Chapter 6, Problem 50IP

(a)

Interpretation Introduction

Interpretation: The two characteristic arrow pushing patterns for the given mechanism is to be interpreted.

  

Concept introduction:

A chemical reaction can complete in more than one step. Such reactions are called multistep reactions. It occurs with the formation of intermediates. The formation of intermediate can be shown with the help of curved arrows.

(b)

Interpretation Introduction

Interpretation: The process is the be interpreted as exothermic and endothermic for the given reaction with the help of the energy profile diagram.

Concept introduction:

The energy profile diagram shows the progress of the chemical reaction. It is the curve between the energy and reaction coordinate of the reaction. It can be used to predict the formation of transition state and product from the given reactant.

(c)

Interpretation Introduction

Interpretation: The $\Delta {\text{S}}_{sys}$ of the process is to be interpreted as positive, negative or approximate zero for the given reaction.

  

Concept introduction:

Entropy is the measurement of the randomness of a chemical system. As the randomness increases, the entropy of the system also increases. Entropy gets affected by the number of molecules in a system, physical state, and presence of ions.

(d)

Interpretation Introduction

Interpretation: The $\Delta \text{G}$ of the process is to be interpreted as positive or negative for the given reaction.

Concept introduction:

A chemical reaction involves the conversion of one or more reactant molecules to product molecules. The Gibb’s equation provides the relation between $\Delta \text{S}$ , $\Delta \text{H}$ , and $\Delta \text{G}$ of the reaction.

  $\Delta \text{G = }\Delta \text{H - T }\Delta \text{S}$

(e)

Interpretation Introduction

Interpretation: The transition state and its location on the energy diagram for the given reaction is to be interpreted.

Concept introduction:

A chemical reaction involves the conversion of one or more reactant molecules to product molecules. The reactant molecules come close to each other and collide effectively to form the transition state that further changes to the product.

(f)

Interpretation Introduction

Interpretation: The closeness of transition state to reactant or product is to be interpreted for the given reaction.

Concept introduction:

A chemical reaction involves the conversion of one or more reactant molecules to product molecules. The reactant molecules come close to each other and collide effectively to form the transition state that further changes to the product.

(g)

Interpretation Introduction

Interpretation: The order of reaction is to be interpreted for the given reaction.

Concept introduction:

The rate of a chemical reaction can be defined as the change in the concentration of the reactant within the given time. The rate law states that the rate of the chemical reaction is directly proportional to the active concentration of the reactant molecules. The proportionality constant is called the rate constant.

(h)

Interpretation Introduction

Interpretation: The effect of the doubled concentration of the hydroxide ion is to be interpreted for the given reaction.

Concept introduction:

The rate of a chemical reaction can be defined as the change in the concentration of the reactant within the given time. The rate law states that the rate of the chemical reaction is directly proportional to the active concentration of the reactant molecules. The proportionality constant is called the rate constant.

(i)

Interpretation Introduction

Interpretation: The effect of increasing the temperature is to be interpreted for the given reaction.

Concept introduction:

The energy profile diagram shows the progress of the chemical reaction. It is the curve between the energy and reaction coordinate of the reaction. It can be used to predict the formation of transition state and product from the given reactant.