0.24 Bis2a 06.appendix a review of red/ox reactions (Page 8/31)

Ucd bis2a intro to biology v1. Page 8 / 31

Calcium cyclamate Ca(C ₆ H ₁₁ NHSO ₃ ) ₂ is an artificial sweetener used in many countries around the world but is banned in the United States. It can be purified industrially by converting it to the barium salt through reaction of the acid C ₆ H ₁₁ NHSO ₃ H with barium carbonate, treatment with sulfuric acid (barium sulfate is very insoluble), and then neutralization with calcium hydroxide. Write the balanced equations for these reactions.

$2 C_{6} H_{11} {NHSO}_{3} H(a q) + {BaCO}_{3} (a q) ⟶ {(C_{6} H_{11} {NHSO}_{3})}_{2} Ba(s) + H_{2} {CO}_{3} (a q)$
${(C_{6} H_{11} {NHSO}_{3})}_{2} Ba(s) + H_{2} {SO}_{4} (a q) ⟶ {BaSO}_{4} (s) + 2 C_{6} H_{11} {NHSO}_{3} H(a q)$
$2 C_{6} H_{11} {NHSO}_{3} H(a q) + Ca {(OH)}_{2} (a q) ⟶ Ca {(C_{6} H_{11} {NHSO}_{3})}_{2} (s) + 2 H_{2} O(l)$

Complete and balance each of the following half-reactions (steps 2–5 in half-reaction method):

(a) ${Sn}^{4+} (a q) ⟶ {Sn}^{2+} (a q)$

(b) ${[Ag {({NH}_{3})}_{2}]}^{+} (a q) ⟶ Ag (s) + {NH}_{3} (a q)$

(d) $H_{2} O(l) ⟶ O_{2} (in acidic solution)$

(e) ${IO}_{3}^{-} (a q) ⟶ I_{2} (s)$

(f) ${SO}_{3}^{2−} (a q) ⟶ {SO}_{4}^{2−} (a q) (in acidic solution)$

(g) ${MnO}_{4}^{-} (a q) ⟶ {Mn}^{2+} (a q) (in acidic solution)$

(h) ${Cl}^{-} (a q) ⟶ {ClO}_{3}^{-} (a q) (in basic solution)$

(a) $\begin{array}{l} S n^{4+} (a q) ⟶ {Sn}^{2+} (a q) \\ {Sn}^{4+} (a q) + {Se}^{-} ⟶ {Sn}^{2+} (a q) \end{array},$ (b) $\begin{array}{l} {[Ag {({NH}_{3})}_{2}]}^{+} (a q) ⟶ Ag(s) + 2 {NH}_{3} (a q) \\ {[Ag {({NH}_{3})}_{2}]}^{+} (a q) + e^{-} ⟶ Ag(s) + 2 {NH}_{3} (a q) \end{array};$ (c) $\begin{array}{l} {Hg}_{2} {Cl}_{2} (s) ⟶ Hg(l) + {Cl}^{−} (a q) \\ {Hg}_{2} {Cl}_{2} (s) ⟶ 2 Hg(l) + 2 {Cl}^{−} (a q) \\ {Hg}_{2} {Cl}_{2} (s) + 2 e^{-} ⟶ 2 Hg(l) + 2 {Cl}^{−} (a q) \end{array};$ (d) $\begin{array}{l} 2 H_{2} O(l) ⟶ O_{2} (g) \\ 2 H_{2} O(l) ⟶ O_{2} (g) + 4 H^{+} (a q) \\ 2 H_{2} O(l) ⟶ O_{2} (g) + 4 H^{+} (a q) + 4 e^{-} \end{array};$ (e) $\begin{array}{l} {IO}_{3}^{-} (a q) ⟶ I_{2} (s) \\ 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) \\ 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) + 6 H_{2} O(l) \\ 12 H^{+} (a q) + 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) + 6 H_{2} O(l) \\ 12 H^{+} (a q) + 12 O H^{-} (aq) + 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) + 6 H_{2} O(l) + 12 O H^{-} (aq) \\ 12 H_{2} O(l) + 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) + 6 H_{2} O(l) + 12 {OH}^{−} (a q) \\ 6 H_{2} O(l) + 2 {IO}_{3}^{-} (a q) ⟶ I_{2} (s) + 12 {OH}^{−} (a q) \\ 6 H_{2} O(l) + 2 {IO}_{3}^{-} (a q) 10 e^{-} ⟶ I_{2} (s) + 12 {OH}^{−} (a q) \end{array};$ (f) $\begin{array}{l} {SO}_{3}^{2−} (a q) ⟶ {SO}_{4}^{2−} (a q) \\ H_{2} O(l) + {SO}_{3}^{2−} (a q) ⟶ {SO}_{4}^{2−} (a q) \\ H_{2} O(l) + {SO}_{3}^{2−} (a q) ⟶ {SO}_{4}^{2−} (a q) + 2 H^{+} (a q) \\ H_{2} O(l) + {SO}_{3}^{2−} (a q) ⟶ {SO}_{4}^{2−} (a q) + 2 H^{+} (a q) + 2 e^{-} \end{array};$ (g) $\begin{array}{l} {MnO}_{4}^{-} (a q) ⟶ {Mn}^{2+} (a q) \\ {MnO}_{4}^{-} (a q) ⟶ {Mn}^{2+} (a q) + 4 H_{2} O(l) \\ 8 H^{+} (a q) + {MnO}_{4}^{-} (a q) ⟶ {Mn}^{2+} (a q) + 4 H_{2} O(l) \\ 8 H^{+} (a q) + {MnO}_{4}^{-} (a q) + 5 e^{-} ⟶ {Mn}^{2+} (a q) + 4 H_{2} O(l) \end{array};$ (h) $\begin{array}{l} {Cl}^{−} (a q) ⟶ {ClO}_{3}^{-} (a q) \\ 3 H_{2} O(l) + {Cl}^{−} (a q) ⟶ {ClO}_{3}^{-} (a q) \\ 3 H_{2} O(l) + {Cl}^{−} (a q) ⟶ {ClO}_{3}^{-} (a q) + 6 H^{+} (a q) \\ 3 H_{2} O(l) + {Cl}^{−} (a q) + 6 {OH}^{-} (a q) ⟶ {ClO}_{3}^{-} (a q) + 6 H^{+} (a q) + 6 {OH}^{-} (a q) \\ 3 H_{2} O(l) + {Cl}^{−} (a q) + 6 {OH}^{−} (a q) ⟶ {ClO}_{3}^{-} (a q) + 6 H_{2} O(l) \\ {Cl}^{−} (a q) + 6 {OH}^{−} (a q) ⟶ Cl O_{3}^{−} (a q) + 3 H_{2} O(l) + 6 e^{-} \end{array}$

