A hypothetical reaction, A2 +B2  2AB mechanism as given below;

A2 A+ A          ............(Fast)

A+B2 → AB + B   ............(Slow)

A+ → AB         ............(Fast)

The order of the overall reaction is:

1. 2

2. 1

3. 1.5

4. zero

Subtopic:  Order, Molecularity and Mechanism |
 55%
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Following mechanism has been proposed for a reaction,

2A+B D+E

A+B C+D    ...(Slow)

A+ C E         ...(Fast)

The rate law expression for the reaction is:

1. r = K[A]2[B]

2. r=K[A][B]

3. r= K[A]2

4. r= K[A][C]

Subtopic:  Definition, Rate Constant, Rate Law |
 75%
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In gaseous reactions important for the understanding of the upper atmosphere H2O and O react bimolecularly to form two OH radicals. H for this reaction is 72kJ at 500 K and Ea is 77 kJ mol-1, then Ea for the bimolecular recombination of two OH radicals to form H2O and O is:

1. 3 kJ mol-1

2. 4 kJ mol-1

3. 5 kJ mol-1

4. 7 kJ mol-1

Subtopic:  Arrhenius Equation |
 70%
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For a reaction A           Product, rate law is -d[A]dt=K[A]0. The concentration of A left after time t when t=1K is:

1. [A]0e

2. [A]0 ×e

3. [A]0e2

4. 1[A]0

Subtopic:  First Order Reaction Kinetics |
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For an exothermic chemical process occurring in two steps as;

(i) A+BX(Slow)

(ii) XAB (Fast)

The progress of the reaction can be best described by:

1. 2.
3. 4. All of the above.

Subtopic:  Arrhenius Equation |
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For a non-stoichiometric reaction 2A + B  C +D, the following kinetic data were obtained in three separate experiments, all at 298 K.

 Initial 

Concentration (A)

 Initial Concentration (B)  Initial rate of formation of C (mol L-1 S-1)
         0.1 M         0.1 M  1.2×10-3
         0.1 M         0.2 M 1.2×10-3
         0.2 M         0.1 M  2.4×10-3

The rate law for the formation of C is:

1. d[C]/dt = k[ A][B]

2. d[C]/dt = k[ A]2[B]

3. d[C]/dt = k[ A][B]2

4. d[C]/dt = k[ A]

Subtopic:  Order, Molecularity and Mechanism |
 66%
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For the reaction N2 + 3H2  2NH3, the rate d[NH3]dt= 2 x 10-4 M s-1 .Therefore, the rate -d[N2]dt is given as:

1. 10-4 Ms-1

2. 104 Ms-1

3. 10-2 sM-1

4. 10-4 sM-1

Subtopic:  Definition, Rate Constant, Rate Law |
 84%
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If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→  AB *, the rate of formation of AB * is directly proportional to:

1. c

2. I

3. I2

4. cI

Subtopic:  Definition, Rate Constant, Rate Law |
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Which curve represents zero order reaction?

1. 

2. 

3. 

4. 

Subtopic:  Order, Molecularity and Mechanism |
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In a reaction, the rate expression is, rate = K[A][B]2/3[C]0, the order of the reaction is:

1. 1

2. 2

3. 5/3

4. zero

Subtopic:  Order, Molecularity and Mechanism |
 91%
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