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Chapter 21: Q21.96P (page 922)

Identify those elements that can be prepared by electrolysis of their aqueous salts: fluorine, manganese, iron, cadmium.

Short Answer

Expert verified

Cadmium, Manganese, and Iron are the elements that can be prepared by electrolysis of their aqueous salts.

Step by step solution

01

Definition of Electrolysis

The process of decomposing ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid form is known as electrolysis. At the cathode, cations are reduced, whereas anions are oxidized.

02

Determining the elements that prepared by electrolysis

Not all ions in aqueous solutions, including these, may be transformed to their free element form via electrolysis due to over voltage:

- Metal cations from Group 1A.

- Metal cations from Group 2A and Aluminum cations from Group 3A.

- While the fluoride ion cannot be oxidized, the other halides can.

Only fluorine can be created from the list of fluorine, manganese, iron, and cadmium, because it is the only halide that is reduced by overvoltage.

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Most popular questions from this chapter

Commercial electrolytic cells for producing aluminium operate at5.0 Vand100,000 A.

(a) How long does it take to produce exactly 1metric ton (1000 kg) of aluminium?

(b) How much electrical power (in kilowatt-hours,kW路h) is used [1 W = 1 J/s;1 kW路h = 3.6脳103KJ]?

(c) If electricity costs0.90perkW路hand cell efficiency is90%, what is the cost of electricity to produce exactly1 lbof aluminium?

Define oxidation and reduction in terms of electron transfer and change in oxidation number.

Comparing the standard electrode potentials (Eo)of the Group 1A(1)metalsLi, Na, and Kwith the negative of their first ionization energies reveals a discrepancy:

Ionization process reversed:M+(g) +e-鈬�M(g) ( - IE)

Electrode reaction:M+(aq) +e-鈬�M(s) (Eo)

Note that the electrode potentials do not decrease smoothly down the group, as the ionization energies do. You might expect that if it is more difficult to remove an electron from an atom to form a gaseous ion (largerIE), then it would be less difficult to add an electron to an aqueous ion to form an atom (smallerEo), yetLi+(aq)is more difficult to reduce thanNa+(aq). Applying Hess鈥檚 law, use an approach similar to that for a Born-Haber cycle to break down the process occurring at the electrode into three steps and label the energy involved in each step. How can you account for the discrepancy?

Commercial electrolysis is performed on both moltenand aqueoussolutions. Identify the anode product, cathode product, species reduced, and species oxidized for the anode.

(a) molten electrolysis and

(b) aqueous electrolysis.

Balance each skeleton reaction, calculateE掳cell, and state whether the reaction is spontaneous:

(a)role="math" localid="1663418747793" Cl2(g) + Fe2 +(aq) Cl-(aq) + Fe3 +(aq)

(b)role="math" localid="1663418761168" Mn2 +(aq) + Co3 +(aq) MnO2(s) + Co2 +(aq)[acidic]

(c) AgCl(s) + NO(g) Ag(s) + Cl-(aq) + NO3-(aq)[acidic]
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