Question

Consider the following standard reduction potentials of some commonly used metals:
ξo (V)
Au3+ (aq) + 3 e- → Au (s) +1.50
Ag+ (aq) + e- → Ag (s) +0.80
Cu2+ (aq) + 2e- → Cu (s) +0.34
Fe3+ (aq) + 3e- → Fe (s) -0.036V
Al3+ (aq) + 3e- → Al (s) -1.66
Mg2+ (aq) + 2e- → Mg (s) -2.37

Using the reduction potentials one can compare the reactivities of metals towards oxidation- reduction processes. Evaluate the following statements and determine if they are True or False.
1. Cu2+ (aq) can oxidize Fe (s).
2. Aluminum has a strong tendancy to be oxidized and is therefore not a precious metal.
3. A positive reduction potential means that the metal is more stable in its ionic state (aq) than in its reduced state (s).
4. Cu (s) can be oxidized by Au3+ (aq).
5. Elemental copper (Cu (s)) is more stable than elemental iron (Fe (s)).

Answer 1

Instead of someone just giving you the answers, I would like to know what it is you don't understand.