The rate constant (K) for the reaction 2A +B  Product was found to be 2.5x10-5 litre mol-1 sec-1 after 15 sec, 2.60 x10-5 litre mol-1sec-1 after 30 sec and 2.55 x10-5litre mol-1 sec-1 after 50 sec. The order of reaction is:

1. 2

2. 3

3. zero

4. 1

Subtopic:  First Order Reaction Kinetics |
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A reaction A2 + B2  2AB occurs by the following mechanism:

A2  A + A               .....(slow)

A + B2  AB + B       .....(fast)

A + B  AB               .....(fast)

Its order would be:

1. 3/2

2. 1

3. 0

4. 2

Subtopic:  Order, Molecularity and Mechanism |
 62%
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For a given reaction, the presence of a catalyst reduces the energy of activation by 2 kcal at 27 oC. The rate of reaction will be increased by:

1. 20 times

2. 14 times

3. 28 times

4. 2 times

Subtopic:  Arrhenius Equation |
 50%
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What fraction of a reactant showing first order remains after 40 minute if t1/2 is 20 minute?

1. 1/4

2. 1/2

3. 1/8

4. 1/6

Subtopic:  First Order Reaction Kinetics |
 74%
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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

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

Subtopic:  Order, Molecularity and Mechanism |
 55%
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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 |
 86%
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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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