A reaction having equal energies of activation for forward and reverse reactions has

1. S = 0

2. G = 0

3. H = 0

4. H = G = S = 0

Subtopic:  Arrhenius Equation |
 67%
NEET - 2013
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For the reaction,

N2O5(g) → 2NO2(g) + \(\frac{1}{2}\)O2(g)

the value of the rate of disappearance of N2O5 is given as 6.25 × 10-3 mol L-1s-1. The rate of formation of NO2 and O2 is given respectively as:

1. 6.25 x 10-3 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

2. 1.25 x 10-2 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1

3. 6.25 x 10-3 mol L-1s-1 and 3.125 x 10-3 mol L-1s-1

4. 1.25 x 10-2 mol L-1s-1 and 6.25 x 10-3 mol L-1s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 86%
From NCERT
NEET - 2010
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For an endothermic reaction, energy of activation is Ea and enthalpy of reaction is H (both of these in kJ/mol). Minimum value of Ea will be

1. Less than H

2. Equal to H

3. More than H

4. Equal to zero

Subtopic:  Arrhenius Equation |
 67%
NEET - 2010
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Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction

is

1. 5.0 x 10-3s-1

2. 0.5 x 10-2s-1

3. 0.5 x 10-3s-1

4. 5.0 x 10-2s-1

Subtopic:  Definition, Rate Constant, Rate Law |
 81%
From NCERT
NEET - 2009
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For the reaction A+B products, it is observed that
 

(1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
(2) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in that rate of the reaction

The rate of this reaction is, given by

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

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

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

4. rate = k[A][B]

Subtopic:  Order, Molecularity and Mechanism |
 83%
From NCERT
NEET - 2009
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In the reaction, BrO-3(aq) + 5Br-(aq) + 6H+ 3Br2(l) + 2H2O(l)

The rate of appearance of bromine (Br2) is related to rate of disappearance of bromide

ions as following 

1. d[Br2]/dt = -(3/5)d[Br-]/dt

2. d[Br2]/dt = (5/3)d[Br-]/dt

3. d[Br2]/dt = -(5/3)d[Br-]/dt

4. d[Br2]/dt = (3/5)d[Br-]/dt

Subtopic:  Definition, Rate Constant, Rate Law |
 81%
From NCERT
NEET - 2009
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The rate constants k1 and k2 for two different reactions are 1016 e-2000/T and 1015 e-1000/T  , respectively. The temperature at which k1=k2 is:

(1) 1000 K

(2) 20002.303K

(3) 2000K

(4) 10002.303K

 

Subtopic:  Arrhenius Equation |
 63%
From NCERT
NEET - 2008
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The bromination of acetone that occurs in acid solution is represented by this equation.

CH3COCH3(aq) + Br2(aq)            CH3COCH2Br(aq) + Br-(aq)

These kinetic 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, disappearance of Br2, Ms-1

                        5.7X10-5

                        5.7X10-5

                        1.2X10-4

                        3.1X10-4

Based on these data, the rate 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 |
 65%
From NCERT
NEET - 2008
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In a first order reaction A               B, if k is rate constant and initial concentration of the reactant A is 0.5 M then the half-life is :

(1) 0.6930.5k

(2) log 2k

(3) log 2k0.5

(4) ln 2k

Subtopic:  Definition, Rate Constant, Rate Law |
 72%
From NCERT
NEET - 2007
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If a first-order reaction reaches 60% completion within 60 minutes, approximately how much time would it take for the same reaction to reach 50% completion? (log 4=0.60, log 5=0.69)

1. 50 min

2. 45 min

3. 60 min

4. 30 min

Subtopic:  First Order Reaction Kinetics |
 74%
From NCERT
NEET - 2007
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