Chemistry, 21.07.2020 18:01 darknessmidnight207

Which one of the following reactions must be carried out in an electrolytic cell rather than in an electrochemical cell? a. Zn2+ + Ca → Zn + Ca2+
b. Al3+ + 3Br– → Al + (3/2)Br2
c. 2Al + 3Fe2+ → 2Al3+ + 3Fe
d. H2 + I2(s) → 2H+ + 2I–

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Answer from: TayTae2237

b. $Al^{3+} + 3 Br^{-}$ → $Al + \frac{3}{2} Br_{2}$

Electrolytic Cell v/s Electrochemical Cell:

Electrochemical cells convert chemical energy into electrical energy or vice versa while an electrolytic cell is a type of electrochemical cell in which electrical energy is converted into chemical energy.Electrochemical cells consist of a cathode (+) and an anode(-) while Electrolytic cells consist of a positively charged anode and a negatively charged cathode.

Out of the given reactions, $Al^{3+} + 3 Br^{-}$ → $Al + \frac{3}{2} Br_{2}$ is carried out in an electrolytic cell rather than in an electrochemical cell.

As we know, In electrolytic cells, like galvanic cells, are composed of two half-cells

one is a reduction half-cell, the other is an oxidation half-cell.

In the given reaction, aluminum is being reduced while bromine gets oxidized and the value of reduction potential of aluminum is -1.66 V while that of bromine is + 1.087. Therefore, the process is non spontaneous and can only occur in an electrolytic cell.

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Answer from: ciarrap552

b. Al3+ + 3Br– → Al + (3/2)Br2

Explanation:

If we look at this reaction closely, aluminum was reduced while bromine was oxidized. The reduction potential of aluminum is -1.66 V while that of bromine is + 1.087. Recall that the more negative the redox potential of a chemical specie, the greater its tendency to function as a reducing agent donating electrons in an electrochemical reaction.

However, in this reaction, aluminium is found to accept rather than donate electrons. Therefore, the process is non spontaneous and can only occur in an electrolytic cell, hence the answer.

Answer from: Quest

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Answer from: Quest

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