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Chapter 4: Problem 51

Which element is oxidized and which is reduced in the following reactions? (a) \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) (b) \(3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow\) \(3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) (c) \(\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)\) (d) \(\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(l)\)

Short Answer

Expert verified
In the given reactions: (a) N is reduced and H is oxidized. (b) Fe is reduced and Al is oxidized. (c) Cl is reduced and I is oxidized. (d) S is oxidized and O is reduced.

Step by step solution

01

(a) Assigning Oxidation Numbers

For the reaction $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g):$ Oxidation numbers: \(N_{2}\): \(0 \longrightarrow -3\) in \(NH_{3}\), \(H_{2}\): \(0 \longrightarrow +1\) in \(NH_{3}\)
02

(a) Identifying Oxidizing and Reducing Elements

\(N_{2}\) goes from 0 to -3, meaning it is reduced (gain in electrons). \(H_{2}\) goes from 0 to +1, meaning it is oxidized (loss of electrons).
03

(b) Assigning Oxidation Numbers

For the reaction \(3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow 3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q):\) Oxidation numbers: \(Fe\) in \(\mathrm{Fe(NO_{3})_{2}}\): \(+2 \longrightarrow 0\) in \(Fe\), \(Al\): \(0 \longrightarrow +3\) in \(\mathrm{Al(NO_{3})_{3}}\)
04

(b) Identifying Oxidizing and Reducing Elements

\(Fe\) goes from +2 to 0, meaning it is reduced (gain in electrons). \(Al\) goes from 0 to +3, meaning it is oxidized (loss of electrons).
05

(c) Assigning Oxidation Numbers

For the reaction \(\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q):\) Oxidation numbers: \(Cl_{2}\): \(0 \longrightarrow -1\) in \(\mathrm{NaCl}\), \(I\) in \(\mathrm{NaI}\): \(-1 \longrightarrow 0\) in \(I_{2}\)
06

(c) Identifying Oxidizing and Reducing Elements

\(Cl_{2}\) goes from 0 to -1, meaning it is reduced (gain in electrons). \(I\) goes from -1 to 0, meaning it is oxidized (loss of electrons).
07

(d) Assigning Oxidation Numbers

For the reaction \(\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(l)\): Oxidation numbers: \(S\) in \(\mathrm{PbS}\): \(-2 \longrightarrow +6\) in \(\mathrm{PbSO_{4}}\), \(O\) in \(\mathrm{H_{2}O_{2}}\): \(-1 \longrightarrow -2\) in \(\mathrm{H_{2}O}\)
08

(d) Identifying Oxidizing and Reducing Elements

\(S\) goes from -2 to +6, meaning it is oxidized (loss of electrons). \(O\) goes from -1 to -2, meaning it is reduced (gain in electrons).

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Most popular questions from this chapter

Using the activity series(Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Iron metal is added to a solution of copper(II) nitrate; (b) zinc metal is added to a solution of magnesium sulfate; (c) hydrobromic acid is added to tin metal; (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride; (e) aluminum metal is added to a solution of cobalt(II) sulfate.

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) \(\mathrm{NiCl}_{2}\), (b) \(\mathrm{Ag}_{2} \mathrm{~S}\), (c) \(\mathrm{Cs}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{SrCO}_{3}\) (e) \(\mathrm{PbSO}_{4}\).

As \(\mathrm{K}_{2} \mathrm{O}\) dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. Write the molecular and net ionic equations for this reaction. Based on the definitions of acid and base, what ion is the base in this reaction? What is the acid? What is the spectator ion in the reaction?

Define oxidation and reduction in terms of (a) electron transfer and (b) oxidation numbers.

The commercial production of nitric acid involves the following chemical reactions: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{NO}_{2}(g) \\ 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow 2 \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g) \end{aligned} $$ (a) Which of these reactions are redox reactions? (b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction.
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