For the reaction
2Co^{3+}(aq)+2Cl^-(aq) ----> 2Co^{2+}(aq)+Cl2(g).E= 0.71V
what is the cell potential at 25 C if the concentrations are [Co^{3+}]= 0.437M, [Co^{2+}]= 0.109 M, and [Cl^-]= 0.856 M and the pressure of Cl2 is 7.20 atm?
Nernst equation is E=E-({0.0591/{n})*log Q
here E^\circ is the standard reduction potential for the reaction in volts and Q is the reaction quotient. The reaction quotient has the usual form
Q ={ products}]^x / [ reactants}]^y}
i think your answer is
E = Eo - 0.0591/n x log ([Co2+]^2 x PCl2) / ([Co3+]^2 x [Cl-])^2
E = 0.71 - 0.0591 / 2 x log (0.109)^2(7.20)/(0.437)^2(0.856)^2
E = 0.71 + 0.006 = 0.72 V (to 2 sig figs
For the reaction 2Co^3+ (aq) + 2Cl^- (aq) ----> 2Co^2+ + Cl2 (g)
E^o = 0.46 V (STANDARD cell potential)
what is the cell potential at (25 deg C) if the concentrations are [Co^3+] = 0.651M , [Co^2+]= 0.846 M, and [Cl^-] = 0.636 M and the pressure of Cl2 is PCl2= 9.30 atm ?
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