The correct statement among the following is:

1.	the rate of a first-order reaction does not depend on reactant concentration; the rate of a second-order reaction does depend on reactant concentrations.
2.	the half-life of a first-order reaction does not depend on [A]o; the half-life of a second-order reaction does depend on [A]0
3.	a first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed.
4.	the rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations

When the initial concentration of the reactant is doubled,
the half-life period of a zero-order reaction:

The rate Constant of reaction A $\to$ B is 0.6 X 10^-3 mole per second. If the Concentration of A is 5, then the concentration of B after 20 min is:

1. 1.08M

2. 3.60M

3. 0.36M

4. 0.72M

When the initial concentration of a reactant is doubled in a reaction,
its half-life period is not affected. The order of the reaction will be:
1. 0
2. 1
3. 1.5
4. 2 

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

1. ΔG = 0

2. ΔH = 0

3. ΔH = ΔG = ΔS = 0

4. ΔS = 0

In a reaction, A + B  → Product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8, when the concentrations of both the reactants (A and B) are doubled. The rate law for the reaction can be written as:

1. Rate = k[A][B]²

2. Rate = k[A]²[B]²

3. Rate = k[A][B]

4. Rate = k[A]²[B]