O_{2}

(in rapid equilibrium)

Here,

K_{1}

is the rate constant for forward reaction while

K_{- 1}

is the rate constant for backward reaction.

Second step :

N_{2} O_{2} + O_{2}_{2} 2 N O_{2}

(slow)

Determine the rate of reaction.

Q. A two-step mechanism has been suggested for the reaction of nitric oxide and bromine.

N O (g) + B r_{2} (g) K_{1} - \to N O B r_{2} (g)

N O B r_{2} (g) + N O (g) K_{2} - \to 2 N O B r (g)

The observed rate law is, rate

= k [N O]^{2} [B r_{2}]

. Hence, the rate-determining step is :

Q. Which of the following elementary reaction mechanism steps is least likely to be the rate determining step in a mechanism?

Q. In a reaction mechanism consisting of elementary reaction steps where the relative rate of each is given, which of the following is most likely to be the rate-determining step?

Q. Mechanism of the reaction

2 N O + C l_{2} \to 2 N O C l

may be written as

2 N O K ⇌ (N O)_{2} . . . . . . . . . . (f a s t)

(N O)_{2} + C l_{2} k ⟶ 2 N O C l . . . . . . . (s l o w)

Rate equation would be:

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The reaction 2NO2Cl→2NO2+Cl2 follows the rate law,Rate =k[NO2Cl] The mechanism is,1st step: NO2Clk1→NO2+Cl2nd step: NO2Cl+Clk2→NO2+Cl2Which is the rate determining step?

The correct option is D 1st stepThe rate law expression is =k[NO2Cl]. This does not contain the term corresponding to the concentration of Cl. Hence, the second step is not the rate determining step. The first step is the rate determining step.

The reaction $2 N O_{2} C l \to 2 N O_{2} + C l_{2}$ follows the rate law,
Rate $= k [N O_{2} C l]$

The mechanism is,
1st step: $N O_{2} C l_{1} N O_{2} + C l$
2nd step: $N O_{2} C l + C l_{2} N O_{2} + C l_{2}$

Which is the rate determining step?

The correct option is D 1st step
The rate law expression is $= k [N O_{2} C l]$ . This does not contain the term corresponding to the concentration of Cl. Hence, the second step is not the rate determining step. The first step is the rate determining step.