Question
Write a balanced equation describing the reduction of $\mathrm{H}_{2} \mathrm{SeO}_{4}$ by $\mathrm{SO}_{2}$ to produce selenium.
Step 1
Now, we need to balance the equation in terms of both mass and charge. The reduction of Se from +6 to 0 (elemental selenium) requires a gain of 6 electrons, while the oxidation of S from +4 to +6 (forming SOāĀ²ā») requires a loss of 2 electrons. To balance the Show more…
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