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chap-20-2011W-a

# Write a balanced net ionic equation of this reaction

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Unformatted text preview: d observed the precipitation of MnO2(s). Write a balanced net ionic equation of this reaction. 1. Write the unbalanced equation for the reaction in ionic form H 2 O 2 (aq) + Mn 2+ (aq) → MnO 2 (s) 2. Separate the equation into two half-reactions Mn 2+ (aq) → MnO 2 (s) H 2 O 2 (aq) → H 2 O(l) 3. Balance the half-reactions halfa. Balance the atoms other than O and H in half-reactions atoms other halfMn 2+ (aq) → MnO 2 (s) H 2 O 2 (aq) → 2H 2 O(l) b. add OH- to balance O atoms and H2O to balance H atoms OH atoms to in basic solution in basic solution Mn (aq) → MnO 2 (s) Mn 2+ (aq) + 4OH - → MnO 2 (s) + 2H 2 O(l) H 2 O 2 (aq) → 2H 2 O(l) H 2 O 2 (aq) + 2H 2 O(l) → 2H 2O(l) + 2OH - (aq) 2+ c. Add electrons to balance the charges on the half-reactions electrons balance halfMn 2+ (aq) + 4OH - → MnO 2 (s) + 2H 2 O(l) + 2e H 2 O 2 (aq) + 2H 2 O(l) + 2e → 2H 2 O(l) + 2OH - (aq) 4. Equalize the number of electrons in the two half-reactions by multiplying the half-reactions by appropriate coefficients. Mn 2+ (aq) + 4OH - → MnO 2 (s) + 2H 2 O(l) + 2e H 2 O 2 (aq) + 2e → 2OH - (aq) 5. Add the two half-reactions together and balance the final equation halfMn 2+ (aq) + H 2 O 2 (aq) + 2OH - → MnO 2 (s) + 2H 2 O(l) Voltaic Voltaic Cells (Galvanic Cells) The energy released in a spontaneou...
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