The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at

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˚-(2.303 RT/nF) * log10
where E is the potential in volts, Eº 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, and F is the Faraday constant, and is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E˚-[(0.0592)/n] log Q
The reaction quotient has the usual form
Q =[products]"/[reactants]"
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.
For the reaction 
2Co³+ (aq) + 2Cl-(aq)→2Co²+ (aq) + Cl₂ (g). Eº = 0.483 V
what is the cell potential at 25°C if the concentrations are [Co³+] =0.598M, [Co²+]= 0.773M and [Cl-]= 0.890M and the pressure of Cl₂ is PCl2 = 5.30 atm ? Express your answer with the appropriate units.

Kunduz · Accepted Answer

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