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Chapter 4: Problem 88

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{Al}(s) \rightarrow \mathrm{Al}^{3+}(a a)+\mathrm{Cl}^{-}(a q)\) b. \(\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Pb}(s) \rightarrow \mathrm{Pb}(\mathrm{OH})_{2}(s)\) c. \(\mathrm{H}^{+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \rightarrow\) \(\mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

Short Answer

Expert verified
The balanced oxidation-reduction reactions are: a. \(2\mathrm{Cl}_{2}(g) + 2\mathrm{Al}(s) \rightarrow 2\mathrm{Al}^{3+}(a q) + 6\mathrm{Cl}^{-}(a q)\) b. \(1/2\mathrm{O}_{2}(g) + \mathrm{H}_{2} \mathrm{O}(l) + \mathrm{Pb}(s) \rightarrow \mathrm{Pb}(\mathrm{OH})_{2}(s)\) c. \(8\mathrm{H}^{+}(a q) + \mathrm{MnO}_{4}^{-}(a q) + 5\mathrm{Fe}^{2+}(a q) \rightarrow \mathrm{Mn}^{2+}(a q) + 5\mathrm{Fe}^{3+}(a q) + 4\mathrm{H}_{2} \mathrm{O}(l)\)

Step by step solution

01

Identify the oxidation states

Before the reaction, Cl in Cl2 has an oxidation state of 0, and Al has an oxidation state of 0. After the reaction, the oxidation state of Al becomes +3 (in Al3+), and the oxidation state of Cl becomes -1 (in Cl-).
02

Balance the electrons lost and gained

Al loses 3 electrons (going from 0 to +3) while each Cl gains 1 electron (going from 0 to -1). Since there are 2 Cl atoms in Cl2, we need 2 Cl- ions to balance the electron gain. Therefore, we need to multiply the Al species by 2 to balance the electron loss. The balanced reaction is: 2Cl2(g) + 2Al(s) → 2Al3+(aq) + 6Cl-(aq) b. \(\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Pb}(s) \rightarrow \mathrm{Pb}(\mathrm{OH})_{2}(s)\)
03

Identify the oxidation states

Before the reaction, O in O2 has an oxidation state of 0, H in H2O has an oxidation state of +1, and Pb has an oxidation state of 0. After the reaction, the oxidation state of O in Pb(OH)2 is -2, and the oxidation state of Pb in Pb(OH)2 is +2.
04

Balance the electrons lost and gained

O gains 2 electrons (going from 0 to -2) while Pb loses 2 electrons (going from 0 to +2). We need to multiply the O2 species by 1/2 to balance the electron gain. The balanced reaction is: 1/2O2(g) + H2O(l) + Pb(s) → Pb(OH)2(s) c. \(\mathrm{H}^{+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)
05

Identify the oxidation states

Before the reaction, the oxidation state of H is +1, Mn in MnO4- is +7, and Fe is +2. After the reaction, the oxidation state of Mn in Mn2+ is +2, Fe in Fe3+ is +3, and O in H2O is -2.
06

Balance the electrons lost and gained

Mn loses 5 electrons (going from +7 to +2) and Fe gains 1 electron (going from +2 to +3). To balance the electron loss for Mn, we need to multiply the Fe species by 5. The balanced reaction is: 8H+(aq) + MnO4^-(aq) + 5Fe2+(aq) → Mn2+(aq) + 5Fe3+(aq) + 4H2O(l)

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Most popular questions from this chapter

A mixture contains only \(\mathrm{NaCl}\) and \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} .\) A \(1.45-\mathrm{g}\) sample of the mixture is dissolved in water and an excess of \(\mathrm{NaOH}\) is added, producing a precipitate of \(\mathrm{Al}(\mathrm{OH})_{3}\). The precipitate is filtered, dried, and weighed. The mass of the precipitate is \(0.107 \mathrm{~g}\). What is the mass percent of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) in the sample?

What volume of \(0.0200 M\) calcium hydroxide is required to neutralize \(35.00 \mathrm{~mL}\) of \(0.0500 \mathrm{M}\) nitric acid?

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{FeSO}_{4}(a q)+\mathrm{KCl}(a q)\) b. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q)\) c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) d. \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Give an example how each of the following insoluble ionic compounds could be produced using a precipitation reaction. Write the balanced formula equation for each reaction. a. \(\mathrm{Fe}(\mathrm{OH})_{3}(s)\) b. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}(s)\) c. \(\mathrm{PbSO}_{4}(s)\) d. \(\mathrm{BaCrO}_{4}(s)\)

A solution is prepared by dissolving \(0.6706 \mathrm{~g}\) oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make \(100.0 \mathrm{~mL}\) of solution. \(\mathrm{A}\) \(10.00-\mathrm{mL}\) aliquot (portion) of this solution is then diluted to a final volume of \(250.0 \mathrm{~mL}\). What is the final molarity of the oxalic acid solution?
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