Question

What will happen to energy of activation if transition state is more stable relative in products ?​

Answer 1

Answer:

The activation energy of a chemical reaction is kind of like that “hump” you have to get over to get yourself out of bed. Even energy-releasing (exergonic) reactions require some amount of energy input to get going, before they can proceed with their energy-releasing steps. This initial energy input, which is later paid back as the reaction proceeds, is called the activation energy and is abbreviated \text E_{\text A}EAstart text, E, end text, start subscript, start text, A, end text, end subscript.

Activation energy

Why would an energy-releasing reaction with a negative ∆G need energy to proceed? To understand this, we need to look at what actually happens to reactant molecules during a chemical reaction. In order for the reaction to take place, some or all of the chemical bonds in the reactants must be broken so that new bonds, those of the products, can form. To get the bonds into a state that allows them to break, the molecule must be contorted (deformed, or bent) into an unstable state called the transition state. The transition state is a high-energy state, and some amount of energy – the activation energy – must be added in order for the molecule reach it. Because the transition state is unstable, reactant molecules don’t stay there long, but quickly proceed to the next step of the chemical reaction.

In general, the transition state of a reaction is always at a higher energy level than the reactants or products, such that \text E_{\text A}EAstart text, E, end text, start subscript, start text, A, end text, end subscript always has a positive value – independent of whether the reaction is endergonic or exergonic overall. The activation energy shown in the diagram below is for the forward reaction (reactants \rightarrow→right arrowproducts), which is exergonic. If the reaction were to proceed in the reverse direction (endergonic), the transition state would remain the same, but the activation energy would be larger. This is because the product molecules are lower-energy and would thus need more energy added to reach the transition state at the top of the reaction “hill.” (An activation energy arrow for the reverse reaction would extend from the products up to the transition state.)

Explanation:

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Answer 2

if the transition state is more stable in the product then the energy of activation will be lowered.

Explanation:

• The energies of of activation can be defined as the energy which is required to cross the threshold level for a reaction to take place.

• there is a transition state that takes place when a reversible reaction moves from the reactant site to the product site and vice versa. However if the transition state is more stable relative to the products then there will be decrease in the activation energy.

To know more about activation energy,

What is the activation energy for a reaction whose rate constant .

..https://brainly.in/question/12218743