Question

Part A For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).

E∘=0.483 V

what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 0.469 M , [Co2+]= 0.448 M , and [Cl−]= 0.850 M and the pressure of Cl2 is PCl2= 5.80 atm ?

Express your answer with the appropriate units.

Answer 1

2Co³⁺(aq) + 2Cl⁻(aq) → 2Co²⁺(aq)+Cl₂(g)

Co³⁺(aq) + e - → Co²⁺(aq)

Cl₂ (g) + 2e- → 2Cl- (aq)

no of electrons transferred n = 2

E∘=0.483 V

[Co3+]= 0.469 M , [Co2+]= 0.448 M , and [Cl−]= 0.850 M and the pressure of Cl2 is PCl2= 5.80 atm

E_cell = E^o_cell - [0.059/n] Iog {[Co²⁺]² PCl2/ [Co³⁺]² [Cl-]²}   

       = 0.483 - [0.059/2] Iog {[0.448]² [5.8]/ [0.469]² [0.85]²}   

       = + 0.457 V

E_cell = + 0.457 V

Therefore,

cell potential = + 0.457 V