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consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Al3+(aq) + 3e− → Al(s) −...

consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts)

Al3+(aq) + 3e− → Al(s) − 1.66

Fe2+(aq) + 2e− → Fe(s)    − 0.44

Sn2+(aq) + 2e− → Sn(s) − 0.14

The Al/Al3+ half-reaction can be paired with the other two to produce voltaic cells because ________

A) Al is a more powerful oxidizing agent

B) Fe and Sn are readily oxidized Al is a more powerful reducing agent

C) Al3+ is a more powerful oxidizing agent

D) Al3+ is a more powerful reducing agent

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Answer #1

This can be explained by taking into account the Gibbs free energy produced after the combination of the half-cells. To make the half cell combination feasible, the value of electrode potential should be positive so that the value of Gibbs free energy is negative according to the formula:-

for Al/Al3+= +1.66V while

for Fe2+/Fe = -0.44V and for Sn2+/Sn = -0.14V

On combining the Al/Al3+ and Fe2+/Fe, = 1.22V while on combining Al/Al3+ and Sn2+/Sn, = 1.52V

Thus, it shows that Al is a powerful reducing agent!

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