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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Select the intermediate in the following reaction mechanism:

O3(g)  O2(g) +O(g)

O(g) +O3(g)  2O2(g)

1. O3(g)

2. O(g)

3. O2(g)

4. none of these

Subtopic:  Definition, Rate Constant, Rate Law |
 79%
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A reactant with initial concentration 1.386 \(\mathrm{mol} \text { litre }{ }^{-1}\) showing first order change takes 40 minute to become half. If it shows zero order change taking 20 minute to becomes half under similar conditions, the ratio, K1/K0 for first order and zero order kinetics will be:

1. 0.5 mol-1 litre

2. 1.0 mol/litre

3. 1.5 mol/litre

4. 2.0 mol-1 litre

Subtopic:  First Order Reaction Kinetics |
 75%
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In a first order reaction, the concentration of the reactant is decreased from 1.0 M to 0.25M in 20 minute. The rate constant of the reaction would be:

1. 10min-1

2. 6.931 min-1

3. 0.6931 min-1

4. 0.06931 min-1

Subtopic:  First Order Reaction Kinetics |
 74%
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The following mechanism has been proposed for the reaction of NO with Br2 to form NOBr:

NO(g) + Br2(g)  NOBr2(g)

NOBr2(g) + NO(g) 2NOBr(g)

If the second step is the rate determining step, the order of the reaction with respect to NO(g) will be:

1. 1

2. 0

3. 3

4. 2

Subtopic:  Order, Molecularity and Mechanism |
 56%
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For the reaction A           nB, at the point of intersection of two curves show, the [B] is can be given by:

1. nA02

2. A0n-1

3. nA0n+1

4. n-1n+1A0

Subtopic:  First Order Reaction Kinetics |
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The rate constant of a first-order reaction is\(4 \times 10^{-3} \mathrm{sec}^{-1}.\) At a reactant concentration of \(0.02~\mathrm{M},\) the rate of reaction would be:

1. \(8 \times 10^{-5} \mathrm{M} ~\mathrm{sec}^{-1} \) 2. \(4 \times 10^{-3} \mathrm{M} ~\mathrm{sec}^{-1} \)
3. \(2 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1} \) 4. \(4 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1}\)
Subtopic:  First Order Reaction Kinetics |
 79%
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If concentration of reactants is increased by 'X', the rate constant K becomes:

1. eK/X

2. K/X

3. K

4. X/K

Subtopic:  Definition, Rate Constant, Rate Law |
 71%
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In acidic medium the rate of reaction between BrO3- and Br- ions is given by the expression

-d[BrO3-]dt=KBrO3-Br-H+2

It means:

1. The rate constant of the overall reaction is 4 sec-1.
2. The rate of reaction is independent of the concentration of the acid.
3. The change in pH of the solution will not affect the rate.
4. Doubling the concentration of H+ ions will increase the rate of reaction by 4 times.
Subtopic:  Definition, Rate Constant, Rate Law |
 75%
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A graph plotted between log (t) 50% vs. log (a) concentration is a straight line. What conclusion can you draw from the given graph?

1. n=1, t1/2 = 1/K.a

2. n=2, t1/2 = 1/a

3. n=1, t1/2 = 0.693/K

4. None of the above

Subtopic:  Order, Molecularity and Mechanism |
 84%
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