The balanced redox equation for the given reaction involving the reduction of chromium ions (Cr3+) and the oxidation of dichlorine heptoxide (Cl2O7) and hydrogen ions (H+) is:
![\[ 10 \text{Cl}_2O_7 + 32 \text{H}^+ + 6 \text{Cr}^(3+) \rightarrow 5 \text{I}_2 + 6 \text{Cr}^(3+) + 21 \text{H}_2O \]](https://img.qammunity.org/2024/formulas/chemistry/high-school/tt285m2gnta5itac7t336o2ad7f3zc753d.png)
This balanced equation ensures conservation of mass and charge, with equal numbers of atoms for each element on both sides of the reaction.
The balanced redox equation illustrates the conservation of mass and charge. Adjusting coefficients ensures an equal number of atoms on both sides, validating the stoichiometric integrity of the reaction.
The given chemical equation represents a redox reaction, involving the reduction of chromium ions (
) and the oxidation of dichlorine heptoxide (
) and hydrogen ions (
), resulting in the formation of iodine molecules (
), chromium ions (
), and water (
).
To balance the equation, it is essential to ensure that the number of atoms for each element is the same on both sides.
The balanced equation is as follows:
![\[ 10I^- + 6Cr_2O_7^(2-) + 32H_3O^+ \rightarrow 5I_2 + 6Cr^(3+) + 21H_2O \]](https://img.qammunity.org/2024/formulas/chemistry/high-school/vhogyuk7zxisiqvcgve0bdjxhh6lvd0sko.png)
This balanced equation obeys the law of conservation of mass and charge. On the reactant side, 10 iodine ions, 6 dichlorine heptoxide ions, and 32 hydrogen ions combine to produce 5 iodine molecules, 6 chromium ions, and 21 water molecules on the product side.
The balancing process involves adjusting coefficients and ensuring that the number of atoms of each element is the same on both sides, preserving the integrity of the chemical equation.