Complete and balance each of the following half-reactions (steps 2–5 in half-reaction method):

(a) ${Cr}^{2+} (a q) ⟶ {Cr}^{3+} (a q)$

(b) $Hg(l) + {Br}^{-} (a q) ⟶ {HgBr}_{4}^{2−} (a q)$

(d) $H_{2} (g) ⟶ H_{2} O(l) (in basic solution)$

(e) $H_{2} (g) ⟶ H_{3} O^{+} (a q) (in acidic solution)$

(f) ${NO}_{3}^{-} (a q) ⟶ {HNO}_{2} (a q) (in acidic solution)$

(g) ${MnO}_{2} (s) ⟶ {MnO}_{4}^{-} (a q) (in basic solution)$

(h) ${Cl}^{-} (a q) ⟶ {ClO}_{3}^{-} (a q) (in acidic solution)$

For an example of the fully worked out solution, see the solution to [link] . (a) ${Cr}^{2+} (a q) ⟶ {Cr}^{3+} (a q) + e^{-};$ (b) $Hg(l) + 4 {Br}^{-} (a q) ⟶ {HgBr}_{4}^{2−} (a q) + 2 e^{-};$ (c) $ZnS(s) + 2 e^{−} ⟶ Zn(s) + S^{2−} (a q);$ (d) $H_{2} (g) + 2 {OH}^{-} (a q) ⟶ 2 H_{2} O(l) + 2 e^{-};$ (e) $H_{2} (g) + 2 H_{2} O(l) ⟶ 2 H_{3} O^{+} (a q) + 2 e^{-};$ (f) ${NO}_{3}^{−} (a q) + 3 H_{3} O^{+} (a q) + 2 e^{-} ⟶ {HNO}_{2} (a q) + 4 H_{2} O(l);$ (g) ${MnO}_{2} (s) + 4 {OH}^{−} (a q) ⟶ {MnO}_{4}^{−} (a q) + 2 H_{2} O(l) + 3 e^{-};$ (h) ${Cl}^{−} (a q) + 3 H_{2} O(l) ⟶ {ClO}_{3}^{−} (a q) + 6 H_{3} O^{+} (a q) + 6 e^{-}$

Balance each of the following equations according to the half-reaction method:

(a) ${Sn}^{2+} (a q) + {Cu}^{2+} (a q) ⟶ {Sn}^{4+} (a q) + {Cu}^{+} (a q)$

(b) $H_{2} S(g) + {Hg}_{2}^{2+} (a q) ⟶ H g (l) + S(s) (in acid)$

(d) ${Fe}^{2+} (a q) + {Ce}^{4+} (a q) ⟶ {Fe}^{3+} (a q) + {Ce}^{3+} (a q)$

(e) $HBrO(a q) ⟶ {Br}^{-} (a q) + O_{2} (g) (in acid)$

For an example of the fully worked out solution, see the solution to [link] . (a) ${Sn}^{2+} (a q) + 2 {Cu}^{2+} (a q) ⟶ {Sn}^{4+} (a q) + 2 {Cu}^{+} (a q);$ (b) $H_{2} S(g) + {Hg}_{2}^{2+} (a q) + 2 H_{2} O(l) ⟶ 2 Hg(l) + S(s) + 2 H_{3} O^{+} (a q);$ (c) $5 {CN}^{-} (a q) + 2 {ClO}_{2} (a q) + 3 H_{2} O(l) ⟶ 5 {CNO}^{-} (a q) + 2 {Cl}^{-} (a q) + 2 H_{3} O^{+} (a q);$ (d) ${Fe}^{2+} (a q) + {Ce}^{4+} (a q) ⟶ {Fe}^{3+} (a q) + {Ce}^{3+} (a q);$ (e) $2 HBrO(a q) + 2 H_{2} O(l) ⟶ 2 H_{3} O^{+} (a q) + 2 {Br}^{-} (a q) + O_{2} (g)$

