Why does an increased temperature cause a reaction to occur faster?A. It does not. The increased temperature causes the particles to spread out and collide less.B. The increased temperature makes the molecules more loosely attached so they can switch atoms more easily.C. The increased kinetic energy causes the particles to move faster, causing more collisions.D. The increased potential energy in the particles means less energy is needed from the environment for the activation energy.

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MareliK711371 MareliK711371 · Answer 1 · 2022-11-03T15:39:33+01:00

Answer

C. The increased kinetic energy causes the particles to move faster, causing more collisions.

Explanation

An increased temperature typically causes a reaction to occur faster by raising the average kinetic energy of the reactant molecules.

Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision.

The correct answer is option C. The increased kinetic energy causes the particles to move faster, causing more collisions.