Why does the rate of a reaction generally increase with increased temperature? (Choose all that apply)

A.

at higher temperatures, molecules are more likely to collide with each other in the correct orientation.

B.

at higher temperatures, molecules will collide more often.

C.

at higher temperatures, the potential energy difference between reactants and products is smaller.

D.

at higher temperatures, more of the collisions will have the required activation energy.

Question

Keira Wilcox

Chemistry

30 October, 18:34

Why does the rate of a reaction generally increase with increased temperature? (Choose all that apply)

A.

at higher temperatures, molecules are more likely to collide with each other in the correct orientation.

B.

at higher temperatures, molecules will collide more often.

C.

at higher temperatures, the potential energy difference between reactants and products is smaller.

D.

at higher temperatures, more of the collisions will have the required activation energy.

+1

Answers (1)

Know the Answer?

Antony Villarreal · Answer 1

Answer: Option (A) is the correct answer.

Explanation:

When we increase the temperature of a chemical reaction then molecules of the given reaction will gain kinetic energy. As a result, they will come into motion and then collide frequently with each other.

For a reaction to increase its rate it is important that the particles must collide in a correct orientation.

Thus, we can conclude that the rate of a reaction generally increase with increased temperature because at higher temperatures, molecules are more likely to collide with each other in the correct orientation.