Question

Draw an energy diagram for an endothermic reaction without a catalyst (use a solid line) and with a catalyst (use a dotted line) Label all parts of the diagram. Explain what a catalyst is and how a catalyst influences the rate of reaction.
If you cannot draw it, can you at least explain how I would do this?

Answer 1

- Endothermic reaction : so the energy of product is higher than the energy of reactant.
- Catalyst lowers the activation energy so it increase the rate of reaction.
- The graph is attached:

Answer 2

Explanation:

Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and $\Delta H$ for the reaction comes out to be positive.

Catalyst is the substance which does not participate in the reaction but increases the rate of the reaction and results in the early formation of product.

Labeling of the parts in the diagram:

• A represents the reactants.
• B represents the products.
• C And D represents the activated complex. C is the activated complex formed without catalyst and D is the activated complex formed with catalyst.
• E represents the potential energy of the reactants.
• F represents the potential energy of the products.
• G represents the activation energy when no catalyst is used in the reaction.
• H represents the activation energy when a catalyst is used in the reaction.
• I represents the total enthalpy change of the reaction, which comes out to be positive for endothermic reaction.

The energy diagram for an endothermic reaction is attached in the image below.