Rate equation for a second order reaction is:

1. K = (2.303/t) log {a/(a-x)}

2. K = (1/t) log {a/(a-x)}

3. K = (1(a)t-1(ao)t)* 1t(1(a)t1(ao)t)* 1t

4. K = (1/t2) log {a/(a-x)}

Subtopic:  Order, Molecularity and Mechanism |
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For the reaction 2NO2 + F2 → 2NO2F, following

mechanism has been provided,

 NO2 + F2   slowslow  NO2F+F

NO2 + F   fastfast 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-EaRTK=AeEa/RT   

In this equation, EaEa 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,

N2(g)+3H2(g)2NH3(g)N2(g)+3H2(g)2NH3(g)

The rate of this reaction can be expressed in terms of time derivative of concentration of  N2 (g), H2(g)N2 (g), H2(g) and NH3(g).

The correct relationship amongest the rate expressions is: 

(1) Rate =-d[N2]dt=-13 d[H2]dt=12 d[NH3]dt

(2) Rate =-d[N2]dt=-3 d[H2]dt=2 d[NH3]dt

(3) Rate =d[N2]dt=13 d[H2]dt=12 d[NH3]dt

(4) Rate =-d[N2]dt=- d[H2]dt= d[NH3]dt

Subtopic:  Definition, Rate Constant, Rate Law |
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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 |
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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 mol 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 |
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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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