Chapter 19, Problem 89GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Calculate equilibrium constants for the following reactions at 298 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. (a) 2 Cl−(aq) + Br2(ℓ) ⇄ Cl2(aq) + 2 Br−(aq) (b) Fe2+(aq) + Ag+(aq) ⇄ Fe3+(aq) + Ag(s)

(a)

Interpretation Introduction

Interpretation:

The equilibrium constants for the following reactions at 298 K have to be determined and also determine the equilibrium is a reactant or product favoured at equilibrium.

(a) 2Cl-(aq) + Br2(l) Cl2(g) + 2Br-(aq)

Concept introduction:

According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system.

The equation is as follows.

ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol  E0= Volts = Work(J)/Charge(C)

The relation between standard cell potential and equilibrium constant is as follows.

lnK = nE00.0257 at 298K

Explanation

The given chemical reaction is as follows.

Â 2Cl-(aq)Â +Â Br2(l)Â â†’Cl2(g)Â +Â 2Br-(aq)

Letâ€™s write an each half cell reaction.

AtÂ anode:OxiationÂ :Â Cl2(aq)Â +Â 2eâˆ’Â â†’Â 2Clâˆ’(aq)AtÂ cathode:ReductionÂ :Â Br2(l)Â +Â 2eâˆ’â†’2Br-(aq)

Letâ€™s calculate the Ecello of the reaction.

Ecello=Â ECathode0-Â EAnode0=Â 1.08Â V-(1.36Â V)=Â -0.28Â V

Letâ€™s calculate the Î”G0 for the reaction.

Î”G0=Â -nFE0nÂ =Â 2FÂ =Â 96485C/molÂ Â E0=Â -0

(b)

Interpretation Introduction

Interpretation:

The equilibrium constants for the following reactions at 298 K have to be determined and also determine the equilibrium is a reactant or product favoured at equilibrium.

(b) Fe2+(aq) + Ag+(aq) Fe3+(aq) + Ag(s)

Concept introduction:

According to the first law of thermodynamics, the change in internal energy of a system is equal ti the heat added to the sysytem minus the work done by the system.

The equation is as follows.

ΔU = Q - WΔU = Change in internal energyQ = Heat added to the systemW=Work done by the system

In voltaic cell, the maximum cell potential is directly related to the free energy difference between the reactants and products in the cell.

ΔG0= -nFE0n = Number of moles transferred per mole of reactant and productsF = Faradayconstant=96485C/mol  E0= Volts = Work(J)/Charge(C)

The relation between standard cell potential and equilibrium constant is as follows.

lnK = nE00.0257 at 298K

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