The standard Gibbs energy change (ΔG°) for a reaction can be calculated using the formula:

ΔG° = -nFE°

where:
- n is the number of moles of electrons transferred in the reaction,
- F is the Faraday constant (approximately 96485 C mol^-1), and
- E° is the standard electrode potential.

For a Daniell cell, the reaction is:

Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s)

In this reaction, each zinc atom loses 2 electrons and each copper ion gains 2 electrons. Therefore, n = 2.

Substituting the given values into the formula gives:

ΔG° = -2 * 96485 C mol^-1 * 1.1 V
ΔG° = -212,267 J mol^-1

However, Gibbs energy is usually expressed in kJ mol^-1, so we need to divide this result by 1000 to convert it:

ΔG° = -212.267 kJ mol^-1

So, the standard Gibbs energy for the reaction in a Daniell cell is -212.267 kJ mol^-1.

Question

The standard Gibbs energy change (ΔG°) for a reaction can be calculated using the formula:

ΔG° = -nFE°

where:
- n is the number of moles of electrons transferred in the reaction,
- F is the Faraday constant (approximately 96485 C mol^-1), and
- E° is the standard electrode potential.

For a Daniell cell, the reaction is:

Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s)

In this reaction, each zinc atom loses 2 electrons and each copper ion gains 2 electrons. Therefore, n = 2.

Substituting the given values into the formula gives:

ΔG° = -2 * 96485 C mol^-1 * 1.1 V
ΔG° = -212,267 J mol^-1

However, Gibbs energy is usually expressed in kJ mol^-1, so we need to divide this result by 1000 to convert it:

ΔG° = -212.267 kJ mol^-1

So, the standard Gibbs energy for the reaction in a Daniell cell is -212.267 kJ mol^-1.

Knowee AI · Accepted Answer

The standard Gibbs energy change (ΔG°) for a reaction can be calculated using the formula:

ΔG° = -nFE°

where:
- n is the number of moles of electrons transferred in the reaction,
- F is the Faraday constant (approximately 96485 C mol^-1), and
- E° is the standard electrode potential.

For a Daniell cell, the reaction is:

Zn(s) + Cu^2+(aq) → Zn^2+(aq) + Cu(s)

In this reaction, each zinc atom loses 2 electrons and each copper ion gains 2 electrons. Therefore, n = 2.

Substituting the given values into the formula gives:

ΔG° = -2 * 96485 C mol^-1 * 1.1 V
ΔG° = -212,267 J mol^-1

However, Gibbs energy is usually expressed in kJ mol^-1, so we need to divide this result by 1000 to convert it:

ΔG° = -212.267 kJ mol^-1

So, the standard Gibbs energy for the reaction in a Daniell cell is -212.267 kJ mol^-1.

the standard electrode potential of a daniell cells is 1.1V. find the standard gibbs energy for the reaction

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