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

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

For an endothermic reaction, the energy of activation is E_a, and the enthalpy of reaction is ΔH (both of these in kJ/mol). The minimum value of E_a will be:

1. Less than $∆$H

2. Equal to $∆$H

3. More than $∆$H

4. Equal to zero

The rate constants k₁ and k₂ for two different reactions are 10¹⁶. e^-2000/T and 10¹⁵. e^-1000/T, respectively. The temperature at which k₁= k₂ is:

1. $1000$ $\mathrm{K}$

2. $\frac{2000}{2.303}$ $\mathrm{K}$

3. $2000$ $\mathrm{K}$

4. $\frac{1000}{2.303}$ $\mathrm{K}$