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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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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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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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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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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In the reaction, 
BrO3-(aq)+5Br-(aq)+6H+ 3Br2(l)+3H2O(l) 
The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions:

1. d[Br2]dt=-35d[Br-]dt

2. d[Br2]dt=-53d[Br]dt

3. d[Br2]dt=53d[Br-]dt

4. d[Br2]dt=35d[Br-]dt

Subtopic:  Definition, Rate Constant, Rate Law |
 84%
From NCERT
AIPMT - 2009
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For the reaction, \(\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3,\) if, \(\frac{d[NH_{3}]}{dt} \ = \ 2\times 10^{-4} \ mol \ L^{-1} \ s^{-1}\), the value of  \(\frac{-d[H_{2}]}{dt}\) would be:

1. \(3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) 2. \(4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)
3. \(6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \) 4. \(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)
Subtopic:  Definition, Rate Constant, Rate Law |
 84%
From NCERT
AIPMT - 2009
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The half-life period of a first-order reaction is 1386 s. The specific rate constant of the reaction is:

1. 5.0×10-3s-1

2. 0.5×10-2s-1

3. 0.5×10-3s-1

4. 5.0×10-2s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 84%
From NCERT
AIPMT - 2009
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During the kinetic study of the reaction, 2A + B\( \rightarrow\)C + D, following results were obtained:
 

Run

[A)/ mol L-1

[B)/ mol L-1

Initial rate of
formation of D/mol 

L-1

I

0.1

0.1

6.0×10-3

II

0.3

0.2

7.2×10-2

III

0.3

0.4

2.88×10-1

IV

0.4

0.1

2.40×10-2


Based on the above data which one of the following is correct?

1. rate= k[A]2[B]

2. rate= k[A][B]

3. rate= k[A]2[B]2

4. rate= k[A][B]2

Subtopic:  Definition, Rate Constant, Rate Law |
 76%
From NCERT
AIPMT - 2010
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The incorrect statement regarding the order of reaction is:

1. Order is not influenced by the stoichiometric coefficient of the reactants.
2. Order of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction.
3. The order of reaction is always a whole number.
4. Order can be determined by experiments only.
Subtopic:  Definition, Rate Constant, Rate Law |
 79%
From NCERT
AIPMT - 2011
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