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 log 10Q nF 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° - (0.0592) 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. S Provide Fe Part A For the reaction Review | Constants I Periodic Table 2Co+ (aq) + 2Cl(aq)-2Co+ (aq) + Cl₂ (g). E = 0.483 V what is the cell potential at 25 °C if the concentrations are [Co3+]=0.493 M. [Co2+]=0.336 M, and [Cl]=0.669 M, and the pressure of Cl₂ is Pa, 3.10 atm? Express your answer with the appropriate units. ▸ View Available Hint(s) E= Value V Submit rovide Feedback Next>