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Chapter 20: Problem 11

(a) What is meant by the term oxidation? (b) On which side of an oxidation half-reaction do the electrons appear? (c) What is meant by the term oxidant? (d) What is meant by the term oxidizing agent?

Short Answer

Expert verified
(a) Oxidation refers to the process in which a species loses one or more electrons, leading to an increase in its oxidation state. (b) In an oxidation half-reaction, electrons appear on the right-hand side. For example: \(Zn\rightarrow Zn^{2+}+2e^-\). (c) An oxidant is a substance that can accept one or more electrons from another species in a redox reaction, promoting oxidation and getting reduced. (d) An oxidizing agent is a substance that causes the oxidation of another species in a redox reaction by accepting electrons. The terms oxidant and oxidizing agent are often used interchangeably.

Step by step solution

01

(a) Definition of Oxidation)

Oxidation is the process in which a species (atom, ion, or molecule) loses one or more electrons. This leads to an increase in the oxidation state of the species. The species that undergoes oxidation is called the reducing agent, as it facilitates the reduction process for another species.
02

(b) Side of Electrons in an Oxidation Half-reaction)

In an oxidation half-reaction, the electrons appear on the right-hand side of the reaction. This indicates that the species (on the left-hand side) is losing electrons during the process. Example of an oxidation half-reaction: \(Zn\rightarrow Zn^{2+}+2e^-\)
03

(c) Definition of Oxidant)

The term oxidant refers to a substance (like an atom, ion, or molecule) that has the ability to accept one or more electrons from another species in a redox (reduction-oxidation) reaction. In other words, the oxidant promotes the oxidation process and gets reduced during the reaction.
04

(d) Definition of Oxidizing Agent)

An oxidizing agent is a substance that causes the oxidation of another species in a redox reaction by accepting electrons from the other species. The terms oxidant and oxidizing agent are often used interchangeably, as both refer to a substance that promotes the oxidation process and undergoes reduction during the reaction.

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Most popular questions from this chapter

A voltaic cell is constructed that is based on the following reaction: $$ \mathrm{Sn}^{2+}(a q)+\mathrm{Pb}(s)--\rightarrow \mathrm{Sn}(s)+\mathrm{Pb}^{2+}(a q) $$ (a) If the concentration of \(\mathrm{Sn}^{2+}\) in the cathode compartment is \(1.00 M\) and the cell generates an emf of \(+0.22 \mathrm{~V}\), what is the concentration of \(\mathrm{Pb}^{2+}\) in the anode compartment? (b) If the anode compartment contains \(\left[\mathrm{SO}_{4}^{2-}\right]=1.00 M\) in equilibrium with \(\mathrm{PbSO}_{4}(s)\), what is the \(K_{s p}\) of \(\mathrm{PbSO}_{4} ?\)

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons. (b) For the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q)-\cdots\) \(\mathrm{Fe}^{2+}(a q)+\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent. (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

A voltaic cell utilizes the following reaction: $$ \mathrm{Al}(s)+3 \mathrm{Ag}^{+}(a q)-\infty \mathrm{Al}^{3+}(a q)+3 \mathrm{Ag}(s) $$ What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. (b) The size of the aluminum electrode is increased. (c) A solution of \(\mathrm{AgNO}_{3}\) is added to the cathode compartment, increasing the quantity of \(\mathrm{Ag}^{+}\) but not changing its concentration. (d) \(\mathrm{HCl}\) is added to the \(\mathrm{AgNO}_{3}\) solution, precipitating some of the \(\mathrm{Ag}^{+}\) as \(\mathrm{AgCl}\)

Some years ago a unique proposal was made to raise the Titanic. The plan involved placing pontoons within the ship using a surface-controlled submarine-type vessel. The pontoons would contain cathodes and would be filled with hydrogen gas formed by the electrolysis of water. It has been estimated that it would require about \(7 \times 10^{8} \mathrm{~mol}\) of \(\mathrm{H}_{2}\) to provide the buoyancy to lift the ship (J. Chem. Educ., Vol. \(50,1973,61\) ). (a) How many coulombs of electrical charge would be required? (b) What is the minimum voltage required to generate \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2}\) if the pressure on the gases at the depth of the wreckage ( \(2 \mathrm{mi}\) ) is \(300 \mathrm{~atm} ?\) (c) What is the minimum electrical energy required to raise the Titanic by electrolysis? (d) What is the minimum cost of the electrical energy required to generate the necessary \(\mathrm{H}_{2}\) if the electricity costs 85 cents per kilowatt-hour to generate at the site?

The \(K_{\infty}\) value for \(\mathrm{PbS}(s)\) is \(8.0 \times 10^{-28} .\) By using this value together with an electrode potential from Appendix \(\mathrm{E}\), determine the value of the standard reduction potential for the reaction $$ \mathrm{PbS}(s)+2 \mathrm{e}^{-}-\cdots \mathrm{Pb}(s)+\mathrm{S}^{2-}(a q) $$
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