For the reaction, 2A → B, rates= k[A]². If the concentration of reactant is doubled, then the:

(a)	rate of reaction will be doubled.
(b)	rate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant.
(c)	rate constant will change since the rate of reaction and rate constant are directly proportional to each other.
(d)	rate of reaction will increase by four times.

Identify the set of correct statements & choose the correct answer from the options given below:

1.	(a) and (c) only	2.	(a) and (b) only
3.	(b) and (d) only	4.	(c) and (d) only

For a general reaction A → B, the plot of concentration of A vs time is given below:

The unit of the rate constant would be:

For a general reaction A → B, the plot of concentration of A vs time is given below:

The order of the reaction would be- 

1. Zero 

2. First

3. Half

4. Second

The correct statement about X in the below mentioned graph:

The graph between lnK and 1/T is given below:

The value of activation energy would be:

Consider the following graph:

The point that represents the most probable kinetic energy is -

1. C

2. A

3. B

4. None of the above

The nature of the reaction represented in the following graph is:

The slope of the given below graph is -

 $1.$ $\frac{\mathrm{k}}{2.303}$
$$
$2.$ $-\frac{\mathrm{k}}{2.303}$
$$
$3.$ $-\frac{2.303}{\mathrm{k}}$
$$
$4.$ $\frac{2.303}{\mathrm{k}}$

Consider the following graph:
      

The instantaneous rate of reaction at t = 600 sec will be:

$1. - 4.75$ $\times {10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$2.$ $5.75\times {10}^{-5}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$3.$ $$ $6.75\times {10}^{-6}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$
$4.$ $-6.75\times {10}^{-6}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$

Based on the graph below, the average rate of reaction will be: 

1.  \(\frac{[R_{2}]-[R_{1}]}{t_{2}-t_{1}}\)
2.  \(-(\frac{[R_{2}]-[R_{1}]}{t_{2}-t_{1}})\)
3.  \(\frac{[R_{2}]}{t_{2}}\)
4.  \(-(\frac{[R_{1}]-[R_{2}]}{t_{2}-t_{1}})\)