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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.

Respuesta :

meerkat18

Use the nernst equation : Ecell=E−RTnFln[Fe3+out][Fe3+in] At eq. ΔG=0=−nFEcell→Ecell=0 and thus: E=RTnFln[Fe3+out][Fe3+in]

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

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