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Chapter 20: Problem 16

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) An oxidizing agent is needed to convert \(\mathrm{CO}\) into \(\mathrm{CO}_{2}\).

Short Answer

Expert verified
(a) False: Reduction refers to the process of gaining electrons, not losing them. (b) True: A reducing agent causes another substance to be reduced and itself gets oxidized in the process. (c) True: An oxidizing agent is needed to provide the additional oxygen atom needed to convert CO into CO2.

Step by step solution

01

Statement A: If something is reduced, it is formally losing electrons.

This statement is false. Reduction actually refers to the process of gaining electrons, not losing them. It is when a substance reduces its oxidation state by gaining electrons.
02

Statement B: A reducing agent gets oxidized as it reacts.

This statement is true. A reducing agent is a substance that causes another substance to be reduced and itself gets oxidized in the process. By losing electrons, the reducing agent makes it possible for the other substance to gain those electrons and be reduced.
03

Statement C: An oxidizing agent is needed to convert CO into CO2.

This statement is true. When carbon monoxide (CO) is converted into carbon dioxide (CO2), oxidation occurs. This means that CO must be gaining oxygen, in this case, by reacting with an oxidizing agent. An oxidizing agent is needed to provide the additional oxygen atom needed to convert CO into CO2.

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Most popular questions from this chapter

(a) A voltaic cell is constructed with all reactants and products in their standard states. Will the concentration of the reactants increase, decrease, or remain the same as the cell operates? (b) What happens to the emf of a cell if the concentrations of the products are increased?

Given the following reduction half-reactions: $$ \begin{gathered} \mathrm{Fe}^{3+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Fe}^{2+}(a q) \quad E_{\text {red }}^{\infty}=+0.77 \mathrm{~V} \\ \mathrm{~S}_{2} \mathrm{O}_{6}^{2-}(a q)+4 \mathrm{H}^{+}(a q)+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{H}_{2} \mathrm{SO}_{3}(a q) \quad E_{\mathrm{ret}}^{\circ}=+0.60 \mathrm{~V} \\ \mathrm{~N}_{2} \mathrm{O}(g)+2 \mathrm{H}^{+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(I) \quad \mathrm{E}_{\mathrm{red}}^{\circ}=-1.77 \mathrm{~V} \\ \mathrm{VO}_{2}^{+}(a q)+2 \mathrm{H}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{VO}^{2+}+\mathrm{H}_{2} \mathrm{O}(l) \quad E_{\mathrm{red}}^{0}=+1.00 \mathrm{~V} \end{gathered} $$ (a) Write balanced chemical equations for the oxidation of \(\mathrm{Fe}^{2+}(a q)\) by \(\mathrm{S}_{2} \mathrm{O}_{6}^{2-}(a q)\), by \(\mathrm{N}_{2} \mathrm{O}(a q)\), and by \(\mathrm{VO}_{2}^{+}\)(aq). (b) Calculate \(\Delta G^{\circ}\) for each reaction at \(298 \mathrm{~K}\). (c) Calculate the equilibrium constant \(K\) for each reaction at \(298 \mathrm{~K}\).

An iron object is plated with a coating of cobalt to protect against corrosion. Does the cobalt protect iron by cathodic protection? Explain.

At \(900^{\circ} \mathrm{C}\) titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction. (b) What is being oxidized, and what is being reduced? (c) Which substance is the reductant, and which is the exidant?

The standard reduction potential for the reduction of \(\mathrm{RuO}_{4}^{-}(a q)\) to \(\mathrm{RuO}_{4}^{2-}(a q)\) is \(+0.59 \mathrm{~V}\). By using Appendix E, which of the following substances can oxidize \(\mathrm{RuO}_{4}^{2-}(a q)\) to \(\mathrm{RuO}_{4}^{-}(a q)\) under standard conditions: \(\mathrm{Br}_{2}(l), \mathrm{BrO}_{3}^{-}(a q)\). \(\mathrm{Mn}^{2+}(a q), \mathrm{O}_{2}(g), \mathrm{Sn}^{2+}(a q) ?\)
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