Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is H + (aq) capable of oxidizing Cu( s ) to Cu 2+ ( aq )? b. Is Fe 3+ ( aq ) capable of oxidizing I − ( aq )? c. Is H 2 ( g ) capable of reducing Ag + ( aq )?

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of H+(aq) to oxidize Cu(s) to Cu2+(aq)

Due to negative value of E°cell it is not possible for H+(aq) to oxidize Cu(s) to Cu2+(aq)

The reaction taking place at cathode is,

2H+(aq)+2e−→H2(g)   E°red=0.00 V

The reaction taking place at anode is,

Cu(s)→Cu2+(aq)+2e−   E°ox=−0.34 V

The overall cell potential is calculated as,

E°cell=E°ox+E°red=−0

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of Fe3+(aq) to oxidize I−(aq) .

Interpretation:

Various questions on the oxidizing and reducing tendency of species based on their reduction potential are to be answered.

Concept introduction:

The species with higher reduction potential undergoes reduction at the cathode while the species with lower reduction potential undergoes oxidation at the anode. The change in Gibbs free energy is the useful amount work that can be done and negative value of ΔG° shows that the reaction is spontaneous in nature.

To determine: The ability of H2(g) to reduce Ag+(aq) .