The solubility product for CuI(s) is 1.1 × 10 −2 Calculate the value of for the half-reaction CuI ( s ) + e − → Cu ( s ) + I − ( a q )

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Interpretation Introduction Interpretation: A half-cell reaction is given. The value of E ° for the given cell reaction is to be calculated. Concept introduction: The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation. The value of E cell is calculated using Nernst formula, E = E ° − ( R T n F ) ln ( Q ) At room temperature the above equation is specifies as, E = E ° − ( 0.0591 n ) log ( Q ) This relation is further used to determine the relation between Δ G ° and K , Δ G ° and E ° cell . Solubility product is applied only for those ionic compounds that are sparingly soluble. The product of solubility of ions is called solubility product and solubility is present in moles per liter. To determine: The value of cell potential E ° for the given cell reaction. Explanation Given The cell reaction is, CuI ( s ) + e − → Cu ( s ) + I − ( a q ) The value of standard reduction potential is, Cu + + e − → Cu E ° = 0.52 V The value of solubility product constant is, CuI ( s ) → Cu + ( a q ) + I − ( a q ) K sp = 1.1 × 10 − 12 The reaction involves the transfer of 1 mole of electrons. The standard cell potential at room temperature can be calculated by using the formula, E ° = 0.0591 n log K sp Where, E o is the standard cell potential. n is the number of moles of electron transfer. K sp is the solubility product constant. Substitute the values of n and K sp in the above equation, E ° = 0.0591 n log K sp = 0.0591 1 log ( 1

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Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation:

A half-cell reaction is given. The value of E° for the given cell reaction is to be calculated.

Concept introduction:

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

This relation is further used to determine the relation between ΔG° and K , ΔG° and E°cell .

Solubility product is applied only for those ionic compounds that are sparingly soluble. The product of solubility of ions is called solubility product and solubility is present in moles per liter.

To determine: The value of cell potential E° for the given cell reaction.

Explanation of Solution

Given

The cell reaction is,

CuI(s)+e−→Cu(s)+I−(aq)

The value of standard reduction potential is,

Cu++e−→Cu E°=0.52 V

The value of solubility product constant is,

CuI(s)→Cu+(aq)+I−(aq) Ksp=1.1×10−12

The reaction involves the transfer of 1 mole of electrons.

The standard cell potential at room temperature can be calculated by using the formula,

E°=0.0591nlog Ksp

Where,

Eo is the standard cell potential.
n is the number of moles of electron transfer.
Ksp is the solubility product constant.

Substitute the values of n and Ksp in the above equation,

E°=0.0591nlog Ksp=0.05911log (1

The solubility product for CuI(s) is 1.1 × 10 −2 Calculate the value of for the half-reaction CuI ( s ) + e − → Cu ( s ) + I − ( a q )

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

The solubility product for CuI(s) is 1.1 × 10⁻² Calculate the value of for the half-reaction

CuI ( s ) + e − → Cu ( s ) + I − ( a q )

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The solubility product for CuI(s) is 1.1 × 10 −2 Calculate the value of for the half-reaction CuI ( s ) + e − → Cu ( s ) + I − ( a q )

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach