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Mazyrski [523]
3 years ago
5

A galvanic cell with E o cell = 0.30 V can be constructed using an iron electrode in a 1.0 M Fe(NO3)2 solution, and either a tin

electrode in a 1.0 M Sn(NO3)2 solution, or a chromium electrode in a 1.0 M Cr(NO3)3 solution even though Sn2+/Sn and Cr3+/Cr have different reduction potentials. Give the overall balanced reaction for Fe-Sn cell. Do not include the states of matter.
Chemistry
1 answer:
Andreyy893 years ago
3 0

<u>Answer:</u> The half reactions are written below.

<u>Explanation:</u>

Oxidation reaction is defined as the reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

X\rightarrow X^{n+}+ne^-

Reduction reaction is defined as the reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

X^{n+}+ne^-\rightarrow X

We are given a chemical cell which is Fe-Sn cell. The half reaction follows:

<u>Oxidation half reaction:</u>  Fe\rightarrow Fe^{2+}+2e^-;E^o_{Fe^{2+}/Fe}=-0.44V

<u>Reduction half reaction:</u>  Sn^{2+}+2e^-\rightarrow Sn;E^o_{Sn^{2+}/Sn}=-0.14V

The substance having highest positive E^o potential will always get reduced and will undergo reduction reaction. Here, zinc will always undergo reduction reaction will get reduced.

<u>Total cell reaction:</u> Fe+Sn^{2+}\rightarrow Fe^{2+}+Sn

Hence, the half reactions are written above.

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