| Column I | Column II | ||
| A. | Catalyst alters the rate of reaction | 1. | Proper orientation is not there always |
| B. | 2. | By lowering the activation energy | |
| C. | Energetically favorable reactions are sometimes slow | 3. | Total probability is one |
| D. | Area under the Maxwell-Boltzmann curve is constant | 4. | Refers to the fraction of molecules with energy equal to or greater than the activation energy |
Codes
| A | B | C | D | |
| 1. | 2 | 4 | 1 | 3 |
| 2. | 3 | 1 | 4 | 2 |
| 3. | 1 | 4 | 3 | 2 |
| 4. | 3 | 4 | 1 | 2 |
Explanation:
1. Catalyst alters the rate of reaction by lowering the activation energy.
2. refers to the fraction of molecules with kinetic energy equal to or greater than the activation energy
3. Energetically favorable reactions are sometimes slow due to the improper orientation of molecules that cause some ineffective collision of molecules.
4. Area under the Maxwell, Boltzmann curve is constant because the total probability of a molecule taking part in a chemical reaction is equal to one.
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