For the reaction 2NO2 + F2 → 2NO2F, following

mechanism has been provided,

 NO2 + F2   slow  NO2F+F

NO2 + F   fast NO2F

Thus, rate expression of the above

reaction can be written as:

1. r = K[NO2]2[F2]

2. r = K[NO2 ][F2]

3. r = K[NO2]

4. r = K[F2]

Subtopic:  Definition, Rate Constant, Rate Law |
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For the reaction:

[Cu(NH3)4]2+ + H2O[Cu(NH3)3H2O]2+ + NH3

the net rate of reaction at any time is given by, net rate =

2.0x10-4 [Cu(NH3)4]2+[H2O] - 3.0x105 [Cu(NH3 )3 H20]2+[NH3]

Then correct statement is/are :

1. rate constant for forward reaction = 2 x 10-4

2. rate constant for backward reaction = 3 x 105

3. equilibrium constant for the reaction = 6.6 x 10-10

4. all of the above

Subtopic:  Definition, Rate Constant, Rate Law |
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Rate constant of reaction can be expressed by Arrhenius equation as,

                             K=Ae-EaRT   

In this equation, Ea represents:

1. the energy above which all the colliding molecules will react

2. the energy below which colliding molecules will not react

3. the total energy of the reacting molecules at a temperature, T

4. the fraction of molecules with energy greater than the activation energy of the reaction

Subtopic:  Arrhenius Equation |
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Consider the chemical reaction,

N2g+3H2g2NH3g

The rate of this reaction can be expressed in terms of time derivative of concentration of  N2 g, H2g and NH3g.

The correct relationship amongest the rate expressions is: 

(1) Rate =-dN2dt=-13 dH2dt=12 dNH3dt

(2) Rate =-dN2dt=-3 dH2dt=2 dNH3dt

(3) Rate =dN2dt=13 dH2dt=12 dNH3dt

(4) Rate =-dN2dt=- dH2dt= dNH3dt

Subtopic:  Definition, Rate Constant, Rate Law |
 92%
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For a first order reaction A Product, the initial concentration of A is 0.1 M and after 40 minute it becomes 0.025 M. Calculate the rate of reaction at reactant concentration of 0.01M:

1. 3.47x10-4 M min-1

2. 3.47x10-5 M min-1

3. 1.735 x 10-6 M min-1

4. 1.735 x10-4 M min-1

Subtopic:  First Order Reaction Kinetics |
 62%
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Select the intermediate in the following reaction mechanism:

O3(g)  O2(g) +O(g)

O(g) +O3(g)  2O2(g)

1. O3(g)

2. O(g)

3. O2(g)

4. none of these

Subtopic:  Definition, Rate Constant, Rate Law |
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A reactant with initial concentration 1.386 \(\mathrm{mol} \text { litre }{ }^{-1}\) showing first order change takes 40 minute to become half. If it shows zero order change taking 20 minute to becomes half under similar conditions, the ratio, K1/K0 for first order and zero order kinetics will be:

1. 0.5 mol-1 litre

2. 1.0 mol/litre

3. 1.5 mol/litre

4. 2.0 mol-1 litre

Subtopic:  First Order Reaction Kinetics |
 75%
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In a first order reaction, the concentration of the reactant is decreased from 1.0 M to 0.25M in 20 minute. The rate constant of the reaction would be:

1. 10min-1

2. 6.931 min-1

3. 0.6931 min-1

4. 0.06931 min-1

Subtopic:  First Order Reaction Kinetics |
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The following mechanism has been proposed for the reaction of NO with Br2 to form NOBr:

NO(g) + Br2(g)  NOBr2(g)

NOBr2(g) + NO(g) 2NOBr(g)

If the second step is the rate determining step, the order of the reaction with respect to NO(g) will be:

1. 1

2. 0

3. 3

4. 2

Subtopic:  Order, Molecularity and Mechanism |
 56%
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For the reaction A           nB, at the point of intersection of two curves show, the [B] is can be given by:

1. nA02

2. A0n-1

3. nA0n+1

4. n-1n+1A0

Subtopic:  First Order Reaction Kinetics |
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