Question

Constants
The following values may be useful when solving this tutorial.
Constant
E°Cu | 0.337V
E°Co | -0.277V
R.      | 8.314 J•mol^-1•K^-1
F       | 96485 C/mol
T.      | 298 K

In the activity, click on the E°cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occurs in the cell are
Cu^2+(aq)+2e^->Cu(s)
and
Co(s)>Co^2+(aq)+2e^-
The net reaction is Cu^2+(aq)+Co(s)>Cu(s)+Co^2+(aq)

Answer 1

Sol: the Given net Reaction is 2+ cu² (aq) + COCs) > Cu Cs) +Col*a91 the half cell reactions are shown below: At Cathode : cet? (29) - Cucs) E'= 0.337 V At anode : CoCS) — Co2+Q2). = -0.274V the standard cell potential is as follows: Eiele = Ecathode - Eanode = 0.337V -(-0.277V) O. 6144 v Equiliblicum constant k by using following relation 0.0592 E cell Togk n 0.614 V = 0.0592 logk 2 log K = 0.614) (2) = 20.74 0.0592 K = 20174 10 = 5.49x1020 Equilibricem constant, K=5.49x109 26