Balancing Redox Reactions
Balance the following redox reaction occurring in acidic solution.
\mathrm{I}^{-}(a q)+\mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q)~\longrightarrow~\mathrm{Cr}^{3+}(a q)+\mathrm{I}_{2}(s)
1. Follow the half-reaction method for balancing redox reactions. Begin by assigning oxidation states.
2. Separate the overall reaction into two half-reactions.
OXIDATION \mathrm{I}^{-}(a q)~\longrightarrow~\mathrm{I}_{2}(s)
REDUCTION \mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q) \longrightarrow \mathrm{C r}^{3^{+}}(a q)
3. Balance each half-reaction with respect to mass.
• Balance all elements other than H and O.
• Balance O by adding \mathrm{H}_{2}\mathrm{O}.
• Balance H by adding \mathrm{H}^{+}.
2~\mathrm{I}^{-}(a q)\longrightarrow\mathrm{I}_{2}(a q)
\mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q)\longrightarrow\mathrm{2}\:\mathrm{Cr}^{\mathrm{3}^{+}}(s)
2~\mathrm{I}^{-}(a q)\longrightarrow\mathrm{I}_{2}(s)
\mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q)\longrightarrow2\,\mathrm{Cr}^{~3+}(a q)+7\,\mathrm{H}_{2}\mathrm{O}(l)
2~\mathrm{I}^{-}(a q)\longrightarrow\mathrm{I}_{2}(s)
\mathrm{14~H^{+}(a q)+\mathrm{C r_{2}O_{7}^{~2-}(a q)}\longrightarrow2\,C r^{3+}(a q)+7~\mathrm{H_{2}O(l)}}
4. Balance each half-reaction with respect to charge.
2~\mathrm{I}^{-}(a q)\longrightarrow\mathrm{I}_{2}(s)+2~\mathrm{e}^{-}
6~\mathrm{e}^{-}+14{\mathrm{~H}}^{+}(a q)+{\mathrm{Cr}}_{2}{\mathrm{O}}_{7}^{~2-}(a q)\longrightarrow2\,\mathrm{Cr}^{~3+}(a q)+7\,\mathrm{H_{2}O(l)}
5. Make the number of electrons in both half-reactions equal.
3 \times[2\,\mathrm{I}^{-}(a q) \longrightarrow\,\mathrm{I}_{2}(s) +2~\mathrm{e}^{-}]
6~\mathrm{e}^{-}+14\,\mathrm{H}^{+}(a q)+\mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q)\longrightarrow2\,\mathrm{Cr}^{3+}(a q)+7\,\mathrm{H}_{2}\mathrm{O}(l)
6. Add the half-reactions together.
6~\mathrm{I}^{-}(a q) \longrightarrow 3\ \mathrm{I}_{2}(s)+ \cancel{6~\mathrm{e}^{-}}
\underline{\cancel{6~\mathrm{e}^{-}}~+14\,{\mathrm{H}}^{+}(a q)+\mathrm{Cr}_{2}\mathrm{O}_{7}^{2-}(a q)\longrightarrow2\,\mathrm{Cr}^{3+}(a q)+7\,\mathrm{H}_{2}\mathrm{O}(l)~~~~~}
6\,\mathrm{I}^{-}(a q)+14\,\mathrm{H}^{+}(a q)+\mathrm{Cr}_{2}\mathrm{O}_{7}^{~2-}(a q)\longrightarrow 3\,\mathrm{I}_{2}(s)+2\,\mathrm{Cr}^{~3+}(a q)+7\,\mathrm{H}_{2}\mathrm{O(l)}
7. Verify that the reaction is balanced.
Reactants Products
6 I 6 I
14 H 14 H
2 Cr 2 Cr
7 O 7 O
+6 charge +6 charge