The Nernst equation is one of the most important equations in electrochemistry.

Question

The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non- standard-state conditions, the equation is E=E degree -2.303 RT/nF logio Q where E is the potential in volts. En is the standard potential in volts. R is the gas constant. T is the temperature in kelvins. n is the number of moles of electrons transferred. F is the Faraday constant, and Q is the reaction quotient. At standard temperature. 25 degree C or 298 K. the equation has the form E=E degree - (0.0592/n) log Q The reaction quotient has the usual form Q =[products]1/[reactants]y A table of standard reduction potentials gives the voltage at standard conditions. 1.00 Mfor all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. For the reaction 2Co3' (aq) + 2C1 (aq)->2Co2f (aq) + Cl2(g). S' =0.483 V what is the cell potential at 25 degreeC if the concentrations are [Co3+ ] = 0.677 M. [Co2+ ] = 0.124 M. and [Cl ] = 0.239 M and the pressure of CI-2 is Pci0 = 5.50 atm ? Express your answer with the appropriate units.

Explanation / Answer

Ecell = E0cell-0.0591/nlog(pcl2*[Co2+]^2/[Cl-]^2[Co^3+]^2)

     = 0.483 - (0.0591/2)log(5.5*0.124^2/(0.239^2*0.677^2))

   = 0.468 V

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