As the temperature of a chemical reaction increases, which of the following typically occurs?

• A. The reaction reaches equilibrium more slowly.
• B. The rate of the reaction decreases because molecules move more slowly at higher temperatures.
• C. The rate of the reaction increases due to more frequent and energetic collisions between reactant molecules.
• D. The activation energy of the reaction increases.

Answer: (C)

Verified step by step guidance

1. Understand the relationship between temperature and reaction rate: Increasing temperature generally increases the kinetic energy of molecules, causing them to move faster.
2. Recall the collision theory, which states that for a reaction to occur, reactant molecules must collide with sufficient energy (activation energy) and proper orientation.
3. Recognize that as temperature increases, the number of molecules with energy equal to or greater than the activation energy increases, leading to more frequent and effective collisions.
4. Note that the activation energy itself is a fixed property of the reaction and does not increase with temperature.
5. Conclude that increasing temperature typically increases the reaction rate, not decreases it, and the reaction reaches equilibrium faster, not more slowly.