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The Finish Line is in site…. Electrochemistry. Balancing Redox Equations. It is essential to write a correctly balanced equation that represents what happens in a chemical reaction We will be using the ½ reaction Method to balance redox reactions. Using half-reactions.

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balancing redox equations
Balancing Redox Equations
  • It is essential to write a correctly balanced equation that represents what happens in a chemical reaction
    • We will be using the ½ reaction Method to balance redox reactions.
using half reactions
Using half-reactions
  • A half-reaction is an equation showing just the oxidation or just the reduction that takes place
  • They are then balanced separately, and finally combined
using half reactions1

Step 1: write unbalanced equation in ionic form

  • Step 2: write separate half-reaction equations for oxidation and reduction
  • Step 3: balance the atoms in the half-reactions (Except O and H)
  • Step 4: Balance the O by adding water molecules to the other side
Using half-reactions
using half reactions2
Using half-reactions
  • Step 5: Balance the H atoms by adding H+ ions to the other side.
  • Step 6: add enough electrons to one side of each half-reaction to balance the charges
  • Step 7: multiply each half-reaction by a number to make the electrons equal in both
  • Step 8: add the balanced half-reactions to show an overall equation
using half reactions in a basic solution
Using half-reactions: In a basic solution
  • Step 9: add enough OH- ions to equal the number of H+ ions present
  • Step 10: form water molecules by combining OH- and H+ ions
  • Step 11: ‘clean-up’ the balanced equation by simplifying the water molecules if needed.