The effect on the equilibrium concentration of FeCl 2+ when F e ( N O 3 ) 3 is added in the given reaction is to be determined. Concept Introduction: Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change. Factor’s that effect chemical equilibria: Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants. Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat. Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium. In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium. If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

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Answer 1

Question

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

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Calculate the equilibrium concentration of H2O for the following esterification reaction performed in ethanol(C2H5OH) C2H5OH + CH3CO2H ⇌CH3CO2C2H5 + H2O KC= 4.0 At equilibrium: [CH3CO2H] = 0.75 M; [CH3CO2C2H5 ]= 2.2 M

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Potassium nitrate is widely used in industries. The reaction for the industrial production of KNO3 is summarized in the equation below; 4KCl + 4 HNO3 + O2 → 4 KNO3 + 2 Cl2 + 2 H2O Which of the following statements below is correct about the production of KNO3? a. A redox reaction; KCl is a reducing agent and O2 is an oxidizing agent b. A redox reaction; HNO3 is a reducing agent and Cl is an oxidizing agent c. Not a redox reaction d. A redox reaction; KCl is a reducing agent and KNO3 is an oxidizing agent e. A redox reaction; HNO3 is a reducing agent and KNO3 is an oxidizing agent

Answer 2

Question

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

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Answer 3

Question

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

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Answer 4

Question

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

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Answer 5

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

Answer 6

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 7

Chapter 7, Problem 7.66AP

(a)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Fe(NO3)3 is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when Cl− is precipitated by addition of AgNO3 in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of FeCl2+ when temperature is increased in the given reaction is to be determined.

Concept Introduction:

Enthalpy (H): It is the total amount of heat in a particular system.

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

Answer 13

(d)

Interpretation Introduction

Interpretation:

The effect on the equilibrium concentration of HI when a catalyst is added in the given reaction is to be determined.

Concept Introduction:

Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.

If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.

Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.

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

Answer 14

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Answer 15

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Answer 17

Ch. 7.1 - Classify each of the following as having potential...Ch. 7.2 - Based on bond energies, which atmospheric gas in...Ch. 7.3 - Prob. 7.1CIAP Ch. 7.3 - How many Calories (i.e., kilocalories) are in a...Ch. 7.3 - Prob. 7.3P Ch. 7.3 - Prob. 7.4P Ch. 7.3 - Prob. 7.5P Ch. 7.3 - Prob. 7.6P Ch. 7.4 - Prob. 7.7P Ch. 7.4 - Prob. 7.8KCP

Solution Summary: The author explains Le Chatelier's principle: if an equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

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