Balancing Redox Reactions in Acidic Medium

The video tutorial explains how to balance a redox reaction involving Cr2O7 2- and C2O4 2- in an acidic medium. It begins by assigning oxidation numbers and identifying species that change oxidation states. The tutorial then details balancing half reactions by atoms and charge, followed by balancing the overall reaction by equalizing electrons. The process concludes with a final check of atom and charge balance, resulting in a balanced redox equation.

What is the first step in balancing a redox reaction in acidic medium?

• Adding water molecules

• Balancing the charges

• Writing the oxidation numbers

• Combining half-reactions

Which element undergoes reduction in the given redox reaction?

• Chromium

• Oxygen

• Carbon

• Hydrogen

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

• By adding more reactants

• By adding water molecules

• By adding electrons

• By adding hydrogen ions

What is the purpose of adding hydrogen ions in the half-reactions?

• To balance oxygen atoms

• To balance charges

• To balance hydrogen atoms

• To balance electrons

How do you ensure the charges are balanced in the half-reactions?

• By adding more reactants

• By adding electrons

• By adding water molecules

• By adding hydrogen ions

What is the next step after balancing the half-reactions?

• Adding more reactants

• Balancing the overall charge

• Balancing the products

• Combining the half-reactions

Why do we multiply the half-reaction by three in the final step?

• To balance the electrons

• To balance the hydrogen ions

• To balance the charges

• To balance the oxygen atoms

What is the final check to ensure the redox reaction is balanced?

• Checking the number of reactants

• Checking the number of products

• Checking the charge and atom balance

• Checking the number of electrons

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

• 6+

• 12+

• 6-

• 12-

What is the significance of having the same number of electrons on both sides?

• It ensures the reaction is spontaneous

• It ensures the reaction is endothermic

• It ensures the reaction is exothermic

• It ensures the reaction is balanced