For a reaction, an energy diagram needs to be drawn having a high E a and value of Δ H = + 20 kcal/mol . Concept Introduction: In energy diagram, energy versus progress of the reaction-the reaction coordinates are plotted. Reactants are placed in the left side and products in right side. These reactants and products are connected by a smooth curve that represent how energy change with time. When two reactions approach each other, a repulsion takes place, so the energy is increased until a maximum value is achieved. This state is called transition state and energy difference between the transition state and reactants are called the activation energy, E a . As the bonds form between the reactants, the energy decreases until a stable minimum energy is achieved. The difference in energy between the reactants and the products is the enthalpy change, ΔH.

Question

V Consider this step in a radical reaction: Br: ? What type of step is this? Check all that apply. Draw the products of the step on the right-hand side of the drawing area below. If more than one set of products is possible, draw any set. Also, draw the mechanism arrows on the left-hand side of the drawing area to show how this happens. ⚫ionization termination initialization neutralization none of the abc Explanation Check 80 Ο F3 F1 F2 2 F4 01 % do5 $ 94 #3 X 5 C MacBook Air 25 F5 F6 66 ©2025 ˇ F7 29 & 7 8

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Question

Chapter 6.3, Problem 6.10P

Interpretation Introduction

Interpretation:

For a reaction, an energy diagram needs to be drawn having a high E_a and value of ΔH=+20 kcal/mol.

Concept Introduction:

In energy diagram, energy versus progress of the reaction-the reaction coordinates are plotted. Reactants are placed in the left side and products in right side. These reactants and products are connected by a smooth curve that represent how energy change with time.

When two reactions approach each other, a repulsion takes place, so the energy is increased until a maximum value is achieved. This state is called transition state and energy difference between the transition state and reactants are called the activation energy, E_a. As the bonds form between the reactants, the energy decreases until a stable minimum energy is achieved. The difference in energy between the reactants and the products is the enthalpy change, ΔH.

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