A first-order reaction has a rate constant of 2.303×10-3 s-1. The time required for 40 g of this reactant to reduce to 10 g will be [Given that log102=0.3010]

1. 230.3 s

2. 301 s

3. 2000 s

4. 602 s

Subtopic:  First Order Reaction Kinetics |
 83%
From NCERT
NEET - 2019
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For a reaction, activation energy Ea=0 and the rate constant at 200 K is    1.6 X 106s-1. The rate constant at 400K will be [Given that gas constant, R=8.314 J K-1 mol-1]

1.  3. 2 x 104 s-1
2. 1.6 x 106s-1

3. 1.6 x103 s-1

4. 3.2 x 106 s-1

Subtopic:  Arrhenius Equation |
 76%
From NCERT
NEET - 2019
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For the chemical reaction N2g+3H2g  2NH3g the correct option is:

1. 3dH2dt=2dNH3dt

2. -13dH2dt=-12dNH3dt

3. -dN2dt=2dNH3dt

4. -dN2dt=12dNH3dt

Subtopic:  Definition, Rate Constant, Rate Law |
 82%
From NCERT
NEET - 2019
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If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by:

1. t=2.303/k

2. t=0.693/k

3. t=6.909/k

4. t=4.606/k

Subtopic:  First Order Reaction Kinetics |
 59%
From NCERT
NEET - 2019
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Consider the reaction 
N2(g) + 3H2(g) → 2NH3(g
The equality relationship between \( \frac{{d}\left[{{NH}_{3}}\right]}{dt}\) and \( {-}\frac{{d}\left[{{H}_{2}}\right]}{dt}\) is :

1. d[NH3]dt=-13d[H2]dt

2. +d[NH3]dt=-23d[H2]dt

3. +d[NH3]dt=-32d[H2]dt

4. +d[NH3]dt=-d[H2]dt

Subtopic:  Definition, Rate Constant, Rate Law |
 82%
From NCERT
AIPMT - 2006
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For the reaction, \(2 A+B \rightarrow 3 C+D\)

An incorrect expression for the rate of reaction is:

1. \(-\frac{d[C]}{3} d t \) 2. \(-\frac{d[B]}{d t} \)
3. \(\frac{d[D]}{d t} \) 4. \(-\frac{d[A]}{2 d t}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 90%
From NCERT
AIPMT - 2006
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If 60% of a first-order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately: 
(log 4 = 0.60, log 5 = 0.69)

1. 50 min 2. 45 min
3. 60 min 4. 40 min
Subtopic:  First Order Reaction Kinetics |
 77%
From NCERT
AIPMT - 2007
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In a first order reaction A \(\overset{                         }{\rightarrow}\) B, if k is rate constant and initial concentration of the reactant A is 0.5 M then the half-life is :

(1) \(\frac{0 . 693}{0 . 5 k}\)

(2) \(\frac{log   2}{k}\)

(3) \(\frac{log   2}{k \sqrt{0 . 5}}\)

(4) \(\frac{ln   2}{k}\)

Subtopic:  First Order Reaction Kinetics |
 72%
From NCERT
AIPMT - 2007
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The reaction of hydrogen and iodine monochloride is given as: 
H2(g) + 2ICl(g) → 2HCl(g) + I2(g
This reaction is of first order with respect to H2(g) and ICl(g), for which of the following proposed mechanisms:
Mechanism A: 
H2(g) + 2ICl(g) → 2HCl(g) + I2(g
Mechanism B: 
H2(g) + ICl(g) →HCl(g) + HI(g); slow 
HI(g) + ICl(g) →HCl(g) + I2(g); fast

1. B Only

2. A and B both

3. Neither A nor B

4. A only

Subtopic:  First Order Reaction Kinetics |
 62%
From NCERT
AIPMT - 2007
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The bromination of acetone occurring in an acid solution is represented by the equation. 
CH3COCH3(aq)+ Br2(aq) → 
CH3COCH2Br(aq) + H+(aq) + Br-(aq) 

The kinetic energy data were obtained for given reaction concentrations. 
Initial concentrations, M 
 CH3COCH3   Br2    H+

   0.30             0.05      0.05

   0.30             0.10      0.05

   0.30             0.10      0.10

   0.40             0.05      0.20
Initial rate, the disappearance of Br2, Ms-1 
5.7 × 10-5

5.7 ×  10-5

1.2 × 10-4

3.1 × 10-4
Based on the above data, the rate of the equation is:

1. Rate = k CH3COCH3 H+

2. Rate = k CH=COCH3 Br2

3. Rate = k CH3COCH3 Br2 H+2

4. Rate = k CH3COCH3 Br2 H+

Subtopic:  Definition, Rate Constant, Rate Law |
 66%
From NCERT
AIPMT - 2008
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