The mixture which is at equilibrium when K > 1 , = 1 o r < 1 has to be identified using the given reaction spices. Concept introduction: Chemical equilibrium : The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant. Reaction quotient ( Q ) : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations. Q= [ Product ] [ Reactant ] The reaction quotient ( Q ) is helpful in predicting the direction of the reaction. When Q > K c , the reaction proceeds towards left to increase the concentration of the reactants. When Q < K c , the reaction proceeds towards right to increase the concentration of the products. When Q = K c , the reaction is at equilibrium.

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Answer 1

Question

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

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Answer 2

Question

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Answer 6

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Answer 7

Chapter 20, Problem 20.103P

(a)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $K>1, =1 or < 1$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The mixture which is at equilibrium when $Kp>Kc, =Kc or < Kc$ has to be identified using the given reaction spices.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The given reaction spices, the $ΔGrxno$ value should be calculated.

Concept introduction:

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K) ΔGo=- RT ln (K)$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy change.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The purple molecules represented $H2$ and blue molecule is $I2$ . Using the given reaction spices the $ΔGrxno$ value should be explained.

Concept introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Answer 14

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Answer 15

Expert Solution & Answer

Answer 16

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Answer 17

Ch. 20.1 - Select the substance with the higher entropy in...Ch. 20.1 - Select the substance with the lower entropy in...Ch. 20.2 - Balance each equation, predict the sign of if...Ch. 20.2 - Balance each equation, predict the sign of if...Ch. 20.2 - Gaseous phosphorus trichloride forms from the...Ch. 20.2 - Prob. 20.3BFP Ch. 20.3 - Use and to calculate at 298 K for this...Ch. 20.3 - Prob. 20.4BFP Ch. 20.3 - Use values to calculate at 298 K: 2NO(g) +...Ch. 20.3 - Prob. 20.5BFP

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