Chapter 6, Problem 38E

a)

Interpretation Introduction

Interpretation: Whether system with $P_{{\text{H}}_2\text{O}}$ of $1.00\text{ atm}$ , $P_{{\text{Cl}}_2\text{O}}$ of $1.00\text{ atm}$ and $P_{\text{HOCl}}$ of $1.00\text{ atm}$ is at equilibrium or not should be determined. Also, shift in system direction if it is not at equilibrium should be determined.

Concept introduction:Chemical equilibrium is taken into consideration if rate of forward and backward reactions become equal. At this stage, reactants and products have constant concentration. Equilibrium constant is denoted by $K$ .

Reaction quotient is determined with help of initial concentrations of reactants and products. It is denoted by $Q$ . If system is not in equilibrium, direction of shift is determined by comparison of $Q$ and $K$ . Below mentioned are three cases to determine shift of reaction direction.

1. If $Q$ and $K$ are equal, equilibrium is attained and no shift in direction is observed.

2. If $Q$ is greater than $K$ , shift in left direction is observed. This results in more consumption of products and formation of reactants.

3. If $Q$ is less than $K$ , shift in right direction is observed. This results in more consumption of reactants and formation of products.

b)

Interpretation Introduction

Interpretation: Whether system with $P_{{\text{H}}_2\text{O}}$ of $2.00\text{ torr}$ , $P_{{\text{Cl}}_2\text{O}}$ of $49.8\text{ torr}$ and $P_{\text{HOCl}}$ of $21.0\text{ torr}$ is at equilibrium or not should be determined. Also, shift in system direction if it is not at equilibrium should be determined.

Concept introduction:Chemical equilibrium is taken into consideration if rate of forward and backward reactions become equal. At this stage, reactants and products have constant concentration. Equilibrium constant is denoted by $K$ .

Reaction quotient is determined with help of initial concentrations of reactants and products. It is denoted by $Q$ . If system is not in equilibrium, direction of shift is determined by comparison of $Q$ and $K$ . Below mentioned are three cases to determine shift of reaction direction.

1. If $Q$ and $K$ are equal, equilibrium is attained and no shift in direction is observed.

2. If $Q$ is greater than $K$ , shift in left direction is observed. This results in more consumption of products and formation of reactants.

3. If $Q$ is less than $K$ , shift in right direction is observed. This results in more consumption of reactants and formation of products.

c)

Interpretation Introduction

Interpretation: Whether system with $P_{{\text{H}}_2\text{O}}$ of $296\text{ torr}$ , $P_{{\text{Cl}}_2\text{O}}$ of $15.0\text{ torr}$ and $P_{\text{HOCl}}$ of $20.0\text{ torr}$ is at equilibrium or not should be determined. Also, shift in system direction if it is not at equilibrium should be determined.

Concept introduction:Chemical equilibrium is taken into consideration if rate of forward and backward reactions become equal. At this stage, reactants and products have constant concentration. Equilibrium constant is denoted by $K$ .

Reaction quotient is determined with help of initial concentrations of reactants and products. It is denoted by $Q$ . If system is not in equilibrium, direction of shift is determined by comparison of $Q$ and $K$ . Below mentioned are three cases to determine shift of reaction direction.

1. If $Q$ and $K$ are equal, equilibrium is attained and no shift in direction is observed.

2. If $Q$ is greater than $K$ , shift in left direction is observed. This results in more consumption of products and formation of reactants.

3. If $Q$ is less than $K$ , shift in right direction is observed. This results in more consumption of reactants and formation of products.