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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For a first-order reaction A  Products, the rate of reaction at [A] = 0.2 M is 1.0 x 10-2 mol litre-1 min-1. The half-life period for the reaction will be:

1. 832 sec 2. 440 sec
3. 416 sec 4. 14 sec
Subtopic:  First Order Reaction Kinetics |
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The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C, the rate of the reaction increases by about :

1. 10 times

2. 24 times

3. 32 times

4. 64 times

Subtopic:  Definition, Rate Constant, Rate Law |
 86%
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Consider the reaction:

Cl2(aq) + H2S(aq) → S(s) +2H+(aq) +2Cl-(aq)

The rate equation for this reaction is rate = k[Cl2][H2S] Which of these mechanisms is/are consistent with this rate equation?

A. Cl+ H2S → H+ Cl- +Cl+ + HS- (slow)

cl+ + HS- → H+ +Cl- + S (fast)

B. H2 H+ + HS- (fast equilibrium)

Cl2 + HS- → 2Cl- + H+ + S (slow)

1. A only

2. B only

3. Both A and B

4. Neither A nor B

Subtopic:  Definition, Rate Constant, Rate Law |
 66%
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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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