Balance the following oxidation–reduction equation. The reactions occur in a basic aqueous solution. Cd2++ H 2S → Cd...

Balance the following oxidation–reduction equation. The reactions occur in a basic aqueous solution.

Cd²⁺+ H ₂S → Cd + S ₈

S^2- + F₂ → SO₄^2- + F^-

Cr + NO₃^- → Cr(OH)₄^- + NH₃

MnO₄^- + C₂O₄²^- → MnO₂ + CO₂

Expert Solution

Solution :-

The redox reactions are balanced in the basic solution by adding the OH- ions at the final steps of the balancing.

Following image shows the balancing steps and final balanced equation for the each reaction

queen_honey_blossom answered 8 months ago

#18.37 Balance each of the following redox reactions occurring in acidic aqueous solution. A) Cd(s)+Cu+(aq)→Cd2+(aq)+Cu(s) B)...

#18.37 Balance each of the following redox reactions occurring in acidic aqueous solution. A) Cd(s)+Cu+(aq)→Cd2+(aq)+Cu(s) B) I−(aq)+SO42−(aq)→H2SO3(aq)+I2(s)

Balance the following redox reaction in a BASIC environment: ClO4- + Cd(s) --> Cl- + Cd2+

In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing...

In an acid solution using the half-reaction method balance the following oxidation/reduction reactions. Identify the oxidizing agent and the reducing agent in each reaction. a. ??(?) + ??3 - (??) → ??2+ (??) + ??(?) b. ??2?72-(??) + ??-(??) → ??3+(??) + ??2 (?) c. ??22+(??) + ??(?) → ?4+(??) + ???42- d. ??2 (??) → ???3-(??) + ??-(??)

Why must the charge balance in oxidation-reduction reactions?

4. Balance the following redox reactions that occur in basic solution using the half-reaction method. a....

4. Balance the following redox reactions that occur in basic solution using the half-reaction method. a. PO33-(aq) + MnO4-(aq) → PO43-(aq) + MnO2(s) b. Mg(s) + OCl-(aq) → Mg(OH)2(s) + Cl-(aq) c. H2CO(aq) + Ag(NH3)2+(aq) → HCO3-(aq) + Ag(s) + NH3(aq)

Balance the followinh equation for the oxidation-reduction reaction occurring in an acidic solution, shoe all work,...

Balance the followinh equation for the oxidation-reduction reaction occurring in an acidic solution, shoe all work, steps. IO3- + N2H4 -> I- + N2

Balance each of the following half-reactions, assuming that they occur in basic solution. CH3OH(aq)?CH2O(aq)

Balance the following reactions in basic solution. a) Zr(OH)2(s) + O2(g) → ZrO2(s) Oxidation reaction =...

Balance the following reactions in basic solution. a) Zr(OH)2(s) + O2(g) → ZrO2(s) Oxidation reaction = Reduction reaction = Net reaction = b) S2O32−(aq) + Cu(OH)2(s) → SO32−(aq) + CuOH(s) Oxidation reaction = Reduction reaction = Net reaction = c) Ti(s) + CrO42−(aq) → Ti(OH)3(s) + Cr(OH)4−(aq) Oxidation reaction = Reduciton reaction = Net reaction = d) NO2−(aq) + H2(g) → NO(g) Oxidation reaction = Reduciton reaction = Net reaction =

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and...

Balance the following redox reactions. Show the complete balanced reduction half and oxidation half reaction, and label each accordingly. Give the complete balanced reaction. A.) CN-1 + MnO4-2 ---> CNO-1 + MnO2 B.) S2O3-2 + IO2-1 ---> I- + S4O6-2

Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing...

Use the half reaction method to balance each of the following oxidation-reduction reactions. Identify the oxidizing agent and the reducing agent. A) Cu(s) + Ag+(aq) ---> Ag(s) + Cu2+ B) Al(s) + I2(s) ---> AlI3(s) C) Pb(s) + Fe3+(aq) ----> Pb2+(aq) + Fe(s)

Question