Vanadium is a transition metal that can form a variety of ions with multiple oxidation states possible. This question is about the reactions of vanadium ions.
Deduce the oxidation state of vanadium in each of the following ions:
- V2+
- VO2+
- VO2+
- V3+
The standard electrode potentials for two half equations are shown below:
Half equations | Eθ / V |
VO2+ (aq) + 2H+ (aq) + e- H2O (l) + VO2+ (aq) | +1.00 |
S4O62- (aq) + 2e- 2S2O32- (aq) | +0.47 |
[1]
[1]
Calculate the standard cell potential between half cells containing VO2+ (aq)/VO2+ (aq) and containing S4O62- (aq)/ S2O32- (aq), using information from the table below.
Half equations | Eθ / V |
VO2+ (aq) + 2H+ (aq) + e- H2O (l) + VO2+ (aq) | +1.00 |
S4O62- (aq) + 2e- 2S2O32- (aq) | +0.47 |
Some other reactions of vanadium ions are shown below:
Half equations | Eθ / V |
Zn2+ (aq) + 2e- Zn(s) | -0.76 |
V3+ (aq) + e- V2+ (aq) | -0.26 |
Sn2+ (aq) + 2e- Sn (s) | -0.14 |
VO2+ (aq) + 2H+ (aq) + e- H2O (l) + V3+ (aq) | +0.34 |
S4O62- (aq) + 2e- 2S2O32- (aq) | +0.47 |
VO2+ (aq) + 2H+ (aq) + e- H2O (l) + VO2+ (aq) | +1.00 |
[1]
[1]
Did this page help you?