The rate equation for the reaction 2A+B→C is found to be:
rate = k [A] [B]
The correct statement in relation to this reaction is that the:

1. Unit of k must be s-1
2. t1/2 is a constant
3. Rate of formation of C is twice the rate of disappearance of A
4. Value of k is independent of the initial concentrations of A and B

Subtopic:  Definition, Rate Constant, Rate Law |
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Half-life of substance A following first order kinetics is 5 days. Starting with 100g of A, the amount left after 15 days will be: 

1.  25 g 

2. 50 g 

3. 12.5 g 

4. 6.25 g 

Subtopic:  First Order Reaction Kinetics |
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H2 gas is absorbed on the metal surface like gold, tungsten, etc. This follows ________ order reaction:

1. Third 

2. Second 

3. Zero 

4. First 

Subtopic:  Order, Molecularity and Mechanism |
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The elementary step of the reaction, \(2 \mathrm{Na}+\mathrm{Cl}_2\rightarrow2 \mathrm{NaCl}\) is found to follow 3rd order kinetics. Its molecularity is:

1. 1

2. 2

3. 3

4. 4

Subtopic:  Order, Molecularity and Mechanism |
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The rate constants of a reaction at 500K is 0.02s–1 . The values of Ea is 18.230 kJ. The value of A is-

1. 1.61
2. 1.41
3. 1.81
4. 1.21


 
Subtopic:  Arrhenius Equation |
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For a reaction, A + B → Product; the rate law is given by, r=k[A]1/2[B]2. The order of the reaction is:
1. -1.5 2. 1.5
3. 0.5 4. 2.5
Subtopic:  Order, Molecularity and Mechanism |
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Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:

1. L mol–1 s–1

2. no unit

3. mol L–1s–1

4. s–1

Subtopic:  Order, Molecularity and Mechanism |
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For the reaction, A + B → Products
Experiment [A] [B] Rate (mole litre-1 min-1)
1. 0.01 0.01 2 × 10-4
2. 0.02 0.01 4 × 10-4
3. 0.01 0.02 8 × 10-4
The rate law and unit of rate constant respectively, are:
 
1. Rate = K [A]2 [B] and litre2 mole-2 min-1
2. Rate = K [A]3 and litre2 mole-2 min-1
3. Rate = K [A] [B]2 and litre mole-1 min-1
4. Rate = K [A] [B]2 and litre2 mole-2 min-1
Subtopic:  Order, Molecularity and Mechanism |
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The time for the half-life period of a certain reaction A → Products is 1 hour. When the initial concentration of the reactant 'A' is 2.0 mol L-1, the time taken for its concentration to come from 0.50 to 0.25 mol L-1,if it is a zero-order reaction, is:

1. 1h

2. 4 h

3. 0.5 h

4. 0.25 h

Subtopic:  Order, Molecularity and Mechanism |
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For the non – stoichiometry 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 S)
0.1 M
0.1 M
0.2 M
0.1 M
0.2 M
0.1 M
1.2 × 10–3
1.2 × 10–3
2.4 × 10–3

The rate law for the formation of C is:

1. dcdt=k[A]2[B]

2. dcdt=k[A][B]2

3. dcdt=k[A]

4. dcdt=k[A][B]

Subtopic:  Order, Molecularity and Mechanism |
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