alleryStart learning →How does collision theory account for faster rates at higher concentration?
AMolecules gain more kinetic energy each
BThe activation energy of the step falls
CThe orientation of collisions improves too
DMore molecules per volume means more collisions
Answer & Solution
Correct answer: D. More molecules per volume means more collisions
1. The first postulate makes the rate proportional to the number of collisions per unit time.
2. Raising a concentration packs more molecules into the same volume.
3. Crowded molecules meet more often, so the collision count per second rises.
4. More collisions of adequate energy means a faster reaction.
5. Adding reactant does not warm the sample, so the average kinetic energy per molecule is unchanged.
_Source: OpenStax Chemistry (CC BY 4.0), Ch 12 "Kinetics", section 12.5 Collision Theory_
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