A cell consists of Ag(s) | Ag + and Cu (s) | Cu 2+ electrodes. If the concentrations of Ag + (aq) and Cu 2+ (aq)
are 2 x 10 -6 M and 3 x 10 -3 M respectively, what is the emf of the cell at 298 K?
22.4)
The standard cell potential E o for the following cell was found to be 0.2684 V at 298 K and 0.2669 V at 303
K.
Pt | H 2 (g) | HCl (aq) | Hg 2 Cl 2 (s) | Hg (l)
Write the cell reaction, calculate r Go at 298 K and also r S o and r H o for the reaction at 298 K and 303 K.
22.5)
The standard Gibbs free energy for the formation of ions f is defined as the free energy change for
the process
M(s, or its most stable state at temperature T) M + (aq) + e
For the reaction ½ H 2 (g) H + (aq) + e, f G oH+ (aq) is taken as zero. Combining the SHE with a) Ag | Ag+ electrode and b) Na | Na + electrodes, find f for Ag+ and Na+ ions from their respective cell potentials w.r.t. the SHE.
22.6)
Devise suitable cells in which the following reactions can be carried out:
a)
H 2 (g) + Cl 2 (g) 2 HCl (aq)
b)
Cu 2+ (aq) + Cu (s) 2 Cu+ (aq)
c)
H 2 (g) + O 2 (g) 2 H 2 O ( l )
d)
Na (s) + H 2 O (l) NaOH(aq) +1/ 2 H 2 (g)
If some of the cell potentials are not found in this web course, please consult any of the reference textbooks mentioned in the Overview given at the beginning of the course.
r Go at 298 K and also 
is defined as the free energy change for 
M + (aq) + e 
2 HCl (aq) 
