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Chapter 18: Problem 103

What reactions take place at the cathode and the anode when each of the following is electrolyzed? a. molten \(\mathrm{NiBr}_{2}\) b. molten \(\mathrm{AlF}_{3}\) c. molten \(\mathrm{MnI}_{2}\)

Short Answer

Expert verified
During the electrolysis of the given molten compounds: a. For molten NiBr鈧�, cathode reaction: \(Ni^{2+}(l) + 2e^- \rightarrow Ni(s)\), and anode reaction: \(2Br^-(l) \rightarrow Br_2(g) + 2e^-\). b. For molten AlF鈧�, cathode reaction: \(Al^{3+}(l) + 3e^- \rightarrow Al(s)\), and anode reaction: \(6F^-(l) \rightarrow 3F_2(g) + 6e^-\). c. For molten MnI鈧�, cathode reaction: \(Mn^{2+}(l) + 2e^- \rightarrow Mn(s)\), and anode reaction: \(2I^-(l) \rightarrow I_2(g) + 2e^-\).

Step by step solution

01

a. Reactions in electrolysis of molten NiBr鈧�

First, let's identify the cations and anions in the compound. NiBr鈧� contains the cations Ni虏鈦� and anions Br鈦�. During electrolysis: - Reduction takes place at the cathode. - Oxidation takes place at the anode. Reduction half-reaction at the cathode: \[Ni^{2+}(l) + 2e^- \rightarrow Ni(s)\] Oxidation half-reaction at the anode: \[2Br^-(l) \rightarrow Br_2(g) + 2e^-\]
02

b. Reactions in electrolysis of molten AlF鈧�

First, let's identify the cations and anions in the compound. AlF鈧� contains the cations Al鲁鈦� and anions F鈦�. Reduction half-reaction at the cathode: \[Al^{3+}(l) + 3e^- \rightarrow Al(s)\] Oxidation half-reaction at the anode: \[6F^-(l) \rightarrow 3F_2(g) + 6e^-\]
03

c. Reactions in electrolysis of molten MnI鈧�

First, let's identify the cations and anions in the compound. MnI鈧� contains the cations Mn虏鈦� and anions I鈦�. Reduction half-reaction at the cathode: \[Mn^{2+}(l) + 2e^- \rightarrow Mn(s)\] Oxidation half-reaction at the anode: \[2I^-(l) \rightarrow I_2(g) + 2e^-\] In summary, during the electrolysis of the given molten compounds, the respective metal cations (Ni虏鈦�, Al鲁鈦�, and Mn虏鈦�) get reduced at the cathode, and the respective halogen anions (Br鈦�, F鈦�, and I鈦�) get oxidized at the anode.

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Most popular questions from this chapter

What reaction will take place at the cathode and the anode when each of the following is electrolyzed? (Assume standard conditions.) a. \(1.0 \mathrm{M}\) KF solution b. \(1.0 \mathrm{M} \mathrm{CuCl}_{2}\) solution c. \(1.0 \mathrm{M} \mathrm{MgI}_{2}\) solution

Consider a cell based on the following half-reactions: $$\begin{aligned}\mathrm{Au}^{3+}+3 \mathrm{e}^{-} \longrightarrow \mathrm{Au} & \mathscr{C}^{\circ}=1.50 \mathrm{~V} \\ \mathrm{Fe}^{3+}+\mathrm{e}^{-} \longrightarrow \mathrm{Fe}^{2+} & \mathscr{C}^{\circ}=0.77 \mathrm{~V} \end{aligned}$$ a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate. b. When enough \(\mathrm{NaCl}(s)\) is added to the compartment containing gold to make the \(\left[\mathrm{Cl}^{-}\right]=0.10 M\), the cell potential is observed to be \(0.31 \mathrm{~V}\). Assume that \(\mathrm{Au}^{3+}\) is reduced and assume that the reaction in the compartment containing gold is $$\mathrm{Au}^{3+}(a q)+4 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{AuCl}_{4}^{-}(a q)$$ Calculate the value of \(K\) for this reaction at \(25^{\circ} \mathrm{C}\).

A chemist wishes to determine the concentration of \(\mathrm{CrO}_{4}^{2-}\) electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; see Exercise 115\()\) and a silver wire coated with \(\mathrm{Ag}_{2} \mathrm{Cr} \mathrm{O}_{4}\). The \(\mathscr{C}^{\circ}\) value for the following halfreaction is \(+0.446 \mathrm{~V}\) relative to the standard hydrogen electrode: $$\mathrm{Ag}_{2} \mathrm{CrO}_{4}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Ag}+\mathrm{CrO}_{4}^{2-}$$ a. Calculate \(\mathscr{E}_{\text {cell }}\) and \(\Delta G\) at \(25^{\circ} \mathrm{C}\) for the cell reaction when \(\left[\mathrm{CrO}_{4}^{2-}\right]=1.00 \mathrm{~mol} / \mathrm{L}\) b. Write the Nernst equation for the cell. Assume that the SCE concentrations are constant. c. If the coated silver wire is placed in a solution (at \(25^{\circ} \mathrm{C}\) ) in which \(\left[\mathrm{CrO}_{4}^{2-}\right]=1.00 \times 10^{-5} M\), what is the expected cell potential? d. The measured cell potential at \(25^{\circ} \mathrm{C}\) is \(0.504 \mathrm{~V}\) when the coated wire is dipped into a solution of unknown \(\left[\mathrm{Cr} \mathrm{O}_{4}{ }^{2-}\right]\). What is \(\left[\mathrm{CrO}_{4}^{2-}\right]\) for this solution? e. Using data from this problem and from Table \(18.1\), calculate the solubility product \(\left(K_{\mathrm{sp}}\right)\) for \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\).

Hydrazine is somewhat toxic. Use the half-reactions shown below to explain why household bleach (a highly alkaline solution of sodium hypochlorite) should not be mixed with household ammonia or glass cleansers that contain ammonia. \(\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-}+\mathrm{Cl}^{-} \quad \mathscr{E}^{\circ}=0.90 \mathrm{~V}\) \(\mathrm{N}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{NH}_{3}+2 \mathrm{OH}^{-} \quad \mathscr{E}^{\circ}=-0.10 \mathrm{~V}\)

Given the following two standard reduction potentials, $$\mathrm{M}^{3+}+3 \mathrm{e}^{-} \longrightarrow \mathrm{M} \quad \mathscr{E}^{\circ}=-0.10 \mathrm{~V}$$ $$\mathrm{M}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{M} \quad \mathscr{E}^{\circ}=-0.50 \mathrm{~V}$$ solve for the standard reduction potential of the half- reaction$$\mathrm{M}^{3+}+\mathrm{e}^{-} \longrightarrow \mathrm{M}^{2+}$$
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