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Chapter 5: Problem 37

Balance these equations for redox reactions occurring in acidic solution. (a) $\mathrm{MnO}_{4}^{-}+\mathrm{I}^{-} \longrightarrow \mathrm{Mn}^{2+}+\mathrm{I}_{2}(\mathrm{s})$ (b) $\mathrm{BrO}_{3}^{-}+\mathrm{N}_{2} \mathrm{H}_{4} \longrightarrow \mathrm{Br}^{-}+\mathrm{N}_{2}$ (c) $\mathrm{VO}_{4}^{3-}+\mathrm{Fe}^{2+} \longrightarrow \mathrm{VO}^{2+}+\mathrm{Fe}^{3+}$ (d) $\mathrm{UO}^{2+}+\mathrm{NO}_{3}^{-} \longrightarrow \mathrm{UO}_{2}^{2+}+\mathrm{NO}(\mathrm{g})$

Short Answer

Expert verified
(a) 5MnO4- + 16H+ + 2I- > 5Mn2+ + 2I2(s) + 8H2O, \n(b) 3BrO3- + 10H+ + 2N2H4 > 3Br- + 2N2 + 6H2O, \n(c) VO4 3- + Fe2+ + H+ > VO2+ + Fe3+ + H2O, \n(d) UO + 2H+ + NO3- > UO2 2+ + NO + H2O

Step by step solution

01

Identify the oxidation and reduction species and assign oxidation numbers

\n(a) In the reaction MnO4- + I- > Mn2+ + I2(s), Mn is reduced from 7 to 2, and I- is oxidized to I2. \n(b) In the reaction BrO3- + N2H4 > Br- + N2, Br is reduced from 5 to -1 and N is oxidized from -2 to 0. \n(c) In the reaction VO4 3- + Fe2+ > VO2+ + Fe3+, V is reduced from 5 to 4 and Fe is oxidized from 2 to 3. \n(d) In the reaction UO+ + NO3- > UO2 2+ + NO, N is reduced from 5 in NO3- to 2 in NO and U is oxidized from 4 to 6.
02

Balance the atoms in the half reactions and add H2O and H+ where necessary

\n(a) Add 8H+ to the left side of the reduction equation (MnO4- > Mn2+) to balance with 4H2O on the right side. Add 2I- on the left side to balance with I2 on the right side in the oxidation equation. \n(b) Add 6H+ to the right side of the reduction equation and 2H2O to the left side to balance with 6H2O on the right side. \n(c) For both the reduction and oxidation equations, no further balancing is needed. \n(d) Add 2H+ to the right side of the reduction equation and H2O to the left side to balance with 2H2O on the right side.
03

Balance charges by adding electrons

\n(a) Add 5 electrons to the left side of the Mn half reaction and 2 to the right side of the I- equation. \n(b) Add 6 electrons to the left side of the Br half reaction and 2 to the left side of the N2H4 equation. \n(c) Add 1 electron to the left side of the Fe2+ equation and 1 to the right side of the VO4 3- equation. \n(d) Add 1 electron to the right side of the NO3- equation and 1 to the right side of the UO equation.
04

Cancel redundant entities and balance the equations

\n(a) Multiply the equations by factors of 5 and 2 respectively and then add them together, cancel out redundant entities. The balanced equation is: 5MnO4- + 16H+ + 2I- > 5Mn2+ + 2I2(s) + 8H2O. \n(b) Multiply the equations by factors of 3 and 2 respectively, the balanced equation will be: 3BrO3- + 10H+ + 2N2H4 > 3Br- + 2N2 + 6H2O. \n(c) There's no need to multiply the equations, the balanced equation is: VO4 3- + Fe2+ + H+ > VO2+ + Fe3+ + H2O. \n(d) There's also no need to multiply the equations, the balanced equation is: UO + 2H+ + NO3- > UO2 2+ + NO + H2O.

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Most popular questions from this chapter

The titration of \(5.00 \mathrm{mL}\) of a saturated solution of sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4},\) at \(25^{\circ} \mathrm{C}\) requires \(25.8 \mathrm{mL}\) of \(0.02140 \mathrm{M} \mathrm{KMnO}_{4}\) in acidic solution. What mass of \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) in grams would be present in \(1.00 \mathrm{L}\) of this saturated solution? \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}+\mathrm{MnO}_{4}^{-} \longrightarrow_{\mathrm{Mn}^{2+}}+\mathrm{CO}_{2}(\mathrm{g}) \quad\) (not balanced)

Which of the following reactions are oxidationreduction reactions? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})\) (b) \(2 \mathrm{Li}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2 \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})\) (c) \(4 \mathrm{Ag}(\mathrm{s})+\mathrm{PtCl}_{4}(\mathrm{aq}) \longrightarrow 4 \mathrm{AgCl}(\mathrm{s})+\mathrm{Pt}(\mathrm{s})\) (d) \(2 \mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \longrightarrow\) \(2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(\mathrm{aq})\)

A method of producing phosphine, \(\mathrm{PH}_{3}\), from elemental phosphorus, \(P_{4}\), involves heating the \(P_{4}\) with \(\mathrm{H}_{2} \mathrm{O} .\) An additional product is phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\) Write a balanced equation for this reaction.

How many milliliters of 2.155 M KOH are required to titrate \(25.00 \mathrm{mL}\) of \(0.3057 \mathrm{M} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\) (prop-ionic acid)?

A \(110.520 \mathrm{g}\) sample of mineral water is analyzed for its magnesium content. The \(\mathrm{Mg}^{2+}\) in the sample is first precipitated as \(\mathrm{MgNH}_{4} \mathrm{PO}_{4},\) and this precipitate is then converted to \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7},\) which is found to weigh 0.0549 g. Express the quantity of magnesium in the sample in parts per million (that is, in grams of \(\mathrm{Mg}\) per million grams of \(\mathrm{H}_{2} \mathrm{O}\) ).
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