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Chapter 18: Problem 9

You are told that metal \(\mathrm{A}\) is a better reducing agent than metal B. What, if anything, can be said about \(\mathrm{A}^{+}\) and \(\mathrm{B}^{+}\) ? Explain.

Short Answer

Expert verified
In conclusion, since metal A is a better reducing agent than metal B, this implies that A has a more negative standard reduction potential than B. Therefore, A鈦� will have a less positive (or more negative) standard reduction potential than B鈦�. Consequently, B鈦� is a stronger oxidizing agent than A鈦�, meaning it will tend to gain electrons more readily than A鈦�.

Step by step solution

01

Understanding reducing agents

A reducing agent is a substance that donates electrons in a redox reaction, thereby causing the other substance to be reduced. In our case, metal A and metal B act as reducing agents.
02

Relating reducing agents to reduction potentials

The standard reduction potential is a measure of the tendency of a chemical species to be reduced. A more negative standard reduction potential indicates that a species is more likely to donate electrons (thus, it is a better reducing agent). Conversely, a more positive standard reduction potential indicates that a species is less likely to donate electrons (thus, it is a less effective reducing agent).
03

Comparing the reduction potentials of A鈦� and B鈦�

Since metal A is a better reducing agent than metal B, we can deduce that A has a more negative standard reduction potential than B. This means that A is more likely to donate electrons than B. Now, we need to analyze the relationship between the standard reduction potentials of the metal ions A鈦� and B鈦�.
04

Relationship between metal ions and their standard reduction potentials

When a metal is oxidized to its ionic form (A 鈫� A鈦� + e鈦� or B 鈫� B鈦� + e鈦�), its standard reduction potential becomes more positive. Therefore, in this case, the standard reduction potentials of A鈦� and B鈦� are the reverse of their metallic forms (A and B).
05

Comparing A鈦� and B鈦� based on their reducing nature

Since metal A is a better reducing agent and has a more negative standard reduction potential than metal B, it means that A鈦� will have a less positive (or more negative) standard reduction potential than B鈦�. Therefore, we can conclude that B鈦� is a stronger oxidizing agent compared to A鈦�. A stronger oxidizing agent will have a greater tendency to be reduced, i.e., it will tend to gain electrons more readily than a weaker oxidizing agent. In conclusion, since metal A is a better reducing agent than metal B, B鈦� is a stronger oxidizing agent than A鈦�.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Standard Reduction Potential
The standard reduction potential is a pivotal concept in understanding redox reactions and the behavior of reducing and oxidizing agents. It serves as a measure of the willingness of a substance to gain electrons, thereby undergoing reduction. The potential is usually measured in volts under standard conditions, which include a concentration of 1 M, a pressure of 1 atm, and a temperature of 25掳C.

**Understanding the Values:**
  • A more negative standard reduction potential indicates a greater tendency for the species to act as a reducing agent. This means it is more inclined to lose electrons.
  • A more positive standard reduction potential suggests that the species has a higher tendency to gain electrons, making it a stronger oxidizing agent.
In the original exercise, since metal A is described as a better reducing agent than metal B, A must have a more negative standard reduction potential than B. In terms of their ionic forms, the situation reverses, leading A鈦� to have a more positive potential than B鈦�, thereby indicating A鈦� as a weaker oxidizing agent compared to B鈦�.
Oxidizing Agents
Oxidizing agents play a crucial role in redox reactions, where they gain electrons and are reduced themselves. By accepting electrons from another substance, they facilitate the oxidation of that substance. Because of this role, they are essential to countless chemical processes.

**Characteristics of Strong Oxidizing Agents:**
  • They have a high affinity for electrons.
  • Typically, they possess a positive standard reduction potential.
  • Their ability to oxidize other substances makes them very reactive.
According to the solution given for the exercise, B鈦� is a stronger oxidizing agent compared to A鈦�. This is because B鈦� has a greater tendency to gain electrons, as implied by its potentially more positive standard reduction potential. It's this ability that makes B鈦� efficient at oxidizing substances, while A鈦� does not quite match up.
Redox Reactions
Redox reactions, short for reduction-oxidation reactions, represent a fundamental type of chemical reaction involving the transfer of electrons between two substances. In these reactions, one reactant undergoes oxidation (loses electrons), while the other undergoes reduction (gains electrons).

