Problem
Problem
The rate constant of a reaction increases with increase of temperature because a. The activation energy increases b. The population of activated molecules increases. c. The activation energy decreases d. The population of activated molecules decreases.Intuitive explanation
The key insight is that activation energy acts as a barrier that molecules must overcome to react. Higher temperature gives reactant molecules more kinetic energy, so a larger fraction of collisions become energetic enough to break bonds and form products. This exponential relationship between temperature and molecular energy (captured by the Arrhenius equation) is why even modest temperature increases can dramatically speed up reactions.
Intuitive explanation
The key insight is that activation energy acts as a barrier that molecules must overcome to react. Higher temperature gives reactant molecules more kinetic energy, so a larger fraction of collisions become energetic enough to break bonds and form products. This exponential relationship between temperature and molecular energy (captured by the Arrhenius equation) is why even modest temperature increases can dramatically speed up reactions.