Balancing Redox Reactions Concepts

This video tutorial demonstrates how to balance a redox reaction using the ion-electron method in an acidic medium. It begins with identifying oxidation numbers and writing half reactions for species with changed oxidation states. The tutorial then guides through balancing atoms, oxygen, hydrogen, and charge using water molecules, H+ ions, and electrons. Finally, it covers the simplification of half reactions to achieve a balanced overall equation.

What method is used to balance redox reactions in the video?

• Ion-electron method

• Molecular method

• Stoichiometric method

• Empirical method

Which element undergoes reduction in the given redox reaction?

• Carbon

• Chromium

• Oxygen

• Hydrogen

How are oxygen atoms balanced in the half-reactions?

• By adding electrons

• By adding water molecules

• By adding H+ ions

• By adding hydroxide ions

What is added to balance hydrogen atoms in the half-reactions?

• Water molecules

• OH- ions

• Electrons

• H+ ions

How is the charge balanced in the half-reactions?

• By adding water molecules

• By adding electrons

• By adding H+ ions

• By adding OH- ions

What is the purpose of multiplying the half-reactions by 2?

• To balance the number of atoms

• To balance the number of electrons

• To balance the number of molecules

• To balance the number of ions

What is the final step in balancing the redox reaction?

• Removing excess electrons

• Simplifying the half-reactions

• Adding more reactants

• Adding more products

What is the charge on the reactant side after balancing?

• 12 plus

• 16 plus

• 10 plus

• 14 plus

What is the charge on the product side after balancing?

• 16 plus

• 10 plus

• 12 plus

• 14 plus

What is the overall balanced equation for the reaction?

• Cr2O7^2- + C2H5OH → Cr^3+ + CO2

• Cr2O7^2- + C2H5OH → Cr^2+ + CO2

• Cr2O7^2- + C2H5OH → Cr^2+ + H2O

• Cr2O7^2- + C2H5OH → Cr^3+ + H2O