6. Balanced equations:
a) 2MnO₄⁻ + 10Br⁻ + 16H⁺ → 2Mn²⁺ + 5Br₂ + 8H₂O
b) 2NO₃⁻ + 3Bi + 6H⁺ → 2Bi³⁺ + 3NO₂ + 3H₂O
c) 2MnO₄⁻ + 5C₂H₂O₄ + 6H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O
d) 2HNO₃ + 6I⁻ + 6H⁺ → 2NO + 3I₂ + 4H₂O
e) I₂ + 2NO₃⁻ + 2H⁺ → 2NO₂ + IO₃⁻ + H₂O
f) Al + NO₃⁻ + OH⁻ + H₂O → Al(OH)₄⁻ + NH₃
g) CrO₄²⁻ + H₂O₂ → CrO₅ + H₂O
h) 2Fe(OH)₂ + H₂O₂ → 2Fe(OH)₃
i) 5I⁻ + IO₃⁻ + 6H⁺ → 3I₂ + 3H₂O
7. Standard EMF = 1.22 V; Cell reaction: Al(s) + Fe³⁺(aq) → Al³⁺(aq) + Fe(s)
8. Salt bridge maintains electrical neutrality by allowing ion flow between half-cells, preventing charge buildup and completing the circuit.
9. Mg(s) | Mg²⁺(aq) || Al³⁺(aq) | Al(s); Zn(s) | Zn²⁺(aq) || Ag⁺(aq) | Ag(s)
10. Not feasible; E°_cell = -0.476 V (negative, so non-spontaneous).
Parent Tip: Review the logic above to help your child master the concept of redox worksheet.
