The time for half-life of a first order reaction is 1 hr. What is the time taken for 87.5% completion of the reaction?

1. 1 hour

2. 2 hour

3. 3 hour

4. 4 hour

Subtopic:  First Order Reaction Kinetics |
 76%
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Which order of reaction obeys the relation t1/2 = 1/Ka?

1. First

2. Second

3. Third

4. Zero

Subtopic:  Order, Molecularity and Mechanism |
 68%
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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:

1. r = K[O3]2

2. r = K[O3]2[O2]-1

3. r = K[O3][O2]

4. unpredictable

Subtopic:  Definition, Rate Constant, Rate Law |
 69%
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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?

1. 16

2. 32

3. 64

4. 128

Subtopic:  Definition, Rate Constant, Rate Law |
 82%
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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 |
 56%
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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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