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balancing_redox_equations

# balancing_redox_equations - coefficients 6Fe 2 6Fe 3 6e-6e...

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Balancing Redox Equations 1. Write the unbalanced equation for the reaction ion in ionic form. The oxidation of Fe 2+ to Fe 3+ by Cr 2 O 7 2- in acid solution? Fe 2+ + Cr 2 O 7 2- Fe 3+ + Cr 3+ 2. Separate the equation into two half-reactions. Oxidation: Cr 2 O 7 2- Cr 3+ +6 +3 Reduction: Fe 2+ Fe 3+ +2 +3 3. Balance the atoms other than O and H in each half-reaction. Cr 2 O 7 2- 2Cr 3+

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Balancing Redox Equations 4. For reactions in acid, add H 2 O to balance O atoms and H + to balance H atoms. Cr 2 O 7 2- 2Cr 3+ + 7H 2 O 14H + + Cr 2 O 7 2- 2Cr 3+ + 7H 2 O 5. Add electrons to one side of each half-reaction to balance the charges on the half-reaction. Fe 2+ Fe 3+ + 1e - 6e - + 14H + + Cr 2 O 7 2- 2Cr 3+ + 7H 2 O 6. If necessary, equalize the number of electrons in the two half- reactions by multiplying the half-reactions by appropriate
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Unformatted text preview: coefficients. 6Fe 2+ 6Fe 3+ + 6e-6e-+ 14H + + Cr 2 O 7 2-2Cr 3+ + 7H 2 O Balancing Redox Equations 7. Add the two half-reactions together and balance the final equation by inspection. The number of electrons on both sides must cancel. 6e-+ 14H + + Cr 2 O 7 2-2Cr 3+ + 7H 2 O 6Fe 2+ 6Fe 3+ + 6e-Oxidation: Reduction: 14H + + Cr 2 O 7 2-+ 6Fe 2+ 6Fe 3+ + 2Cr 3+ + 7H 2 O 8. Verify that the number of atoms and the charges are balanced . 14x1 – 2 + 6 x 2 = 24 = 6 x 3 + 2 x 3 9. For reactions in basic solutions, add OH-to both sides of the equation for every H + that appears in the final equation....
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