For an endothermic reaction, where ΔH represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be

1. Less than ΔH

2. Zero

3. More than ΔH

4. Equal to ΔΗ

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How fast the reaction is at 25°C as compared to 0°C. If the activation energy is 65 KJ :-

(1) 2 times

(2) 5 times

(3) 11 times

(4) 16 times

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The activation energy of a reaction is zero. The rate constant of the reaction is :

(1) increases with increase in temperature

(2) decreases with decrease in temperature

(3) decreases with increase in temperature

(4) is nearly independent of temperature

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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

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Rate constant for a chemical reaction takes place at 500 K, is expressed as K = A e-1000. The activation energy of the reaction is

(1) 100 cal/mol

(2) 1000 kcal/mol

(3) 104 kcal/mol

(4) 106 kcal/mol

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The activation energy of a reaction can be determined from the slope of which of the following graphs?

(a) In K vs T

(b) In K/T vs T

(c) In K vs 1/T

(d) T/In K vs 1/T

 

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

(a) S = 0

(b) G = 0

(c) H = 0

(d) H = G = S = 0

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In a zero order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become

(a) 256 times
(b) 512 times
(c) 64 times
(d) 128 times

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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

(a) less than H

(b) equal to H

(c) more than H

(d) equal to zero

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The rate constants k1 and k2 for two different reactions are 1016e-2000/T and 1015e-1000/T  , respectively. The temperature at which k1=k2 is:

(a) 1000 K
(b) 20002.303K
(c) 2000K
(d) 10002.303K

 

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