The chemical reaction, 2O3 $\to$3O2 proceeds as follows;

O3 $⇌$O2 + O .....(Fast)

O+O3 $\to$ 2O2 ....(Slow)

The rate law expression should be:

(a) r = K[O3]2

(b) r = K[O3]2[O2]-1

(c) r = K[O3][O2]

(d) unpredictable

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The rate of reaction becomes 2 times for every 10°C rise in temperature. How the rate of reaction will increase when temperature is increased from 30°C to 80°C?

(a) 16

(b) 32

(c) 64

(d) 128

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The rate constant (K) for the reaction 2A +B $\to$ Product was found to be 2.5x10-5 litre mol-1 sec-1 after 15 sec, 2.60 x10-5 litre mol-1sec-1 after 30 sec and 2.55 x10-5litre mol-1 sec-1 after 50 sec. The order of reaction is:

(a) 2

(b) 3

(c) zero

(d) 1

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A reaction A2 + B2 $\to$ 2AB occurs by the following mechanism;

A2 $\to$ A + A               .....(slow)

A + B2 $\to$ AB + B       .....(fast)

A + B $\to$ AB               .....(fast)

Its order would be:

(a) 3/2

(b) 1

(c) zero

(d) 2

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For a given reaction, presence of catalyst reduces the energy of activation by 2 kcal at 27$°$C. The rate of reaction will be increased by:

1. 20 times

2. 14 times

3. 28 times

4. 2 times

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What fraction of a reactant showing first order remains after 40 minute if t1/2 is 20 minute?

(a) 1/4

(b) 1/2

(c) 1/8

(d) 1/6

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Rate equation for a second order reaction is:

(a) K = (2.303/t) log {a/(a-x)}

(b) K = (1/t) log {a/(a-x)}

(c) K = (1/t) log {a/a(a-x)}

(d) K = (1/t2) log {a/(a-x)}

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For the reaction 2NO2 + F2 → 2NO2F, following

mechanism has been provided,

NO2 + F2   $\stackrel{slow}{\to }$  NO2F+F

NO2 + F   $\stackrel{fast}{\to }$ NO2F

Thus, rate expression of the above

reaction can be written as:

(a) r = K[NO2]2[F2]

(b) r = K[NO2 ][F2]

(c) r = K[NO2]

(d) r = K[F2]

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For the reaction:

[Cu(NH3)4]2+ + H2O$⇌$[Cu(NH3)3H2O]2+ + NH3

the net rate of reaction at any time is given by, net rate =

2.0x10-4 [Cu(NH3)4]2+[H2O] - 3.0x105 [Cu(NH3 )3 H20]2+[NH3]

Then correct statement is/are :

(a) rate constant for forward reaction = 2 x 10-4

(b) rate constant for backward reaction = 3 x 105

(c) equilibrium constant for the reaction = 6.6 x 10-10

(d) all of the above

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Rate constant of reaction can be expressed by Arrhenius equation as,

$K=A{e}^{-{E}_{a}}{RT}}$

In this equation, ${\mathrm{E}}_{\mathrm{a}}$ represents:

(a) the energy above which all the colliding molecules will react

(b) the energy below which colliding molecules will not react

(c) the total energy of the reacting molecules at a temperature, T

(d) the fraction of molecules with energy greater than the activation energy of the reaction