Question

What is the value of the activation energy of the uncatalyzed reaction? Express your answer to three significant figures and include the appropriate units.

Answer 1

Answer:

175 kJ

Explanation:

Activation energy can be defined as the potential energy that is needed to change reactants to products. This is the minimum energy required for the chemical reaction to take place. Thus, using the given figure:

Activation energy = activation complex - reactant energy

In the given figure, activation complex = 400 kJ

reactant energy = 225 kJ

Therefore:

Activation energy = 400 - 225 = 175 kJ

Answer 2

Answer:

175KJ

Explanation:

I will assume the diagram is as in the attachment I’ve supplied herein.

Activation energy is the minimum energy required by reactant particles for a chemical reaction to occur. Depending on reaction conditions, especially for reversible reactions, reactants can become products and vice versa.

Activation energy for a forward reaction = energy of the activated complex (transition state) – energy of the reactants.

Activation energy for a reverse reaction = energy of the activated complex – energy of the products.

For the forward reaction above, reading the values from the diagram,

Activation energy = energy of the activated complex –energy of the reactants

Activation energy = (400 – 225)KJ = 175KJ