How does the energy of the activated complex compare with the energies of reactants an products? a. It is lower than the energy of both reactants and products. b. It is lower than the energy of reactants but higher than the energy of products. c. It is higher than the energy of reactants but lower than the energy of products. d. It is higher than the energy of both reactants and products.

Question

Skylar Calderon

Chemistry

22 September, 09:05

How does the energy of the activated complex compare with the energies of reactants an products? a. It is lower than the energy of both reactants and products. b. It is lower than the energy of reactants but higher than the energy of products. c. It is higher than the energy of reactants but lower than the energy of products. d. It is higher than the energy of both reactants and products.

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Answers (2)

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Makai King · Answer 1

Option d, It is higher than the energy of both reactants and products.

Explanation:

When reactant molecules collide with each other during the course of the reaction, an intermediate state is reached before the formation of product. This intermediate state is also called activated complex.

Activated complex consist energy higher than that of both the reactants and products. Because of possessing higher energy, it is unstable and temporary.

Hence, among given, option d is correct.

Dominic Robertson · Answer 2

d. It is higher than the energy of both reactants and products.

Explanation:

The activated complex is a transient state, or intermediate phase, between reagents (weak or not), in which the final product has not yet been formed. This effective shock, like any chemical bond, needs energy. To form this transient state requires an activation energy, a minimum energy for this intermediate phase to occur.

Within this phenomenon, the activation energy must occur by some criteria, which characterizes a chemical bond in an activated complex:

Binding reagent molecules need to be involved; This collision in the activation energy must be as close as possible to the geometric formation of the complex in order to activate it; The collision cannot have a lower energy than the activation energy. Must be equal to or greater than propagated during reaction.

Within these three rules, it is clearer to define this complex as the moment when a molecule of a given atom collides with another molecule of any other atom and breaks the bond established between them.

For it to happen, the energy needs to be high. When this potential energy is present at a high level during the reaction, it is also necessary to have a high energy charge to complete the complex and also the collision of the reactant molecules to form the binding products.