Aacha see let H2So4 then :-we have,O.N of H is +1O.N of S we don't have so let it be xO.N of O is -2 we had taken H2So4 na then put the value in thatNow,H2So4= (+1)*2+(x)*1+(-2)*4 =0 = 2+x-8 =0= 2+x =8= x =8-2= x =+6Therefore, we get the O.N of S is +6.so, it's very simple yaar and this is a very Easy way to Balance the Equation. Hope it will help you.😏😏

Understanding the Oxidation Number Method
The oxidation number method is a systematic approach for balancing redox reactions by tracking the changes in oxidation states of elements involved. Here’s a step-by-step guide:
Step 1: Assign Oxidation Numbers
- Determine the oxidation state of each element in the reactants and products.
- Use standard rules for oxidation states (e.g., O is usually -2, H is +1).
Step 2: Identify Changes in Oxidation Numbers
- Identify which elements are oxidized (increase in oxidation number) and which are reduced (decrease in oxidation number).
- Write down the oxidation and reduction half-reactions.
Step 3: Write Half-Reactions
- Separate the oxidation and reduction processes into two half-reactions.
- Ensure that each half-reaction is balanced for atoms and charge.
Step 4: Balance Electrons
- Adjust the number of electrons lost in the oxidation half-reaction to match the number of electrons gained in the reduction half-reaction.
- You can do this by multiplying the half-reactions by appropriate coefficients.
Step 5: Combine Half-Reactions
- Add the balanced half-reactions together.
- Ensure that electrons cancel out and that all elements and charges are balanced.
Step 6: Verify the Final Equation
- Check that the number of atoms of each element and the total charge are the same on both sides of the equation.
- Make any necessary adjustments to achieve balance.
By following these steps, you can effectively balance redox reactions using the oxidation number method. This method is particularly useful in complex reactions where charge and mass balance can be challenging to achieve.