Problem 94
Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{MnO}_{2}\) b. \(\mathrm{BaCrO}_{4}\) C. \(\mathrm{H}_{2} \mathrm{SO}_{3}\) d. \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)
Problem 95
Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{CrCl}_{3}\) b. \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) c. \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) d. \(\operatorname{Cr}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\)
Problem 96
Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{BiO}^{+}\) b. \(\mathrm{PO}_{4}^{3-}\) c. \(\mathrm{NO}_{2}^{-}\) d. \(\mathrm{Hg}_{2}^{2+}\)
Problem 97
In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. \(\mathrm{C}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)\) b. \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}_{2}(g)\) c. \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) d. \(\mathrm{C}_{2} \mathrm{H}_{2}(g)+2 \mathrm{H}_{2}(g) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)\)
Problem 98
In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. \(2 \mathrm{B}_{2} \mathrm{O}_{3}(s)+6 \mathrm{Cl}_{2}(g) \rightarrow 4 \mathrm{BCl}_{3}(l)+3 \mathrm{O}_{2}(g)\) b. \(\operatorname{GeH}_{4}(g)+\mathrm{O}_{2}(g) \rightarrow \operatorname{Ge}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{C_{2} H_{4}(g)+C l_{2}(g) \rightarrow C_{2} H_{4} C l_{2}(l)}\) d. \(\mathrm{O}_{2}(g)+2 \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{OF}_{2}(g)\)
Problem 99
Balance each of the following half-reactions. a. \(\mathrm{I}^{-}(a q) \rightarrow \mathrm{I}_{2}(s)\) b. \(\mathrm{O}_{2}(g) \rightarrow \mathrm{O}^{2-}(s)\) c. \(\mathrm{P}_{4}(s) \rightarrow \mathrm{P}^{3-}(s)\) d. \(\mathrm{Cl}_{2}(g) \rightarrow \mathrm{Cl}^{-}(a q)\)
Problem 100
Balance each of the following half-reactions, which take place in acidic solution. a. \(\mathrm{SiO}_{2}(s) \rightarrow \mathrm{Si}(s)\) b. \(\mathrm{S}(s) \rightarrow \mathrm{H}_{2} \mathrm{S}(a q)\) c. \(\mathrm{NO}_{3}^{-}(a q) \rightarrow \mathrm{HNO}_{2}(a q)\) d. \(\mathrm{NO}_{3}(a q) \rightarrow \mathrm{NO}(g)\)
Problem 101
Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method. a. \(\mathrm{I}^{-}(a q)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{I}_{2}(a q)+\mathrm{Mn}^{2+}(a q)\) b. \(\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(a q)+\mathrm{Cr}^{3+}(a q) \rightarrow \mathrm{SO}_{4}^{2-}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)\) c. \(\mathrm{BiO}_{3}^{-}(a q)+\mathrm{Mn}^{2+}(a q) \rightarrow \mathrm{Bi}^{3+}(a q)+\mathrm{MnO}_{4}^{-}(a q)\)
Problem 102
Potassium permanganate, \(\mathrm{KMnO}_{4}\), is one of the most widely used oxidizing agents. Balance each of the following oxidation-reduction reactions of the permanganate ion in acidic solution by using the "half-reaction" method. a. \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{C}_{2} \mathrm{O}_{4}^{2-}(a q) \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{CO}_{2}(g)\) b. \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q)\) c. \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Cl}^{-}(a q) \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Cl}_{2}(g)\)
Problem 103
Consider the oxidation-reduction reaction \(\mathrm{Mg}(s)+\mathrm{Cu}^{2+}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cu}(s)\) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
