Question

Which of following is not a key concept of a collision theory

Answer 1

Collision theory states that when suitable particles of the reactant hit each other, only a certain amount of collisions result in a perceptible or notable change; these successful changes are called successful collisions. The successful collisions must have enough energy, also known as activation energy, at the moment of impact to break the pre-existing bonds and form all new bonds. This results in the products of the reaction. Increasing the concentration of the reactant brings about more collisions and hence more successful collisions. Increasing the temperature increases the average kinetic energy of the molecules in a solution, increasing the collisions that have enough energy. Collision theory was proposed independently by Max Trautz in 1916[1] and William Lewis in 1918.[2]

Reaction rate tends to increase with concentration phenomenon explained by collision theory

When a catalyst is involved in the collision between the reactant molecules, less energy is required for the chemical change to take place, and hence more collisions have sufficient energy for reaction to occur. The reaction rate therefore increases.

Collision theory is closely related to chemical kinetics.

Collision theory is a model for explaining chemical reactions and reaction rates using the interactions of particles within the reactants. There are three important parts to collision theory, that reacting substances must collide, that they must collide with enough energy and that they must collide with the correct orientation. Increasing the kinetic energy of these particles or decreasing their volume increases the frequency of collisions and speeds a reaction.

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Answer 2

A particle should collide slowly to one another or else they will bounce off each other is not a key concept of a collision theory

• The collision theory is based on the fact that occurrence of any chemical reaction can only be possible when the particles hit each other or collide in order to react.

• The collision that occurs between the particles in a chemical reaction must be effective which means that it should occur with a proper orientation.
• The collision between the particles of reactant side is necessary but this collision is not enough for a chemical reaction to take place. The particles must have adequate amount of energy to attain the activated complex.

Hence, Collision theory does not involve the concept that a particle should collide slowly to one another or else they will bounce off each other.