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Chapter 20: Problem 13

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.

Short Answer

Expert verified
(a) True (b) False (c) True

Step by step solution

01

Statement (a): Oxidation and Electron Loss

To determine if this statement is true or false, we need to recall the meaning of oxidation in a redox reaction. Oxidation is the process of losing electrons, while reduction is the process of gaining electrons. So, if something is oxidized, it is indeed formally losing electrons. Thus, statement (a) is true.
02

Statement (b): Identifying the Reducing and Oxidizing Agents

Given the redox reaction: \[\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q) \rightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Co}^{3+}(a q)\] We need to determine if \(\mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent. The reducing agent is the species that gets oxidized (loses electrons), while the oxidizing agent is the species that gets reduced (gains electrons). In this reaction, \(\mathrm{Fe}^{3+}\) is reduced to \(\mathrm{Fe}^{2+}\), and \(\mathrm{Co}^{2+}\) is oxidized to \(\mathrm{Co}^{3+}\). So, \(\mathrm{Fe}^{3+}(a q)\) is the oxidizing agent, and \(\mathrm{Co}^{2+}(a q)\) is the reducing agent. Therefore, statement (b) is false.
03

Statement (c): Redox Reactions and Changes in Oxidation State

This statement says that 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. Redox reactions are characterized by changes in oxidation states between reactants and products, as one species loses electrons while another species gains electrons. Therefore, if there are no changes in the oxidation states, it means that there is no electron transfer and the reaction is not a redox reaction. Thus, statement (c) is true.

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Most popular questions from this chapter

Using data from Appendix \(\mathrm{E}\), calculate the equilibrium constant for the disproportionation of the copper(I) ion at room temperature: \(2 \mathrm{Cu}^{+}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{Cu}(s)\)

During a period of discharge of a lead-acid battery, \(402 \mathrm{~g}\) of \(\mathrm{Pb}\) from the anode is converted into \(\mathrm{PbSO}_{4}(s) .\) What mass of \(\mathrm{PbO}_{2}(s)\) is reduced at the cathode during this same period?

Is each of the following substances likely to serve as an oxidant or a reductant: (a) \(\mathrm{Ce}^{3+}(a q)\), (b) \(\mathrm{Ca}(\mathrm{s})\), (c) \(\mathrm{ClO}_{3}^{-}(a q)\), (d) \(\mathrm{N}_{2} \mathrm{O}_{5}(g)\) ?

This oxidation-reduction reaction in acidic solution is spontaneous: \(5 \mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q)-\rightarrow\) \(5 \mathrm{Fe}^{3+}(a q)+\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)\) A solution containing \(\mathrm{KMnO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is poured into one beaker, and a solution of \(\mathrm{FeSO}_{4}\) is poured into another. A salt bridge is used to join the beakers. A platinum foil is placed in each solution, and a wire that passes through a voltmeter connects the two solutions. (a) Sketch the cell, indicating the anode and the cathode, the direction of electron movement through the external circuit, and the direction of ion migrations through the solutions. (b) Sketch the process that occurs at the atomic level at the surface of the anode. (c) Calculate the emf of the cell under standard conditions. (d) Calculate the emf of the cell at \(298 \mathrm{~K}\) when the concentrations are the following: \(\mathrm{pH}=0.0, \quad\left[\mathrm{Fe}^{2+}\right]=0.10 \mathrm{M}, \quad\left[\mathrm{MnO}_{4}^{-}\right]=1.50 \mathrm{M}\) \(\left[\mathrm{Fe}^{3+}\right]=2.5 \times 10^{-4} \mathrm{M},\left[\mathrm{Mn}^{2+}\right]=0.001 \mathrm{M}\)

The following quotation is taken from an article dealing with corrosion of electronic materials: "Sulfur dioxide, its acidic oxidation products, and moisture are well established as the principal causes of outdoor corrosion of many metals." Using \(\mathrm{Ni}\) as an example, explain why the factors cited affect the rate of corrosion. Write chemical equations to illustrate your points. (Note: \(\mathrm{NiO}(s)\) is soluble in acidic solution.)
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