The incorrect statement among the following is:

1.	The value of the equilibrium constant is changed in the presence of a catalyst in the reaction at equilibrium
2.	Enzymes catalyze mainly bio-chemical reactions
3.	Coenzymes increase the catalytic activity of the enzyme
4.	The catalyst does not initiate any reaction

The correct statement among the following is:

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

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

The incorrect statement regarding the order of reaction is:

During the kinetic study of the reaction, 2A + B\( \rightarrow\)C + D, following results were obtained:
 

Based on the above data which one of the following is correct?

1. rate= k[A]²[B]

2. rate= k[A][B]

3. rate= k[A]²[B]²

4. rate= k[A][B]²

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

1. $5.0\times {10}^{-3}{s}^{-1}$

2. $0.5\times {10}^{-2}{s}^{-1}$

3. $0.5\times {10}^{-3}{s}^{-1}$

4. $5.0\times {10}^{-2}{s}^{-1}$