At 37 °C the concentration of Fe3+ inside a cell is 0.053 M and outside is 0.044 M. The cell membrane is permeable to Fe3+. What potential difference in volts would have to exist across the membrane for Fe3+ to be in equilibrium at the stated conditions? Give you answer as the absolute value of the potential difference in volts.

The potential difference in volts would have to exist across the membrane for Fe³⁺ to be in equilibrium at the stated conditions is 0.000720 V.

How we calculate potential difference?

We can calculate the potential difference by using the Nernst Equation as:

Ecell = E°cell - RT/nF log [Fe³⁺]o/[Fe³⁺]i

Following values for this question as:

[Fe³⁺]i concentration of Fe³⁺ inside the cell = 0.053M

[Fe³⁺]o concentration of Fe³⁺ outside the cell = 0.044M

T temperature = 37°C = 310K

F faradays constant = 9.6485 × 10⁴ C/mole

n valency of Fe³⁺ = 3

R universal gas constant = 8.314 J/mol.K

E°cell standard electrode potential = 0

On putting all these values on the above equation, we get the value of potential difference as:

Ecell = -(8.314)(310)/3×9.6485×10⁴ × log(0.044)/(0.053)

Ecell = -(2,577.34/289,455) × -0.0809

Ecell = 0.000720 V

Hence, potential difference is 0.000720 V.

To know more about Nernst equation, visit the below link:
https://brainly.com/question/15394851