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]

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

Activation energy $E_a$ and rate constant (k₁ and k₂) of a chemical reaction at two different temperatures (T₁ and T₂) are related by:

1. $ln$ $\frac{k_2}{k_1}=-\frac{E_a}{R}(\frac{1}{T_2}-\frac{1}{T_1})$ $$

2. $In$ $\frac{k_2}{k_1}=-\frac{E_a}{R}(\frac{1}{T_2}+\frac{1}{T_1})$ $$

3. $In$ $\frac{k_2}{k_1}=\frac{E_a}{R}(\frac{1}{T_2}-\frac{1}{T_1})$ $$

4. $In$ $\frac{k_2}{k_1}=-\frac{E_a}{R}(\frac{1}{T_1}-\frac{1}{T_2})$ $$