**Components of Redox Reactions:**
  • **Reducing Agent:** Donates electrons and becomes oxidized. In the context of the exercise, metal A is the reducing agent since it donates electrons more readily compared to metal B.
  • **Oxidizing Agent:** Accepts electrons and becomes reduced. Here, B鈦� acts as the oxidizing agent because it gains electrons more easily than A鈦�.
Balancing redox reactions is crucial to ensure that the number of electrons lost in oxidation matches the number gained in reduction. Understanding the interplay between reducing and oxidizing agents via their standard reduction potentials can greatly clarify the outcomes and paths of these reactions.

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Most popular questions from this chapter

An electrochemical cell is set up using the following unbalanced reaction: $$\mathrm{M}^{a+}(a q)+\mathrm{N}(s) \longrightarrow \mathrm{N}^{2+}(a q)+\mathrm{M}(s)$$ The standard reduction potentials are: $$\mathrm{M}^{a+}+a \mathrm{e}^{-} \longrightarrow \mathrm{M} \quad \mathscr{E}^{\circ}=0.400 \mathrm{V}$$ $$\mathrm{N}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{N} \quad \mathscr{E}^{\circ}=0.240 \mathrm{V}$$ The cell contains 0.10\(M \mathrm{N}^{2+}\) and produces a voltage of 0.180 \(\mathrm{V}\) . If the concentration of \(\mathrm{M}^{a+}\) is such that the value of the reaction quotient \(Q\) is \(9.32 \times 10^{-3},\) calculate \(\left[\mathrm{M}^{a+}\right] .\) Calculate \(w_{\text { max }}\) for this electrochemical cell.

Which of the following statements concerning corrosion is(are) true? For the false statements, correct them. a. Corrosion is an example of an electrolytic process. b. Corrosion of steel involves the reduction of iron coupled with the oxidation of oxygen. c. Steel rusts more easily in the dry (arid) Southwest states than in the humid Midwest states. d. Salting roads in the winter has the added benefit of hindering the corrosion of steel. e. The key to cathodic protection is to connect via a wire a metal more easily oxidized than iron to the steel surface to be protected.

Under standard conditions, what reaction occurs, if any, when each of the following operations is performed? a. Crystals of \(\mathrm{I}_{2}\) are added to a solution of \(\mathrm{NaCl}\) . b. \(\mathrm{Cl}_{2}\) gas is bubbled into a solution of \(\mathrm{Nal}\). c. A silver wire is placed in a solution of \(\mathrm{CuCl}_{2}\) d. An acidic solution of \(\mathrm{FeSO}_{4}\) is exposed to air. For the reactions that occur, write a balanced equation and calculate \(\mathscr{E}^{\circ}, \Delta G^{\circ},\) and \(K\) at \(25^{\circ} \mathrm{C}\)

Consider the following galvanic cell at \(25^{\circ} \mathrm{C} :\) $$\text { Pt }\left|\mathrm{Cr}^{2+}(0.30 M), \mathrm{Cr}^{3+}(2.0 M)\right|\left|\mathrm{Co}^{2+}(0.20 M)\right| \mathrm{Co}$$ The overall reaction and equilibrium constant value are $$2 \mathrm{Cr}^{2+}(a q)+\mathrm{Co}^{2+}(a q) \rightleftharpoons_{2 \mathrm{Cr}^{3+}}(a q)+\mathrm{Co}(s) \quad K=2.79 \times 10^{7}$$ Calculate the cell potential, \(\mathscr{E},\) for this galvanic cell and \(\Delta G\) for the cell reaction at these conditions.

The following standard reduction potentials have been determined for the aqueous chemistry of indium: $$\operatorname{In}^{3+}(a q)+2 \mathrm{e}^{-} \longrightarrow \operatorname{In}^{+}(a q) \quad \mathscr{E}^{\circ}=-0.444 \mathrm{V}$$ $$\operatorname{In}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \operatorname{In}(s) \qquad \quad \mathscr{E}^{\circ}=-0.126 \mathrm{V}$$ a. What is the equilibrium constant for the disproportionation reaction, where a species is both oxidized and reduced, shown below? $$3 \ln ^{+}(a q) \longrightarrow 2 \operatorname{In}(s)+\operatorname{In}^{3+}(a q)$$ b. What is \(\Delta G_{i}^{\circ}\) for \(\operatorname{In}^{+}(a q)\) if \(\Delta G_{f}^{\circ}=-97.9 \mathrm{kJ} / \mathrm{mol}\) for \(\operatorname{In}^{3+}(a q) ?\)
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