   Chapter 14, Problem 100SCQ

Chapter
Section
Textbook Problem

Draw a reaction coordinate diagram for an exothermic reaction that occurs in a single step. Identify the activation energy and the net energy change for the reaction on this diagram. Draw a second diagram that represents the same reaction in the presence of a catalyst, assuming a single-step reaction is involved here also. Identify the activation energy of this reaction and the energy change. Is the activation energy in the two drawings different? Does the energy evolved in the two reactions differ?

Interpretation Introduction

Interpretation:

The reaction coordinate diagram should be drawn for single step exothermic reaction and to indicate how the activation energy changes with respect to addition of catalyst to the reaction and also the energy change involved in the reaction before and after addition of catalyst should be discussed.

Concept Introduction:

In order to establish the plausibility of a mechanism, one must compare the rate law of the rate determining step to the experimentally determined rate law.

Rate determining step: In a chemical reaction the rate determining step is the slowest step in which the rate of the reaction depends on the rate of that slowest step.

Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.

Reactant: In a chemical reaction the species that present left is denoted as reactant which undergoes chemical change and result to given new species called product.

Product: In a chemical reaction the species that present in right side is denoted as product that results from the reactant.

Reaction coordinate: It is the diagrammatic representation of a chemical reaction which depicts how the reactants gets transformed into product where the transition state and the intermediates present in the reaction are also depicted.

Enthalpy change: The change in the energy as the product formed from the reactants is represented by the enthalpy change in the reaction coordinate diagram.

Intermediate species: It is the species formed during the middle of the chemical reaction between the reactant and the desired product.

Exothermic Reaction: In a chemical reaction if the energy of reactants are higher than the corresponding products which means the energy is released in the form of heat then that chemical reaction is considered as exothermic.

Explanation

Consider the chemical reaction AB which is actually a single step exothermic reaction. The reaction becomes exothermic when energy is released that means the energy of product is less when compared with the energy of the reactant.

This shows that the reactant A is higher in energy and the product B is lower in energy.

The reaction is a single step hence it has only one transition without any intermediate in-between them.

The diagram for this reaction is depicted as below,

Now, diagram is drawn for the same reaction but this time with addition of catalyst. A catalyst is a substance which is used to lower the activation energy without getting involved in the reaction

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