Answer the following questions using data from Table 17-1 (all under standard conditions). a. Is H 2 ( g ) capable of reducing Ni 2+ ( aq )? b. Is Fe 2+ ( aq ) capable of reducing VO 2 + ( aq )? c. Is Fe 2+ ( aq ) capable of reducing Cr 3+ ( aq) to Cr 2+ ( 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 oxidize Cu(s) to Ni2+(aq)

Due to negative value of E°cell it is not possible for H2(g) to reduce Ni2+(aq) .

The reaction taking place at cathode is,

Ni2+(aq)+2e−→Ni(s)   E°red=−0.23 V

The reaction taking place at anode is,

H2(g)→2H+(aq)+2e−   E°ox=0.00 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 Fe2+(aq) to reduce VO2+(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 Fe2+(aq) to reduce Cr3+(aq) to Cr2+(aq) .