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Chapter 5: Problem 38

Balance these equations for redox reactions occurring in acidic solution. (a) $\mathrm{P}_{4}(\mathrm{s})+\mathrm{NO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{NO}(\mathrm{g})$ (b) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{MnO}_{4}^{-} \longrightarrow \mathrm{SO}_{4}^{2-}+\mathrm{Mn}^{2+}$ (c) $\mathrm{HS}^{-}+\mathrm{HSO}_{3}^{-} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}$ (d) $\mathrm{Fe}^{3+}+\mathrm{NH}_{3} \mathrm{OH}^{+} \longrightarrow \mathrm{Fe}^{2+}+\mathrm{N}_{2} \mathrm{O}(\mathrm{g})$

Short Answer

Expert verified
The balanced redox reactions are: (a) \(P_4 + 20 NO_3^- + 24 H^+ \rightarrow 4 H_2PO_4^- + 20 NO\) (b) \(3 S_2O_3^{2-} + 2 MnO_4^- + 8 H^+ \rightarrow 3 SO_4^{2-} + 2 Mn^{2+} + 5 H_2O\) (c) \(HS^- + 2 HSO_3^- \rightarrow S_2O_3^{2-} + 2 H_2O\) (d) \(8 Fe^{3+} + 10 NH_3OH^+ \rightarrow 8 Fe^{2+} + 5 N_2O + 25 H_2O\)

Step by step solution

01

Split the reaction into half-reactions

This allows us to focus on balancing the oxidation and reduction processes separately. Each half reaction should include the reactant being oxidized or reduced, the product of that process, and electrons showing the gain for reduction or loss for oxidation.
02

Balance atoms in half-reactions

Start by balancing the atoms that are not hydrogen or oxygen in the half-reactions, followed by oxygen atoms, which can be balanced using water molecules (\(H_2O\)), and finally balance hydrogen atoms using \(H^+\) ions.
03

Balance charges in half-reactions

This can be achieved by adding electrons which themselves carry charge. If in reduction half-reaction, add the electrons to the left side of the equation, and if in oxidation half-reaction, add the electrons to the right side of the equation.
04

Equalize electron transfer

Make sure the number of electrons lost in the oxidation half-reaction equals the number gained in the reduction half-reaction. If they are not equal, multiply each equation by an appropriate factor so the number of electrons will cancel out when the equations are added together.
05

Combine the half-reactions

Add the half-reactions together and simplify to get the balanced redox reaction.

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Most popular questions from this chapter

Every antacid contains one or more ingredients capable of reacting with excess stomach acid (HCl). The essential neutralization products are \(\mathrm{CO}_{2}\) and/ or \(\mathrm{H}_{2} \mathrm{O} .\) Write net ionic equations to represent the neutralizing action of the following popular antacids. (a) Alka-Seltzer (sodium bicarbonate) (b) Tums (calcium carbonate) (c) milk of magnesia (magnesium hydroxide) (d) Maalox (magnesium hydroxide, aluminum hydroxide) (e) Rolaids \(\left[\mathrm{NaAl}(\mathrm{OH})_{2} \mathrm{CO}_{3}\right]\)

Balance these equations for disproportionation reactions. (a) $\mathrm{MnO}_{4}^{2-} \longrightarrow \mathrm{MnO}_{2}(\mathrm{s})+\mathrm{MnO}_{4}^{-}$ (basic solution) (b) $\mathrm{P}_{4}(\mathrm{s}) \longrightarrow \mathrm{H}_{2} \mathrm{PO}_{2}^{-}+\mathrm{PH}_{3}(\mathrm{g})$ (basic solution) (c) $\mathrm{S}_{8}(\mathrm{s}) \longrightarrow \mathrm{S}^{2-}+\mathrm{S}_{2} \mathrm{O}_{3}^{2-}$ (basic solution) (d) $\mathrm{As}_{2} \mathrm{S}_{3}+\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow \mathrm{AsO}_{4}^{3-}+\mathrm{SO}_{4}^{2-}$

A \(0.4324 \mathrm{g}\) sample of a potassium hydroxide-lithium hydroxide mixture requires \(28.28 \mathrm{mL}\) of \(0.3520 \mathrm{M} \mathrm{HCl}\) for its titration to the equivalence point. What is the mass percent lithium hydroxide in this mixture?

The number of moles of hydroxide ion in 0.300 L of \(0.0050 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) is (a) \(0.0015 ;(\mathrm{b}) 0.0030 ;(\mathrm{c}) 0.0050\) (d) 0.010.

Explain why these reactions cannot occur as written. (a) \(\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{MnO}_{4}^{-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \longrightarrow\) \(\mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1)\) (b) \(\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq})+\mathrm{Cl}_{2}(\mathrm{aq}) \longrightarrow\) \(\mathrm{ClO}^{-}(\mathrm{aq})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}^{+}(\mathrm{aq})\)
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