1 mole of a gas changes linearly from its initial state (2 atm, 10 lt) to its final state (8 atm, 4 lt). The maximum rate constant is equal to 20 sec-1 and the value of activation energy is 40 kJ, assuming that the activation energy does not change in this temperature range. The value of the rate constant, at the maximum temperature that the gas can attain, is: 

1. 0.56 × 10-3 sec-1                                          

2. 3.16 × 10-3 sec-1

3. 1.56 × 10-3sec-1                                          

4. 5.12 × 10-3 sec-1

Subtopic:  First Order Reaction Kinetics |
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A first-order reaction was started with a decimolar solution of the reactant. After 8 minutes and 20 seconds, its concentration was found to be M/100. The rate constant of the reaction will be:

1. 4.6 × 10-3sec-1                                      

2. 16.6 × 10-3 sec-1

3. 24.6 × 10-3 sec-1                                   

4. 40.6 × 10-3 sec-1

Subtopic:  First Order Reaction Kinetics |
 70%
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87.5% of a radioactive substance disintegrates in 40 minutes. What is the half life of the substance ?

(1) 13.58 min                                                   

(2) 135.8 min

(3) 1358 min                                                    

(4) None of these

Subtopic:  First Order Reaction Kinetics |
 79%
From NCERT
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A gaseous substance AB3 decomposes irreversibly according to the overall equation AB312A2+32B2 Starting with pure AB3 the partial pressure of the reactant varies with time for which the data are given below.
Time in hours 0      5.0      15.0       53.0

PAB3mm Hg  660   330      165       82.5

What is the order of the reaction ?

(1) 2                                                            

(2) 0.5

(3) 1                                                            

(4) 1.5

Subtopic:  Order, Molecularity and Mechanism |
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The inversion of cane sugar proceeds with half life of 500 minute at pH 5 for any concentration of sugar. However if pH = 6, the half life changes to 50 minute. The rate law expression for the sugar inversion can be written as 

(1) r = K[sugar]2 [H]6                                             

(2) r = K[sugar]1 [H]0

(3) r = K[sugar]0 [H+]6                                          

(4) r = K[sugar]0 [H+]1

Subtopic:  Order, Molecularity and Mechanism |
 63%
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The decomposition of A into product has value of k as \(4.5 \times 10^3 \mathrm{~s}^{-1} \text { at } 10^{\circ} \mathrm{C}.\) Energy of activation of the reaction is \(60 \mathrm{~kJ}~mol^{-1}.\) The temperature at which value k would become \(1.5\times10^4~s^{-1}\) is : 

1. \(12{ }^{\circ} \mathrm{C} \) 2. \(24^{\circ} \mathrm{C} \)
3. \(48^{\circ} \mathrm{C} \) 4. \(36^{\circ} \mathrm{C}\)
Subtopic:  Arrhenius Equation |
 60%
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Decomposition on NH3on heated tungsten yields the following data :

Initial pressure (mm)      65    105     y    185

Half-life (s)                   290     x     670   820

What are the values of x and y in that order ?

(1) 420 s, 110 mm                                                  

(2) 500 s, 160 mm

(3) 520 s, 170 mm                                                  

(4) 460 s, 150 mm

Subtopic:  First Order Reaction Kinetics |
 53%
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The half life period of gaseous substance undergoing thermal decomposition was measured for various initial pressure ‘P’ with the following result. 

P(mm)       250     300      400     450

t1/2(min)   136    112.5     85      75.5

Calculate the order of reaction.

(A) 2                                                 

(B) 4

(C) 6                                                 

(D) 10

Subtopic:  First Order Reaction Kinetics |
 69%
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For the reaction 2N2O5(g) → 4NO2(g) + O2(g)the concentration of  NO2 increases by 2.4 × 10-2 mol L-1

in 6 seconds. The rate of appearance of NO2 and the rate of disappearance of N2O5 , respectively, are:

1. 2 x 10-3 mol L-1 sec-1, 4 x 10-3 mol L-1 sec-1

2. 2 x 10-3 mol L-1 sec-1, 1 x 10-3 mol L-1 sec-1

3. 2 x 10-3 mol L-1 sec-1, 2 x 10-3 mol L-1 sec-1

4. 4 x 10-3 mol L-1 sec-1, 2 x 10-3 mol L-1 sec-1

Subtopic:  Definition, Rate Constant, Rate Law |
 60%
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The rate constant of a particular reaction has the dimension of frequency. The order of the reaction is: 

1. Zero.                                                     

2. First.

3. Second.                                                 

4. Fractional.

Subtopic:  Definition, Rate Constant, Rate Law |
 80%
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