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Chapter 20: Problem 14

Indicate whether each of the following statements is true or false: (a) If something is reduced, it is formally losing electrons. (b) A reducing agent gets oxidized as it reacts. (c) Oxidizing agents can convert \(\mathrm{CO}\) into \(\mathrm{CO}_{2}\).

Short Answer

Expert verified
(a) False: If something is reduced, it is formally gaining electrons. (b) True: A reducing agent gets oxidized as it reacts. (c) True: Oxidizing agents can convert \(\mathrm{CO}\) into \(\mathrm{CO}_{2}\).

Step by step solution

01

Statement (a) Analysis

The first statement says, "If something is reduced, it is formally losing electrons." When a species is reduced, it means that its oxidation state is decreasing, which means that it is gaining electrons rather than losing them. So the correct statement would be: "If something is reduced, it is formally gaining electrons."
02

Statement (a) Conclusion

Having analyzed the given statement for the concept of a reduction, we can conclude that: (a) the statement is false.
03

Statement (b) Analysis

The second statement says, "A reducing agent gets oxidized as it reacts." A reducing agent is a substance that causes another species to become reduced by providing electrons. In this process, the reducing agent itself gets oxidized, which means it loses electrons and its oxidation state increases.
04

Statement (b) Conclusion

By understanding the role of a reducing agent in a reaction and that it becomes oxidized, we can now conclude that: (b) the statement is true.
05

Statement (c) Analysis

The third statement says, "Oxidizing agents can convert \(\mathrm{CO}\) into \(\mathrm{CO}_{2}\)." An oxidizing agent is a substance that causes another species to become oxidized by accepting electrons. In the process of converting \(\mathrm{CO}\) to \(\mathrm{CO}_{2}\), the carbon in the molecule is being oxidized from an oxidation state of +2 to +4 while gaining an oxygen atom. This means that the presence of an oxidizing agent enables this conversion to take place.
06

Statement (c) Conclusion

By understanding the role of an oxidizing agent in the conversion of \(\mathrm{CO}\) to \(\mathrm{CO}_{2}\) and the oxidation process involved, we can now conclude that: (c) the statement is true.

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Most popular questions from this chapter

(a) \(\mathrm{A} \mathrm{Cr}^{3+}(a q)\) solution is electrolyzed, using a current of \(7.60 \mathrm{~A}\). What mass of \(\mathrm{Cr}(s)\) is plated out after \(2.00\) days? (b) What amperage is required to plate out \(0.250 \mathrm{~mol} \mathrm{Cr}\) from a \(\mathrm{Cr}^{3+}\) solution in a period of \(8.00 \mathrm{~h}\) ?

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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 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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This oxidation-reduction reaction in acidic solution is spontaneous: $$ \begin{array}{r} 5 \mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q)-\rightarrow \\ 5 \mathrm{Fe}^{3+}(a q)+\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) \end{array} $$ 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: \(\mathrm{pH}=0.0, \quad\left[\mathrm{Fe}^{2+}\right]=0.10 \mathrm{M}, \quad\left[\mathrm{MnO}_{4}^{-}\right]=1.50 \mathrm{M}\) \(\left[\mathrm{Fe}^{3+}\right]=2.5 \times 10^{-4} \mathrm{M},\left[\mathrm{Mn}^{2+}\right]=0.001 \mathrm{M}\)
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