For the reaction 2Co3+(aq)+2Cl(aq)2Co2+(aq)+Cl2(g). E=0.483 V what is the cell p

Question

For the reaction 2Co3+(aq)+2Cl(aq)2Co2+(aq)+Cl2(g). E=0.483 V what is the cell potential at 25 C if the concentrations are [Co3+]= 0.667 M , [Co2+]= 0.369 M , [Cl]= 0.591 M , and [Cl2]= 0.100 M ?

E=?

Helpful information:

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=E2.303RTnFlog10Q

where E is the potential in volts, E 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 C or 298 K, the equation has the form

E=E(0.0592n)logQ

The reaction quotient has the usual form

Q=[products]x[reactants]y

A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for 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.

Explanation / Answer

Ecell = Eo (cell) - 0.0591/2 log(Co2+)^2 (Cl2)/ (Co3+)^2 (Cl-)^2

= 0.483 - 0.02955 log (0.369)^2 * 0.1 / (0.667)^2 * 0.591 ^2

= 0.483 + 0.0313

= 0.514 V

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