Constants 1 Periodic Table Part A The Nermst equation is one of the most importa

Question

Constants 1 Periodic Table Part A The Nermst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is For the reactionNW 2Co3 (ag) +2()2 (aq) +C(). 0483 V what is the cell potential at 25 °C if the concentrations are [Co3+)-0.104 M. (Co2+1- 0.579 M, and (Cl]0.797 M, and the pressure of Cl2 is Pcl, 740 atm? Express your answer with the appropriate units. , View Available Hint(s) E- E 2.303 RT 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-Value Units Submit Ans E-E?.. (0.0592) logQ X Incorrect: Try Again; 4 attempts remaining rn The reaction quotient has the usual form products reactants

Explanation / Answer

2Co^3+ (aq) + 2Cl^- (aq) -------------> 2Co^2+ (aq) + Cl2(g)      E0 = 0.483v

n   = 2 electrons are involve

Ecell    = E0cell - 0.0592/nlogQ

Ecell   = 0.483 - 0.0592/2 log[Co^2+]^2PCl2/[Co^3+]^2[Cl^-]^2

           = 0.483 - 0.0296 log(0.579)^2*7.4/(0.104)^2(0.797)^2

         = 0.483 -0.0296log361.08

          = 0.483-0.0296*2.5576   = 0.4073v >>>>answer

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