For a certain reaction the variation of the rate constant with temperature is given by the equation

                            In k1=In k0+In 310t t0°C

The value of the temperature coefficient of the reaction rate is therefore –

(A) 4                                                  

(B) 3

(C) 2                                                   

(D) 10

 

Concept Questions :-

First Order Reaction Kinetics
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A catalyst lowers the activation energy of a reaction from 20 kJ mole-1 to 10 kJ mole-1. The temperature at which the uncatalysed reaction will have the same rate as that of the catalysed at 27°C s

(A) -123°C                                                     

(B) 327°C

(C) 327°C                                                         

(D) +23°C

Concept Questions :-

Arrhenius Equation
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The rate of reaction triples when temperature change from 20°C to 50°C. Calculate energy of activation for the reaction.

(A)28.81 kJ mol-1                                         

(B)  38.51 kJ mol-1

(C) 18.81 kJ mol-1 

D 8.31 kJ mol-1

Concept Questions :-

Arrhenius Equation
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The half life time for the decomposition of a substance dissolved in CCl4 is 2.5 hour at 30°C. How much of the substance will be left after 10 hours, if the initial weight of the substance is 160 gm ?

(A) 20 gm                                                          

(B) 30 gm

(C) 40 gm                                                          

(D) 10 gm

Concept Questions :-

First Order Reaction Kinetics
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For the reaction

[Cr(H2O)4Cl2 ]+ (aq.) k1  [Cr(H2O)5C1]2+ (aq.) k2  [Cr(H2O)6 ]3+(aq.)

k1 = 1.78 × 10-3 s-1 and k2 = 5.8 × 10-5 s-1

If initial concentration of  [Cr(H2O)4Cl2 ]+is 0.0.174 M at 273 K. Calculate time at which concentration of [Cr(H2O)5Cl]2+ is maximum

(A) 1990 seconds.                                          

(B) 1090 seconds

(C) 2100 seconds.                                         

(C) 2110 seconds.

Concept Questions :-

First Order Reaction Kinetics
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What is the activation energy for the decomposition of N2O5 as N2O5 2NO2+ (1/2) O2 If the values of the rate constants are 3.45×105 and 6.9×10-3 at 27°C and 67°C respectively.

(A) 102 ×102kJ                                      

(B) 488.5 kJ

(C) 112 kJ                                              

(D) 112.5 kJ

Concept Questions :-

Arrhenius Equation
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Find out the percentage of the reactant molecules crossing over the energy bariier at 325 K, given that H325=0.12 kcal, Eab=+0.02 kcal

1. 80.62 %

2. 85.23 %

3. 89.27 &

4. None of the above

Concept Questions :-

First Order Reaction Kinetics
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The rate constant for a first order reaction is 60s-1. How much time will it take to reduce the initial concentration of the reactant to its 1/16th value –

(A) 0.046 s                                                         

(B) 0.46 s

(C) 1.124 s                                                         

(D) 2.123 s

Concept Questions :-

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

(A) 0.56 × 10-3 sec-1                                          

(B) 3.16 × 10-3 sec-1

(C) 1.56 × 10-3sec-1                                          

(D) 5.12 × 10-3 sec-1

Concept Questions :-

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. Determine the rate constant of the reaction. 

(A) 4.6 × 10-3sec-1                                      

(B) 16.6 × 10-3 sec-1

(C) 24.6 × 10-3 sec-1                                   

(D) 40.6 × 10-3 sec-1

Concept Questions :-

First Order Reaction Kinetics
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Difficulty Level: