Why do reactants require relatively high-energy collisions to form products?

a. So that the orientation is correct for bond breaking to occur.

b. So that there are more frequent collisions.

c. Reactants need to gain energy to break bonds and to form new ones.

d. no right answer

Question

Hamza Barr

Chemistry

23 June, 02:22

Why do reactants require relatively high-energy collisions to form products?

a. So that the orientation is correct for bond breaking to occur.

b. So that there are more frequent collisions.

c. Reactants need to gain energy to break bonds and to form new ones.

d. no right answer

+1

Answers (1)

Know the Answer?

Walter Osborne · Answer 1

The correct option is C. Reactants need to gain energy to break bonds and to form new ones.

Explanation:

The Collision Theory explains the fact that for a chemical reaction to occur, the reactants must collide with one another with a force which breaks the bonds in the reactants, so that new bonds can be formed among the reactants. If molecules do not collide with a certain force, the chemical reaction won't occur. The energy with which the molecules collide is termed as the activation energy. The more the concentration of reactants, the more are the chances of collisions and the more will be the activation energy.

Why do reactants require relatively high-energy collisions to form products?a. So that the orientation is correct for bond breaking to occur.b. So that there are more frequent collisions.c. Reactants need to gain energy to break bonds and to form new ones.d. no right answer

Why do reactants require relatively high-energy collisions to form products?

a. So that the orientation is correct for bond breaking to occur.

b. So that there are more frequent collisions.

c. Reactants need to gain energy to break bonds and to form new ones.

d. no right answer