Question

according to the collision theory, for a reaction to be successful, it must have correct orientation of the atoms of the reactants. which of the following must also be true for a successful reaction to occur? a catalyst must be present. the collision must have sufficient energy. the particles must have adequate velocity. reactants must have high molecular mass.

Answer 1

The collision must have sufficient energy as well.  If sufficient energy is not present the activation energy will not be over come and the bonds in the reactants will not be broken.

I hope this helps.  Let me know if anything is unclear.

Answer 2

Answer: The correct answer is the particles must have adequate velocity.

Explanation:

According to collision theory, a product is formed only when the collisions between the reactants is effective.

There are 2 factors on which the effective collisions depends:

• Energy factor: This factor says that the colliding molecules must have energy greater than the threshold energy.
• Orientation factor: This factor says that the colliding molecules must have a proper orientation at the time of collision.

Velocity is related to kinetic energy by the formula:

$E=\frac{1}{2}mv^2$

where,

E = kinetic energy of the particle

m = mass of the particle

v = velocity of the particle

So, from this we can say that the velocity of the particles must be sufficient enough for collision to be elastic.

Hence, the correct answer is the particles must have adequate velocity.