To learn how to use the Nernst equation. The standard reduction potentials liste

Question

To learn how to use the Nernst equation.

The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 C and 1 M. To calculate the cell potential at non-standard-state conditions, one uses the Nernst equation,

E=E2.303RTnFlog10Q

where E is the potential in volts, E is the standard potential in volts, R=8.314J/(Kmol) is the gas constant, Tis the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e) is the Faraday constant, and Q is the reaction quotient.

Substituting each constant into the equation the result is

E=E0.0592 Vnlog10Q

Part E

What is the cell potential for the reaction

Mg(s)+Fe2+(aq)Mg2+(aq)+Fe(s)

at 81 C when [Fe2+]= 3.20 M and [Mg2+]= 0.310 M .

E =

Explanation / Answer

Ecell = Eº - RT/nF lnQ

Ecell = Eº - (8.314)(354)/(2)(96485) ln 0.0186

the standard potential(Eº) of the cell is not given.

if you submit the Eº you will get teh cell potential, E

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