Balance the following oxidation-reduction equation: Al(s) + Ag⁺(aq) → Al³⁺(aq) + Ag(s) A) Al(s) + Ag⁺(aq) → Al³⁺(aq) + Ag(s) B) 3Al(s) + Ag⁺(aq) → 3Al³⁺(aq) + Ag(s) C) Al(s) + 3Ag⁺(aq) → Al³⁺(aq) + 3Ag(s) D) 3Al(s) + Ag⁺(aq) → Al³⁺(aq) + 3Ag(s) E) Al(s) + 3Ag⁺(aq) → 3Al³⁺(aq) + Ag(s)

Question

Quizplus · Accepted Answer

In the balanced equation, aluminum (Al) is oxidized, going from a 0 oxidation state to a +3 oxidation state, while silver (Ag) is reduced, going from a +1 oxidation state to a 0 oxidation state. For every Al atom that is oxidized, three Ag+ ions are reduced to maintain charge balance, resulting in the correct stoichiometry being 1 Al(s) reacts with 3 Ag+ ions to produce 1 Al3+ ion and 3 Ag(s) atoms.

Balance the Following Oxidation-Reduction Equation: Al(s) + Ag+(aq) → Al3+(aq)

Balance the Following Oxidation-Reduction Equation: Al(s) + Ag⁺(aq) → Al³⁺(aq)