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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The reaction of iodomethane with sodium ethoxide proceeds as : EtO+MeIEtOMe+ I

A plot of log MeIEtOon the Y-axis against 't' on the X-axis gives a straight line with a positive slope. What is the order of the reaction ?

(1) Second                                                

(2) First

(3) Third                                                   

(4) Fractional

Subtopic:  Order, Molecularity and Mechanism |
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For the reaction, C2H5I + OH- → C2H5OH + I- the rate constant was found to have a value of 5.03 × 10-2 moI-1 dms-1 at 289 K and 6.71 mol-1 dm3 s-1 at 333 K. 

The rate constant at 305 K will be: 

1. 1.35 mol-1 dm3 s-1                  

2. 0.35 mol-1 dm3 s-1

3. 3.15 mol-1 dm3 s-1                    

4. 7.14 mol-1 dm3 s-1

Subtopic:  Arrhenius Equation |
 52%
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A plot of ln rate Vs ln C for the nth order reaction gives 

(1) a straight line with slope n and intercept ln kn

(2) a straight line with slope (n – 1)

(3) a straight line with slope ln kn and intercept ‘n’

(4) a straight line with slope –n and intercept kn

Subtopic:  Definition, Rate Constant, Rate Law |
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The first order rate constant for a certain reaction increases from\(1.667 \times 10^{-6} \mathrm{~s}^{-1} \text { at } 727^{\circ} \mathrm{C} \text { to } 1.667 \times 10^{-4} \mathrm{~s}^{-1} \text { at } 1571{ }^{\circ} \mathrm{C}.\) The rate constant at \(1150^{\circ} \mathrm{C}\) is: 
(assume activation energy is constant over the given temperature range)

1. \(3.911 \times 10^{-5} \mathrm{~s}^{-1} \) 2. \(1 .139 \times 10^{-5} \mathrm{~s}^{-1} \)
3. \(3.318 \times 10^{-5} s^{-1} \) 4. \(1.193 \times 10^{-5} \mathrm{~s}^{-1}\)
Subtopic:  Arrhenius Equation |
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The solvolysis of 2-chloro-2-methyl propane in aqueous acetone: H2O+CH33C-ClHO-CCH33+H+Cl- has a rate equation. 

Rate =K[(CH3 )3 C  Cl].From this it may be inferred that the energy profile of the reaction leading from reactants to products is

(A)                                 

(B) 

(C)                             

(D) 

Subtopic:  First Order Reaction Kinetics |
 51%
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