Question

plz solve this question I need perfect answer for both the questions
if answer is wrong I won't see I will report u then u loose extra points also

Answer 1

1) Just to start your equation is not balanced. But what I would do is remove all your spectator ions and just focus on the ions that are being oxidised and reduced.

Reduction - MnO−4 →Mn2+
Oxidation - H2O2 → O2

Your K+ and SO2−4 are spectator ions and can be removed.

You balance in the following way:

Add Water to balance Oxygens

Add H+ ions to balance Hydrogens

Add e− to balance out charges

Reduction

MnO−4→Mn2++4H2O

MnO−4+8H+→Mn2++4H2O

MnO−4+8H++5e−→Mn2++4H2O

Oxidation

H2O2→O2 (Oxygen balanced already)

H2O2→O2+2H+

H2O2→O2+2H++2e−

So 2 half equations (stage 3) are

1. MnO−4+8H++5e−→Mn2++4H2O

2. H2O2→O2+2H++2e−

To combine the equations to make an ionic equation you need to make sure the electrons in both equations are the same . To do this we multiply equation 1 by 2 and equation 2 by 5 to give us -
3.** 2MnO−4+16H++10e−→2Mn2++8H2O

4. 5H2O2→5O2+10H++10e−

Combine equation 3. and 4. and cancel out electrons to give -

2MnO−4+16H++5H2O2→2Mn2++5O2+10H++8H2O

Cancel out protons to give

2MnO−4+6H++5H2O2→2Mn2++5O2+8H2O