Consider the following statements and select the correct statements:

(A) The energy required to form the activated complex is known as activation energy.
(B) The Arrhenius equation explains the temperature dependence of the rate of chemical reaction.
(C) The number of collisions per second per unit volume of the reaction mixture is known as collision frequency.
(D) Lower the value of activation energy, lower will be the rate of reaction.

Choose the correct answer from the options given below:

(A), (B) and (C) only

The correct answer is Option (2) → (A), (B) and (C) only

Reaction rates depend on several kinetic factors such as activation energy, temperature, and collision frequency. Each statement can be evaluated using principles of chemical kinetics.

Statement (A)

The activated complex (transition state) is formed when reactant molecules acquire sufficient energy to reach a high-energy unstable state during the reaction.

The minimum energy required to form this activated complex is called activation energy.

Thus, this statement is correct.

Statement (B)

The Arrhenius equation describes how the rate constant depends on temperature.

Arrhenius equation:

$k = A e^{(−Ea/RT)}$

where

k = rate constant

A = frequency factor

Ea = activation energy

R = gas constant

T = temperature

This equation clearly explains how increasing temperature increases the reaction rate.

Thus, this statement is correct.

Statement (C)

According to collision theory, reactions occur due to collisions between reacting molecules. The collision frequency is defined as the number of collisions occurring per second per unit volume of the reaction mixture. Thus, this statement is correct.

Statement (D)

Activation energy represents the energy barrier that reactants must overcome to form products. If activation energy is lower, more molecules will possess sufficient energy to react, and the rate of reaction increases. Since the statement claims the rate decreases, it is incorrect.