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Balance redox equations
MnO4 - + HCO2H --> Mn^2+ + CO2
K2S3O6 + KClO + KOH --> K2SO4 + KCL + H2O
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I understand that you're struggling with balancing redox equations in chemistry. Don't worry, I'm here to help! Balancing redox equations can seem intimidating at first, but it becomes easier with some practice.
For the first equation:
MnO4- + HCO2H → Mn2+ + CO2
To balance this equation, follow these steps:
Step 1: Break down the equation into two half-reactions: the oxidation half-reaction and the reduction half-reaction.
Oxidation half-reaction: MnO4- → Mn2+
Reduction half-reaction: HCO2H → CO2
Step 2: Balance the elements other than oxygen and hydrogen in each half-reaction.
Oxidation half-reaction: MnO4- → Mn2+
Since there is only one manganese (Mn) atom on both sides, it is already balanced.
Reduction half-reaction: HCO2H → CO2
On the left side, there is one carbon (C) and two oxygen (O) atoms. On the right side, there is one carbon and two oxygen atoms. Therefore, it is already balanced.
Step 3: Balance the oxygen atoms by adding water (H2O) molecules. For every oxygen atom needed, add one water molecule.
Oxidation half-reaction: MnO4- → Mn2+ + 4H2O
Here, four water molecules are added to balance the four oxygen atoms.
Step 4: Balance the hydrogen atoms by adding hydrogen ions (H+). For every hydrogen atom needed, add one hydrogen ion.
Reduction half-reaction: HCO2H + 2H+ → CO2
Here, two hydrogen ions are added to balance the two hydrogen atoms.
Step 5: Balance the charges on each side of the half-reactions by adding electrons (e-) as needed.
Oxidation half-reaction: MnO4- → Mn2+ + 4H2O + 4e-
Here, four electrons are added to balance the charges.
Reduction half-reaction: HCO2H + 2H+ + 2e- → CO2
In this case, two electrons are added to balance the charges.
Step 6: Multiply each half-reaction so that the number of electrons gained equals the number of electrons lost.
In this case, if you multiply the reduction half-reaction by 4 and the oxidation half-reaction by 2, the number of electrons gained and lost will be equal.
Multiply the oxidation half-reaction by 2:
2MnO4- → 2Mn2+ + 8H2O + 8e-
Multiply the reduction half-reaction by 4:
4HCO2H + 8H+ + 8e- → 4CO2
Step 7: Add the balanced half-reactions to obtain the final balanced redox equation.
2MnO4- + 4HCO2H + 8H+ → 2Mn2+ + 4CO2 + 8H2O
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For the second equation:
K2S3O6 + KClO + KOH → K2SO4 + KCl + H2O
Follow the same steps mentioned above to balance this equation.
After balancing, the balanced redox equation will be:
3K2S3O6 + 6KClO + 12KOH → 6K2SO4 + 6KCl + 9H2O
Remember, balancing redox equations requires practice. By following these steps and practicing more examples, you'll gain more confidence in balancing redox equations.