I have the question find the balanced equation when Fe(s) is placed in HClO4 (aq).
How do I balance this redox reaction?
I'm not entirely sure its right but the unbalanced equation I have so far is
Fe (s) + HClO4 (aq) -->Fe(ClO4)3 + H2
I'm not sure what to do after that...or how to use the oxidation number/s to solve this problem either.
See your post above.
To balance a redox reaction, you need to follow these steps:
1. Assign oxidation numbers: Start by assigning oxidation numbers to each element in the equation. In this case, Fe (iron) is an element with an oxidation number of 0 since it's in its elemental state. Oxygen (O) generally has an oxidation number of -2. The oxidation number of Cl can be calculated by assuming that H has an oxidation number of +1 and O has an oxidation number of -2.
2. Identify the species being oxidized and reduced: Determine which elements are being oxidized and reduced. Oxidation involves an increase in the oxidation number, while reduction involves a decrease in the oxidation number.
In this case, Fe(s) is being oxidized, as its oxidation number increases from 0 to +3, forming Fe(ClO4)3. H in HClO4 is being reduced, as its oxidation number decreases from +1 to 0, forming H2.
3. Balance the atoms: Balance the atoms in the equation by adjusting the coefficients in front of the chemical formulas. Start by balancing atoms other than hydrogen and oxygen. In this case, you only need to balance Fe and Cl.
Fe(s) + HClO4(aq) -> Fe(ClO4)3 + H2
4. Balance oxygen: Add water molecules (H2O) to balance the oxygen atoms. Since there are 4 oxygen atoms on the right side and 4 chlorine atoms on the left side, we need to add 4 water molecules on the right side.
Fe(s) + HClO4(aq) -> Fe(ClO4)3 + 4H2O
5. Balance hydrogen: Add hydrogen ions (H+) to balance the hydrogen atoms. Since there are now 8 hydrogen atoms on the right side and 1 hydrogen atom on the left side, we need to add 8H+ ions on the left side.
Fe(s) + 8HClO4(aq) -> Fe(ClO4)3 + 4H2O
6. Balance charges: Finally, balance the charges by adding electrons (e-) to one side of the equation. In this case, Fe(ClO4)3 has a charge of 0, so no electrons are needed on that side. The left side has a charge of +8 (from the H+ ions), and Fe(s) has a charge of 0. Since Fe is being oxidized, the electrons are placed on the left side.
Fe(s) -> Fe(ClO4)3 + 4H2O + 8H+ + e-
The balanced equation is:
Fe(s) + 8HClO4(aq) -> Fe(ClO4)3 + 4H2O + 8H+ + e-