2. The activity of water at 11 bar and 298 K is
3. Given that E°(Fe3+, Fe) = -0.4 V and E°(Fe2+, Fe) = -0.44 V, the value of E°(Fe3+, Fe2+) is
4. According to the Debye-Huckel limiting law, if the concentration of a dilute aqueous solution of KCl is increased 4-fold, the value of In γz (γz is the molar mean ionic activity coefficient) will
5. Given the standard potential for the following half-cell reaction at 298 K,
Cu+(aq) + e- → Cu(s); E° = 0.52 V
Cu2+(aq) + e- → Cu+(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu+(aq) → Cu(s) + Cu2+]
Cu+(aq) + e- → Cu(s); E° = 0.52 V
Cu2+(aq) + e- → Cu+(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu+(aq) → Cu(s) + Cu2+]
6. A student recorded a polarogram of 2.0 mM Cd2+ solution and forget to add KCl solution. What type of error do you expect in his results?
7. For a 2 molal aqueous NaCl solution, the mean ionic activity coefficient $$\left( {{\gamma _ \pm }} \right)$$ and the Debye-Huckel Limiting Law constant (A) are related as
8. The standard reduction potentials at 298 K for single electrodes are given below.
Electrode
Electrode potential (volt)
Mg2+ /Mg
-2.34
Zn2+ /Zn
-0.76
Fe2+ /Fe
-0.44
From this we can infer that
Electrode | Electrode potential (volt) |
Mg2+ /Mg | -2.34 |
Zn2+ /Zn | -0.76 |
Fe2+ /Fe | -0.44 |