When the following reaction is balanced in acidic solution,what is the coefficient of I₂? IO₃^- + I^- $\to$ I₂

Question

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First, let's identify the atoms that are being oxidized and reduced in the reaction. We can assign oxidation states to each atom to do so: ION: +1 +5 -2 +6 -2 -1 +1 -2 +1 -2 -1 +1 -2 left: I₂ IO₃^- F1F1F1S1F1F1F10 right: I₂ F1F1F10 Bromine is being reduced from +5 to -1, gaining electrons. We need to balance the number of electrons gained by bromine with the number of electrons lost by fluorine. The coefficient of the fluorine compound is already balanced with respect to fluorine, so we just need to balance the bromine and the electrons. There are 2 bromine atoms on each side, but the left side has a total of 13 electrons while the right side only has 10. To balance this, we can add 3 electrons to the right side: ION: +1 +5 -2 +6 -2 -1 +1 -2 +1 -2 -1 +1 -2 left: I₂ IO₃^- F1F1F1S1F1F1F10 right: I₂ F1F1F103e-F1F1F10 Now we can balance the bromine by adding a coefficient of 2 to the left-hand side: ION: +1 +5 -2 +6 -2 -1 +1 -2 +1 -2 -1 +1 -2 left: 2I₂ 2IO₃^- F1F1F1S1F1F1F10 right: I₂ F1F1F103e-F1F1F10 The coefficient of I₂ on the left-hand side is 2. Therefore, the answer is (C) 3.

When the Following Reaction Is Balanced in Acidic Solution,what Is →\to→

When the Following Reaction Is Balanced in Acidic Solution,what Is $\to$