Question

Balance each reaction below, and write a cell schematic representing the reaction as it would occur in a galvanic cell.

(a) Al()+Zr⁴⁺()⟶Al³⁺()+Zr()Al(s)+Zr⁴⁺(aq)⟶Al³⁺(aq)+Zr(s)

(b) Ag+()+NO()⟶Ag()+NO₃−()(acidic solution)Ag+(aq)+NO(g)⟶Ag(s)+NO₃−(aq)(acidic solution)

(c) SiO₃²^−()+Mg()⟶Si()+Mg(OH)²()(basic solution)SiO₃²^−(aq)⁺Mg(s)⟶Si(s)+Mg(OH)₂(s)(basic solution)

(d) ClO³^−()+MnO₂()⟶Cl−()+MnO⁴^−()(basic solution)ClO³^−(aq)+MnO₂(s)⟶Cl−(aq)+MnO₄−(aq)(basic solution)

Answer 1

(a) 2Al(s) + 3Zr⁴⁺(aq) → 2Al³⁺(aq) + 3Zr(s)

(b) 3Ag⁺(aq) + NO(g) → 3Ag(s) + NO₃⁻(aq) (acidic solution)

(c) SiO₃²⁻(aq) + 3Mg(s) → Si(s) + 3Mg(OH)₂(s) (basic solution)

(d) 6ClO₃⁻(aq) + 2MnO₂(s) → 6Cl⁻(aq) + 2MnO₄⁻(aq) (basic solution)

Step-by-step explanation:

(a) The balanced reaction is 2Al(s) + 3Zr⁴⁺(aq) → 2Al³⁺(aq) + 3Zr(s). In a galvanic cell, the anode is where oxidation occurs, so 2Al(s) undergoes oxidation to 2Al³⁺(aq), while 3Zr⁴⁺(aq) is reduced to 3Zr(s) at the cathode.

(b) The balanced reaction is 3Ag⁺(aq) + NO(g) → 3Ag(s) + NO₃⁻(aq) (acidic solution). In a galvanic cell under acidic conditions, the half-reaction at the anode is 3Ag⁺(aq) being oxidized to 3Ag(s), and at the cathode, NO(g) is reduced to NO₃⁻(aq).

(c) The balanced reaction is SiO₃²⁻(aq) + 3Mg(s) → Si(s) + 3Mg(OH)₂(s) (basic solution). In a galvanic cell under basic conditions, SiO₃²⁻(aq) is oxidized at the anode, producing Si(s), and 3Mg(s) undergoes reduction to 3Mg(OH)₂(s) at the cathode.

(d) The balanced reaction is 6ClO₃⁻(aq) + 2MnO₂(s) → 6Cl⁻(aq) + 2MnO₄⁻(aq) (basic solution). In a galvanic cell under basic conditions, 6ClO₃⁻(aq) is oxidized at the anode to 6Cl⁻(aq), and 2MnO₂(s) undergoes reduction to 2MnO₄⁻(aq) at the cathode