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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

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate \(\Delta G^{\circ}\) at \(298 \mathrm{~K}\), and calculate the equilibrium constant \(K\) at \(298 \mathrm{~K}\). (a) Aqueous iodide ion is oxidized to \(\mathrm{I}_{2}(s)\) by \(\mathrm{Hg}_{2}{ }^{2+}(a q)\). (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion. (c) In basic solution, \(\mathrm{Cr}(\mathrm{OH})_{3}(s)\) is oxidized to \(\mathrm{CrO}_{4}^{2-}(a q)\) by \(\mathrm{ClO}^{-}(a q)\)

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