Reaction 1 Cu+NO → Cu2++ NO Reaction 2 MnO4 + H2S → Mn2+ + S Reaction 3 AS2O3 + NO3 → H3ASO4 + N2O3

The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced REDUCTION half reaction. Cl- + H3AsO4  HAsO2 + ClO3-

Al(s) + KOH(aq) → KAI(OH)₄(aq) + H₂(g) How is the redox balanced step by step?

The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced OXIDATION half reaction. S2O32- + Bi(OH)3Bi + SO32-       Reactants   Products

The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. Al3+ + NiAl + Ni2+       Reactants -> Products

The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′ where n is the number of electrons transferred, F is Faraday's constant, 96.5 kJ·mol−1·V−1, and ΔE∘′ is the difference in reduction potential. For each of the given reactions, determine the number of electrons transferred (n) and calculate standard free energy (ΔG∘′) . Consider the half-reactions and overall reaction for reaction 1. half-reactions: fumarate^2− + 2H^+ ↽−−⇀ succinate^2− CoQH2 ↽−−⇀ CoQ + 2H^+   overall reaction: fumarate^2− + CoQH2↽−−⇀succinate^2− + CoQ ΔE∘′= −0.009 V   n=____ ΔG∘′= ____ (kJ⋅mol^−1) Consider the half-reactions and overall reaction for reaction 2. half-reactions: cytochrome (c1) (Fe^2+) ↽−−⇀ cytochrome (c1) (Fe^3+) cytochrome (c) (Fe^3+) ↽−−⇀ cytochrome (c) (Fe^2+)   overall reaction: cyt (c1) (Fe^2+)+cyt (c) (Fe^3+)↽−−⇀cyt (c1) (Fe^3+)+cyt (c) (Fe^2+) ΔE∘′=0.034 V n= ____ ΔG∘′=____(kJ⋅mol^−1)

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.

The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction. BrO3 + Cl¯→→→Br¯ + CIO3¯ Reactants Enter electrons as e. Products

The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.