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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

Calcium is obtained industrially by electrolysis of moltenCaCl2and is used in aluminium alloys. How many coulombs are needed to produce 10.0 gof Cametal? If a cell runs at 15 A, how many minutes will it take to produce 10.0 gof Ca(s)?

You are given the following three half-reactions:

(1) Fe3 +(aq) +e-⇌Fe2 +(aq)(2) Fe2 +(aq) + 2e-⇌Fe(s)(3) Fe3 +(aq) + 3e-⇌Fe(s)

(a). Use Eohalf - cellvalues for ( 1 ) and ( 2 ) to find Eohalf - cell for ( 3 ).

(b) Calculate∆G0 for ( 1) and ( 2) from their Eohalf - cellvalues.

(c) Calculate∆G0 for (3) from (1) and ( 2 ).

(d) Calculate Eohalf - cellfor ( 3) from its ∆G0.

(e) What is the relationship between the Eohalf - cellvalues for (1) and (2) and theEohalf - cellvalue for (3 )?

You are investigating a particular chemical reaction. State all the types of data available in standard tables that enable you to calculate the equilibrium constant for the reaction at298 K.

A chemist designs an ion-specific probe for measuring [ Ag+] in an NaCl solution saturated with AgCl. One half-cell has an Ag-wire electrode immersed in the unknown AgCl saturated NaCl solution. It is connected through a salt bridge to the other half-cell, which has a calomel reference electrode [a platinum wire immersed in a paste of mercury and calomel ( Hg2Cl2)] in a saturated KCl solution. The measuredEcell is 0.060V. (a) Given the following standard half-reactions, calculate [Ag+ ].

Calomel:Hg2Cl2(s) + 2e-→2Hg + 2Cl-Eo= 0.24 V

Silver:Ag+(aq) +e-→Ag(s)Eo= 0.80 V

(Hint: Assume [ Cl-] is so high that it is essentially constant.) (b) A mining engineer wants an ore sample analyzed with theAg+ - selective probe. After pre-treating the ore sample, the chemist measures the cell voltage as V. What is [ Ag+]?

A voltaic cell using Cu/ Cu2 +and Sn/Sn2 +half-cells is set up at standard conditions, and each compartment has a volume of345mL. The cell delivers 0.17A for48.0 h. (a) How many grams of Cu(s) are deposited? (b) What is the [ Cu2 +] remaining?
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