Balanced ionic equation for ClO + Fe(OH)3 = Cl + FeO4. Show electron balance and work
Here is a good site to show you how to do these. Post any specific questions you have.
http://www.chemteam.info/Redox/Redox.html
To write the balanced ionic equation for the reaction between ClO and Fe(OH)3, we need to first determine the oxidation states of the elements in each compound.
The oxidation state of chlorine (Cl) in ClO is +1, and the oxidation state of oxygen (O) is -2. Since the overall charge of ClO is 0, the oxidation state of chlorine must change to -1 in the balanced equation.
The oxidation state of iron (Fe) in Fe(OH)3 is +3, and the oxidation state of oxygen (O) is -2. Since the overall charge of Fe(OH)3 is 0, the oxidation state of iron remains the same in the balanced equation.
Now, let's write the balanced ionic equation:
ClO + Fe(OH)3 → Cl + FeO4
To balance the equation, we need to ensure that the number of each type of atom is the same on both sides. Let's start by balancing the atoms other than oxygen (O) and hydrogen (H).
On the reactant side, we have 1 Cl atom, 1 Fe atom, 3 O atoms, and 3 H atoms.
On the product side, we have 1 Cl atom, 1 Fe atom, and 4 O atoms.
To balance the chlorine (Cl) and iron (Fe) atoms, we can write:
Balanced equation: ClO + Fe(OH)3 → Cl + Fe(OH)3
Now, let's balance the oxygen (O) and hydrogen (H) atoms:
On the reactant side, we have 1 O atom from ClO and 9 O atoms from Fe(OH)3. We also have 3 H atoms from Fe(OH)3.
On the product side, we have 4 O atoms from FeO4.
To balance the oxygen (O) atoms, we can write:
Balanced equation: 2ClO + 3Fe(OH)3 → 2Cl + 3Fe(OH)3
Finally, let's balance the hydrogen (H) atoms by adding water (H2O) to the reactant side:
Balanced equation: 2ClO + 3Fe(OH)3 → 2Cl + 3Fe(OH)3 + 3H2O
To ensure the electron balance, we need to add electrons (e-) to the appropriate side of the equation. Since iron (Fe) is being reduced from +3 to +4, it gains one electron:
Balanced equation: 2ClO + 3Fe(OH)3 + e- → 2Cl + 3Fe(OH)3 + 3H2O
Therefore, the balanced ionic equation for the reaction between ClO and Fe(OH)3 is:
2ClO + 3Fe(OH)3 + e- → 2Cl + 3Fe(OH)3 + 3H2O
To balance the ionic equation for the reaction between ClO and Fe(OH)3, we need to ensure that the total charges on both sides of the equation are equal and that the number of atoms of each element is the same on both sides.
Here's the step-by-step process to balance the equation:
Step 1: Write the unbalanced equation:
ClO + Fe(OH)3 → Cl + FeO4
Step 2: Separate the reactants and products into their respective ions:
ClO^- + Fe(OH)3 → Cl^- + FeO4^2-
Step 3: Identify the elements that are unbalanced. In this case, we have Chlorine (Cl) and Iron (Fe).
Step 4: Balance the elements one by one. Let's start with Chlorine:
There is 1 Cl on the left and 1 Cl on the right, so Chlorine is already balanced.
Step 5: Now let's balance Iron (Fe):
There is 1 Fe on the left and 1 Fe on the right, so Iron is already balanced.
Step 6: Now let's balance Oxygen (O):
On the left side, we have 4 O atoms from the FeO4^2- ion.
On the right side, we have 1 O atom from the ClO^- ion.
To balance the oxygen, we need to add 3 O atoms on the right side. We can do this by adding 3 H2O molecules to the left side of the equation:
ClO^- + Fe(OH)3 → Cl^- + FeO4^2- + 3H2O
Step 7: Now the equation is partially balanced, but we need to check the charge balance.
On the left side, we have a total charge of -1 from the ClO^- ion.
On the right side, we have a total charge of -1 from the Cl^- ion and -2 from the FeO4^2- ion.
To balance the charges, we need to add 1 electron (e^-) to the right side:
ClO^- + Fe(OH)3 → Cl^- + FeO4^2- + 3H2O + e^-
Now the equation is balanced both in terms of atoms and charges.
To summarize, the balanced ionic equation for the reaction is:
ClO^- + Fe(OH)3 → Cl^- + FeO4^2- + 3H2O + e^-
Note: The balanced equation includes the electron (e^-) to show electron transfer, but it is important to remember that electrons are not typically represented in balanced ionic equations.