Question

Using the Nernst Equation:

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=E??2.303RTnFlog10Q

where E is the potential in volts, E? is the standard potential in volts, R=8.314J/(K?mol) is the gas constant, T is 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=E??0.0592 Vnlog10Q

Part E What is the cell potential for the reaction the reaction Mgs) Mg(s) + Fe2+ (aq) →Mg2 + (aq) + Fe(s) Express your answer to three significant figures and include the appropriate units 2 EValueUnits Submit Hints My Answers Give Up Review Part