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Redox Reactions – Examples (1 – Synthesis)

Redox Reactions – Examples (1 – Synthesis) The following is one type of oxidation/ reduction reaction. Balance the equation. Indicate the species that are oxidized and reduced. Write the half reactions for each. Fe + O 2 ---> Fe 2 O 3.

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Redox Reactions – Examples (1 – Synthesis)

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  1. Redox Reactions – Examples (1 – Synthesis) The following is one type of oxidation/ reduction reaction. Balance the equation. Indicate the species that are oxidized and reduced. Write the half reactions for each. Fe + O2 ---> Fe2O3

  2. The following is one type of oxidation/ reduction reaction. Balance the equation. Indicate the species that are oxidized and reduced. Write the half reactions for each. Fe(s) + O2(g) ---> Fe2O3 (s) 4Fe + 3O2 ---> 2Fe2O3 balanced

  3. The following is one type of oxidation/ reduction reaction. • Balance the equation. • Indicate the species that are oxidized and reduced. • Write the half reactions for each. • Fe + O2 ---> Fe2O3 • 4Fe + 3O2 ---> 2Fe2O3 balanced • Oxidation: Iron • Fe ---> Fe3+ + 3e‒ • Electrons are removed • Oxygen is added • Charge increases

  4. The following is one type of oxidation/ reduction reaction. • Balance the equation. • Indicate the species that are oxidized and reduced. • Write the half reactions for each. • Fe + O2 ---> Fe2O3 • 4Fe + 3O2 ---> 2Fe2O3 balanced • Oxidation: Iron • Fe ---> Fe3+ + 3e‒ • Electrons are removed • Oxygen is added • Charge increases • Reduction: Oxygen • O0 + 2e‒ ---> O2‒ • Electrons are added • Charge decreases

  5. Half Reactions: Fe0---> Fe3+ + 3e‒ O0 + 2e‒ ---> O2‒ Multiply coefficients through so that electrons cancel. 2Fe0---> 2Fe3+ + 6e‒ 3 O0+ 6e‒ ---> 3 O2‒ After electrons are cancelled: 2Fe0---> 2Fe3+ 3 O0---> 3 O2‒ Change elemental oxygen to diatomic, elemental. 2Fe0---> 2Fe3+ 1½ O20---> 3 O2‒ Multiply coefficients through so that they are whole numbers 4Fe0---> 4Fe3+ 3 O20 ---> 6 O2‒ Combine. 4Fe + 3 O2---> 4Fe3+ 6 O2‒ Combine ions to make a compound, adjust coefficient. 4Fe + 3 O2---> 2Fe2O3

  6. (2 – single replacement) Another type of oxidation/ reduction reaction is as follows. Balance the equation. Indicate the species that are oxidized and reduced. Write the half reactions for each. Fe(s) + CuSO4(aq) ---> FeSO4(aq) + Cu(s)

  7. (2 – single replacement) Another type of oxidation/ reduction reaction is as follows. Balance the equation. Indicate the species that are oxidized and reduced. Write the half reactions for each. Fe(s) + CuSO4(aq) ---> FeSO4(aq) + Cu(s) Balanced!

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