1. | Probability of collision. |
2. | Orientation of reactant molecules during collision. |
3. | Rate constant at two different temperatures. |
4. | Rate constant at standard temperature. |
1. | 2. | ||
3. | 4. |
1. | 2. | ||
3. | 4. |
Assertion (A): | A reaction can have zero activation energy. |
Reason (R): | The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
The plot of ln k vs \({1 \over T}\) for the following reaction
\(2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) \) gives a straight line with the slope of the line equal to \(-1.0 \times 10^4 K \).
The activation energy for the reaction in J mol–1 is:
(Given R = 8.3 J K–1 mol–1)
1. | \(4.0 \times 10^2 \) | 2. | \(4.0 \times 10^{-2} \) |
3. | \(8.3 \times 10^{-4} \) | 4. | \(8.3 \times 10^4 \) |
For a reaction AB, enthalpy of reaction is and enthalpy of activation is . The correct potential energy profile for the reaction is:
1. | 2. | ||
3. | 4. |
The slope of Arrhenius Plot (ln k v/s ) of the first-order reaction is . The value of Ea of the reaction is:
[Given R = 8.314 JK–1 mol–1]
1. | 166 kJ mol–1 | 2. | –83 kJ mol–1 |
3. | 41.5 kJ mol–1 | 4. | 83.0 kJ mol–1 |