Balance each of the following equations according to the half-reaction method:

(a) $Zn(s) + {NO}_{3}^{-} (a q) ⟶ {Zn}^{2+} (a q) + N_{2} (g) (in acid)$

(b) $Zn(s) + {NO}_{3}^{-} (a q) ⟶ {Zn}^{2+} (a q) + {NH}_{3} (a q) (in base)$

(d) ${NH}_{3} (a q) + O_{2} (g) ⟶ {NO}_{2} (g) (gas phase)$

(e) ${Cl}_{2} (g) + {OH}^{-} (a q) ⟶ {Cl}^{-} (a q) + {ClO}_{3}^{-} (a q) (in base)$

(f) $H_{2} O_{2} (a q) + {MnO}_{4}^{-} (a q) ⟶ {Mn}^{2+} (a q) + O_{2} (g) (in acid)$

(g) ${NO}_{2} (g) ⟶ {NO}_{3}^{-} (a q) + {NO}_{2}^{-} (a q) (in base)$

(h) ${Fe}^{3+} (a q) + I^{−} (a q) ⟶ {Fe}^{2+} (a q) + I_{2} (a q)$

For an example of the fully worked out solution, see the solution to [link] . (a) $5 Zn(s) + 12 H_{3} O^{+} (a q) + 2 {NO}_{3}^{−} (a q) ⟶ 5 {Zn}^{2+} (a q) + N_{2} (g) + 18 H_{2} O(l);$ (b) $4 Zn(s) + {NO}_{3}^{−} (a q) + 6 H_{2} O(l) ⟶ 4 {Zn}^{2+} (a q) + {NH}_{3} (a q) + 9 {OH}^{−} (a q);$ (c) $3 CuS(s) + 8 H_{3} O^{+} (a q) + 2 {NO}_{3}^{−} (a q) ⟶ 3 {Cu}^{2+} (a q) + 3 S(s) + 2 NO(g) + 12 H_{2} O(l);$ (d) $4 {NH}_{3} (a q) + 7 O_{2} (g) ⟶ 4 {NO}_{2} (g) + 6 H_{2} O(l);$ (e) $3 {Cl}_{2} (g) + 6 {OH}^{−} (a q) ⟶ 5 {Cl}^{−} (a q) + {ClO}_{3}^{−} (a q) + 3 H_{2} O(l);$ (f) $5 H_{2} O_{2} (a q) + 2 {MnO}_{4}^{−} (a q) + 6 H_{3} O^{+} (a q) ⟶ 2 {Mn}^{2+} (a q) + 5 O_{2} (g) + 14 H_{2} O(l);$ (g) $2 {NO}_{2} (g) + 2 {OH}^{−} (a q) ⟶ {NO}_{3}^{−} (a q) + {NO}_{2}^{−} (a q) + H_{2} O(l);$ (h) $2 {Fe}^{3+} (a q) + 2 I^{−} (a q) ⟶ 2 {Fe}^{2+} (a q) + I_{2} (a q)$

Balance each of the following equations according to the half-reaction method:

(a) ${MnO}_{4}^{−} (a q) + {NO}_{2}^{−} (a q) ⟶ {MnO}_{2} (s) + {NO}_{3}^{−} (a q) (in base)$

(b) ${MnO}_{4}^{2−} (a q) ⟶ {MnO}_{4}^{−} (a q) + {MnO}_{2} (s) (in base)$

For an example of the fully worked out solution, see the solution to [link] . (a) $2 {MnO}_{4}^{−} (a q) + {3NO}_{2}^{−} (a q) + H_{2} O(l) ⟶ 2 {MnO}_{2} (s) + 3 {NO}_{3}^{−} (a q) + 2 {OH}^{−} (a q);$ (b) $3 {MnO}_{4}^{2−} (a q) + 2 H_{2} O(l) ⟶ 2 {MnO}_{4}^{−} (a q) + 4 {OH}^{−} (a q) + {MnO}_{2} (s) (in base);$ (c) ${Br}_{2} (l) + {SO}_{2} (g) + 2 H_{2} O(l) ⟶ 4 H^{+} (a q) + 2 {Br}^{−} (a q) + {SO}_{4}^{2−} (a q)$

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Practice Key Terms 23

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Source: OpenStax, Ucd bis2a intro to biology v1.2. OpenStax CNX. Sep 22, 2015 Download for free at https://legacy.cnx.org/content/col11890/1.1

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