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 Part A E E- 2.303 RT logO For the reaction nF 2C03 (aq)2Ci (aq)+2C02+ (aq) Cl2 (g). E = 0.483 V where E is the potential in volts, E° is the standard potential in volts, R is the gas constant, T what is the cell potential at 25 °C if the concentrations are Co3+ M, and the pressure of Cl2 is P = 5.50 atm? 0.585 M, [Co2+1= 0.110 M, and CIF1 = 0.580 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 Express your answer with the appropriate units. View Available Hint(s) 0.0592logQ E E°- HA The reaction quotient has the usual form Q= products reactants Value Units E= 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 Nemst equation allows for the calculation of the cell potential E at other conditions of concentration and Previous Answers Submit Incorrect; Try Again; 4 attempts remaining pressure.

Answer 1

NERST EQUATION Eun = Eco -0,0591092 0 [Coʻ+]° x Por =1Co* j* *[CI-T we have to calculate concentration of Cl, from pressure [C] = RI - 0.0821x298 TOP - 5.5_ =0.224M = Equ=0.483-2 10[0.585]" x[0.580) =0.59V = Eq=0.483 -0.059 [0.110] x0.224