Question

The value of Eºcell for the following reaction is 0.500 V. 2Mn3+ + 2H20 Mn2+ + MnO2 +4H What is the value of AG cell for this reaction? = kJ

Answer 1

The value of ΔG° for an electrochemical reaction can be calculated using the formula ΔG° = -nFE°cell, but the number of moles of electrons transferred (n) is required, which is not given in the question.

Step-by-step explanation:

The question asks about the relationship between the standard cell potential (E°cell) and the free energy change (ΔG°) of an electrochemical reaction under standard conditions.

The student wants to determine the ΔG° for a specific reaction using the given E°cell value of 0.500 V.

To calculate the free energy change (ΔG°) for the reaction, we use the formula:

ΔG° = -nFE°cell

where:

n is the number of moles of electrons transferred in the reaction,

F is Faraday's constant (96,485 C/mol e−),

E°cell is the standard cell potential.

However, as the number of moles of electrons (n) isn't provided in the question, we cannot calculate the exact value of ΔG°.

Usually, n corresponds to the balanced overall redox reaction.

Since the half-reactions and stoichiometry are not provided, the student would need this additional information to determine n and proceed with the calculation.

Answer 2

The value of ΔGº for the given redox reaction is -96.485 kJ/mol.

Step-by-step explanation:

The value of Eºcell for a redox reaction is a measure of the electrical potential difference between the two half-cell reactions involved. In this case, the reaction is:

2Mn3+ + 2H2O → Mn2+ + MnO2 + 4H+

Given that Eºcell = 0.500 V, we can use the formula:

ΔGº = -nFEºcell

where ΔGº is the standard Gibbs free energy change, n is the number of moles of electrons transferred, F is Faraday's constant (96485 C/mol), and Eºcell is the standard cell potential.

Therefore, to find the value of ΔGº, we need to determine the number of moles of electrons transferred in the reaction. From the balanced equation, we can see that 2 moles of electrons are transferred. Thus, we have:

ΔGº = -2 * 96485 C/mol * 0.500 V = -96485 C/mol

Since the unit of Coulombs (C) is equivalent to Joules (J) in this context, the value of ΔGº for this reaction is -96485 J/mol = -96.485 kJ/mol.