Final answer:
The total change in entropy (ΔS total) and activation energy (Ea) of a chemical reaction are independent of each other, as ΔS total pertains to disorder in the system and surroundings, while Ea concerns the energy barrier that must be overcome for the reaction to proceed.
The Correct Option is:
3) DS total and activation energy are independent of each other
Step-by-step explanation:
The relationship between the total change in entropy (ΔS total) and the activation energy (Ea) of a chemical reaction is not straightforward; they are not directly proportional or inversely proportional to each other by nature.
While ΔS total involves changes in the disorder or randomness of the system and surroundings, activation energy is related to the energy required for a chemical reaction to proceed. The Arrhenius equation illustrates how activation energy affects the rate of a reaction, which is influenced by the temperature and frequency factor, as well as the orientation of reacting particles.
Since the question specifically links the reaction rate to activation energy, it is important to understand the role of activation energy in a chemical reaction. It represents the minimum energy required for reactants to form an activated complex or transition state before transforming into products.
ΔS total, on the other hand, reflects the total entropy change of a system and is not concerned with the energy needed to reach the transition state. As a result, we can conclude that ΔS total and activation energy are independent of each other (ΔS total and activation energy are independent of each other).