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 and rate constant (k1 and k2) of a chemical reaction at two different temperatures (T1 and T2) are related by:
1. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)\) |
2. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_2}+\frac{1}{T_1}\right)\) |
3. | \(\ln \frac{k_2}{k_1}=\frac{E_a}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)\) |
4. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_1}-\frac{1}{T_2}\right)\) |
For an endothermic reaction, the energy of activation is Ea, and the enthalpy of reaction is ΔH (both of these in kJ/mol). The minimum value of Ea 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.
2.
3.
4.