The rate constant of the reaction A $\to$ B is 0.6 x 10^-3 molar per second. If the

concentration of A is 5 M then concentration of B after 20 min is

1. 1.08 M

2. 3.60 M

3. 0.36 M

4. 0.72 M

If the rate of reaction doubles when the temperature is raised from 20 °C to 35 °C, then the activation energy for the reaction will be :
(R = 8.314 J mol^-1 K^-1)

1. 342 kJ mol^-1

2. 269 kJ mol^-1

3. 34.7 kJ mol^-1

4. 15.1 kJ mol^-1

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

1. $∆$S = 0

2. $∆$G = 0

3. $∆$H = 0

4. $∆$H = $∆$G = $∆$S = 0

In a reaction, A+B $\stackrel{ }{\to }$ Product, rate is doubled when the concentration of B is

doubled, and rate increases by a factor of 8 when the concentrations of both the

reactants (A and B) are doubled. Rate law for the reaction can be written as

1. Rate = k[A][B]²

2. Rate = k[A²][B²]

3. Rate = k[A][B]

4. Rate = k[A]² [B]

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

1. 256 times

2. 512 times

3. 64 times

4. 128 times

Which one of the following statements for the order of a reaction is incorrect?

1. Order is not influenced by stiochiometric coefficient of the reactants.

2. Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction.

3. Order of reaction is always whole number.

4. Order can be determined only experimentally.

For the reaction,

N₂O₅(g) → 2NO₂(g) + \(\frac{1}{2}\)O₂(g)

the value of the rate of disappearance of ${\mathrm{N}}_2{\mathrm{O}}_5$ is given as $6.\mathrm{25 }\times {10}^{-3}$ $mol$ $L^{-1}{s}^{-1}$. The rate of formation of $N{O}_2$ $and$ $O_2$ is given respectively as:

1. 6.25 x 10^-3 mol L^-1s^-1 and 6.25 x 10^-3 mol L^-1s^-1

2. 1.25 x 10^-2 mol L^-1s^-1 and 3.125 x 10^-3 mol L^-1s^-1$\mathrm{}{\mathrm{}}^{}$

3. 6.25 x 10^-3 mol L^-1s^-1 and 3.125 x 10^-3 mol L^-1s^-1

4. 1.25 x 10^-2 mol L^-1s^-1 and 6.25 x 10^-3 mol L^-1s^-1

For an endothermic reaction, energy of activation is E_a and enthalpy of reaction is $∆$H (both of these in kJ/mol). Minimum value of E_a will be

1. Less than $∆$H

2. Equal to $∆$H

3. More than $∆$H

4. Equal to zero

During the kinetic study of the reaction, 2A + B → C + D, the following results were obtained:

Based on the above data, the correct rate law is:
1.  Rate=k[A]²[B]

2.  Rate=k[A][B]

3.  Rate=k[A]²[B]²

4.  Rate=k[A][B]²

Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction

is

1. 5.0 x 10^-3s^-1

2. 0.5 x 10^-2s^-1

3. 0.5 x 10^-3s^-1

4. 5.0 x 10^-2s^-1