   Chapter 12, Problem 64AE

Chapter
Section
Textbook Problem

# Draw a rough sketch of the energy profile for each of the following cases:a. ∆E = + 10 kJ/mol, Ea = 25 kJ/molb. ∆E = − 10 kJ/mol, Ea = 50 kJ/molc. ∆E = − 50 kJ/mol, Ea = 50 kJ/mol

(a)

Interpretation Introduction

Interpretation: The values of activation energy and ΔE are given. The rough sketch of energy profile are to be drawn for each value of activation energy and ΔE .

Concept introduction: A certain threshold energy which is necessary for the reaction to occur is called activation energy.

The relationship between the rate constant and activation energy is given by the Arrhenius equation,

k=AeEaRT

The change in energy (ΔE) is the energy difference between reactant and product. The value of ΔE is either positive or negative.

To determine: A rough sketch of energy profile for activation energy Ea=25kJ/mol and ΔE=10kJ/mol .

Explanation

The minimum energy needed to start the reaction is known as activation energy.

During a chemical reaction, the minimum amount of energy is required to break the existing bonds. If this minimum energy is less than that of kinetic energy of molecules upon collision, then breaking of bonds takes place and new product is formed.

In energy graph, the highest point indicates the activation energy. The difference between the energy of reactant and the product is represented by ΔE . The value of ΔE can be positive or negative. If the energy of product is less than reactant, then ΔE is negative and if the energy of product is greater than reactant, then ΔE is positive

(b)

Interpretation Introduction

Interpretation: The values of activation energy and ΔE are given. The rough sketch of energy profile are to be drawn for each value of activation energy and ΔE .

Concept introduction: A certain threshold energy which is necessary for the reaction to occur is called activation energy.

The relationship between the rate constant and activation energy is given by the Arrhenius equation,

k=AeEaRT

The change in energy (ΔE) is the energy difference between reactant and product. The value of ΔE is either positive or negative.

To determine: A rough sketch of energy profile for activation energy Ea=50kJ/mol and ΔE=10kJ/mol .

(c)

Interpretation Introduction

Interpretation: The values of activation energy and ΔE are given. The rough sketch of energy profile are to be drawn for each value of activation energy and ΔE .

Concept introduction: A certain threshold energy which is necessary for the reaction to occur is called activation energy.

The relationship between the rate constant and activation energy is given by the Arrhenius equation,

k=AeEaRT

The change in energy (ΔE) is the energy difference between reactant and product. The value of ΔE is either positive or negative.

To determine: A rough sketch of energy profile for activation energy Ea=50kJ/mol and ΔE=50kJ/mol .

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