By which can activation energy be calculated?
1.  At a constant temperature
2.  At two different temperature
3.  For reversible reaction
4.  For volatile reaction

When a biochemical reaction is carried out in a laboratory outside the human body in the absence of an enzyme, then the rate of reaction obtained is ${10}^{-6}$ times. The activation energy of a reaction in the presence of an enzyme is:

1. $\frac{6}{RT}$
2. P is required.
3. Different from $E_a$ obtained in the laboratory.
4. Data is insufficient.

The activation energy for a simple chemical reaction A → B is E_a in a forward direction. The activation energy for the reverse reaction:

1. Is negative of E_a

2. Is always less than E_a

3. Can be less than or more than E_a

4. Is always double of E_a

The temperature dependence of the rate constant (k) of a chemical reaction is written in terms of the Arrhenius equation,
k = A.e^–E*/RT. The activation energy (E*) of the reaction can be calculated by plotting: 

1. $\mathrm{k}$ $\mathrm{vs}$ $\mathrm{T}$

2. $\mathrm{k}$ $\mathrm{vs}$ $\frac{1}{\log }$ $\mathrm{T}$

3. $\log$ $\mathrm{k}$ $\mathrm{vs}$ $\frac{1}{\mathrm{T}}$

4. $\log$ $\mathrm{k}$ $\mathrm{vs}$ $\frac{1}{\mathrm{log\; T}}$