For a certain reaction, 10% of the reactant dissociates in 1 hour, 20% of the reactant dissociates in 2 hours, 30% of the reactant dissociates in 3 hours. Then the units of the rate constant is:-

(1) hour-1

(2) mol L-1 hr-1

(3) mol L-1 sec-1

(4) mol L sec-1

Subtopic:  Order, Molecularity and Mechanism |
 58%
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For a first order reaction A  product :

(1)

 

(2)

 

(3)

 

(4) 

Subtopic:  Order, Molecularity and Mechanism |
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Two reactions of the same order have equal Pre-exponential factors but their activation energies differ by 24.9 kJ/mol. Calculate the ratio between the rate constants (K1/K2) these reactions at 27°C :

1. 2.2 × 104

2. 1/2 × 10-4

3. 1/2 × 104

4. 2.2 × 10-4

Subtopic:  First Order Reaction Kinetics |
 53%
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The activation energy of a reaction is zero. The rate constant of the reaction is :

1. increases with an increase in temperature

2. decreases with a decrease in temperature

3. decreases with an increase in temperature

4. is nearly independent of temperature

Subtopic:  Arrhenius Equation |
 75%
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The rate constant of a first order reaction is 10-3 min-1 at 27°C. The temperature coefficient of this  reaction is 2. The rate constant at 17°C will be :

(1) 10-3 min-1

(2) 5  x 10-4 min-1

(3) 2 x 10-3 min-1

(4) 10-2 min-1

Subtopic:  Arrhenius Equation |
 64%
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 For the pseudo first order reaction A + B  P, when studied with 0.1 M of B is given by -d[A]/dt =k[A] where K = 1.85 x 104 sec-1. Calculate the value of rate constant for second order reaction :

(1) 1.85 x 104

(2) 1.85 x 10-4

(3) 1.85 x 10-5

(4) 1.85 x 105

Subtopic:  First Order Reaction Kinetics |
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Time required to decompose half of the substance for (n)th order reaction is propotional to:-

1. 1/an-1

2. a1-n

3. an-1

4. Both 1 and 2

Subtopic:  Order, Molecularity and Mechanism |
 55%
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What is the activation energy for reverse reaction on the basis of given data ?

N2O4(g)  2NO2(g)  ΔH = +54kJ

Ea(forward) = +57.2 kJ

1. -54 kJ

2.  +3.2 kJ

3. 60.2 kJ

4. 111.2 kJ

Subtopic:  Arrhenius Equation |
 84%
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For a first-order reaction, the time required for 99.9% of the reaction to take place is nearly :

(1) 10 times that required for half of the reaction

(2) 100 times that required for two-third of the reaction

(3) 10 times that required for one-fourth of the reaction

(4) 20 times that required for half of the reaction

Subtopic:  First Order Reaction Kinetics |
 81%
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The rate constant for a chemical reaction that takes place at 500 K is expressed as K = A e-1000. The activation energy of the reaction will be:

1. 100 cal/mol

2. 1000 kcal/mol

3. 104 kcal/mol

4. 106 kcal/mol

Subtopic:  Arrhenius Equation |
 69%
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