A zero order reaction is one:

(1) In which reactants do not react

(2) In which one of the reactants is in large excess

(3) Whose rate does not change with time

(4) Whose rate increases with time

Subtopic:  Order, Molecularity and Mechanism |
 73%
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For A+B C+D, H = -20 kJmol-1 the activation energy of the forward reaction is 85 kJ mol-1. The activation energy for backward reaction is...... kJ mol-1

1. 105

2. 85

3. 40

4. 65

Subtopic:  Arrhenius Equation |
 77%
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For the elementary reaction M  N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M is:

(1) 4

(2) 3

(3) 2

(4) 1

Subtopic:  First Order Reaction Kinetics |
 78%
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The rate constant for a second order reaction is 8x10-5 M-1 min-1 . How long will it take a 1M solution to be reduced to 0.5M?

(1) 8.665 x 103 minute

(2) 8 x 10-5 minute

(3) 1.25 x 104 minute

(4) 4x10-5 minute

Subtopic:  Order, Molecularity and Mechanism |
 67%
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The time for the half-life of a first-order reaction is 1 hr. The time taken for 87.5% completion of the reaction is-

1. 1 hour

2. 2 hour

3. 3 hour

4. 4 hour

Subtopic:  First Order Reaction Kinetics |
 79%
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Which order of reaction obeys the relation t1/2 = 1/Ka?

(a) First

(b) Second

(c) Third

(d) Zero

Subtopic:  Order, Molecularity and Mechanism |
 79%
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The chemical reaction, 2O3 3O2 proceeds as follows;

O3 O2 + O .....(Fast)

O+O3  2O2 ....(Slow)

The rate law expression should be:

(a) r = K[O3]2

(b) r = K[O3]2[O2]-1

(c) r = K[O3][O2]

(d) unpredictable

Subtopic:  Definition, Rate Constant, Rate Law |
 71%
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The rate of reaction becomes 2 times for every 10°C rise in temperature. How the rate of reaction will increase when temperature is increased from 30°C to 80°C?

(a) 16

(b) 32

(c) 64

(d) 128

Subtopic:  Definition, Rate Constant, Rate Law |
 87%
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The fraction of a reactant showing first-order reaction remains after 40 minutes if t1/2 is 20 minutes -

1. 1/4

2. 1/2

c. 1/8

4. 1/6

Subtopic:  First Order Reaction Kinetics |
 77%
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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:

(a) r = K[NO2]2[F2]

(b) r = K[NO2 ][F2]

(c) r = K[NO2]

(d) r = K[F2]

Subtopic:  Definition, Rate Constant, Rate Law |
 89%
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