Question

Questions on balancing redox reaction and their workings .

Answer 1

[AI-generated answer — Bot GPT 3.5]

1) How do you balance a redox reaction?

To balance a redox reaction, you start by assigning oxidation states to each element in the reactants and products. Then, identify the element that is being oxidized and the element being reduced. Next, balance the atoms other than hydrogen and oxygen. After that, balance the oxygen atoms by adding water molecules to the side of the equation that lacks oxygen atoms. Finally, balance the hydrogen atoms by adding hydrogen ions (H+) to the side of the equation that lacks hydrogen atoms. Overall charge should also be balanced by adding electrons (e-) to one side of the equation. Make sure the total electrons lost in oxidation are equal to the total electrons gained in reduction. Adjust coefficients accordingly until the equation is balanced in terms of atoms and charges.

2) Can you provide an example of balancing a redox reaction?

Sure! Let's balance the following redox reaction:

Fe2+ + MnO4- -> Fe3+ + Mn2+

Step 1: Assign oxidation states -
Fe2+ (reduced form) and Fe3+ (oxidized form)
MnO4-: Mn = +7 (oxidized form), O = -2, overall charge = -1

Step 2: Identify the element being oxidized and the element being reduced -
Fe is being oxidized from +2 to +3 (losing electrons)
Mn is being reduced from +7 to +2 (gaining electrons)

Step 3: Balance atoms other than hydrogen and oxygen -
Fe2+ + MnO4- -> Fe3+ + Mn2+

Step 4: Balance oxygen atoms -
Fe2+ + MnO4- -> Fe3+ + Mn2+ + 4O2-

Step 5: Balance hydrogen atoms -
Fe2+ + 4H+ + MnO4- -> Fe3+ + Mn2+ + 4O2- + 2H+

Step 6: Balance charge by adding electrons -
Fe2+ + 4H+ + MnO4- -> Fe3+ + Mn2+ + 4O2- + 2H+ + 5e-

Step 7: Multiply half-reactions to balance the electrons -
5(Fe2+ + 4H+ + MnO4-) -> 5(Fe3+ + Mn2+ + 4O2- + 2H+ + 5e-)

Final balanced equation:
5Fe2+ + 4H+ + MnO4- -> 5Fe3+ + Mn2+ + 4O2- + 2H+ + 5e-