Balancing Redox Reactions Concepts

This video tutorial explains how to balance a redox reaction using the ion-electron method in an acidic medium. It covers writing oxidation numbers, identifying half reactions, and balancing atoms and charges using water and hydrogen ions. The tutorial also demonstrates balancing electrons and simplifying the final redox reaction, ensuring both mass and charge are balanced.

What method is used to balance the redox reaction in this tutorial?

• Ion-electron method

• Empirical method

• Stoichiometric method

• Molecular method

What is the oxidation state change for manganese in the reaction?

• From -1 to 0

• From 0 to -1

• From +7 to +2

• From +2 to +7

How do you balance the oxygen atoms in the half-reactions?

• By adding electrons

• By adding hydrogen ions

• By adding water molecules

• By adding oxygen gas

What is added to balance the hydrogen atoms in the reaction?

• Hydrogen gas

• Hydrogen ions

• Water molecules

• Electrons

How are charges balanced in the half-reactions?

• By adding water

• By adding electrons

• By adding neutrons

• By adding protons

What is the purpose of multiplying the half-reactions by different factors?

• To balance the number of ions

• To balance the number of molecules

• To balance the number of atoms

• To balance the number of electrons

What happens to the electrons in the final balanced redox reaction?

• They are added to the products

• They are added to the reactants

• They cancel out

• They are doubled

What is the final charge on the reactant side after balancing?

• 2+

• 4+

• 8+

• 0

What is the final charge on the product side after balancing?

• 0

• 2+

• 4+

• 8+

What is the final balanced redox reaction for MnO4- and I-?

• I2 + Mn2+ → MnO4- + I-

• Mn2+ + I- → I2 + MnO4-

• MnO4- + I2 → I- + Mn2+

• MnO4- + I- → I2 + Mn2+