Complete and balance the following chemical equations:
(a) \(\text{MnO}_4^- + \text{C}_2\text{O}_4^{2-} + \text{H}^+ \to \)
(b) \(\text{KMnO}_4 \xrightarrow{\text{Heat}} \)
(c) \(\text{Cr}_2\text{O}_7^{2-} + \text{H}_2\text{S} + \text{H}^+ \to \)
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Always ensure to balance the number of atoms and charge on both sides of the reaction. Redox reactions often require you to consider electron balance as well.
(a) The balanced equation for the reaction between permanganate and oxalate in an acidic environment is: \[ 2\text{MnO}_4^- + 5\text{C}_2\text{O}_4^{2-} + 16\text{H}^+ \to 2\text{Mn}^{2+} + 10\text{CO}_2 + 8\text{H}_2\text{O} \] (b) Heating potassium permanganate yields potassium manganate: \[ 2\text{KMnO}_4 \xrightarrow{\text{Heat}} 2\text{K}_2\text{MnO}_4 + \text{O}_2 \] (c) The reaction between dichromate and hydrogen sulfide in an acidic environment is: \[ \text{Cr}_2\text{O}_7^{2-} + 3\text{H}_2\text{S} + 8\text{H}^+ \to 2\text{Cr}^{3+} + 3\text{SO}_2 + 4\text{H}_2\text{O} \]