Question

Below is a set of redox reactions. Assign oxidation numbers below each atom. Also determine the substance that is reduced, the substance that is oxidized, the oxidizing agent, and the reducing agent. (Note: Don’t worry about the stoichiometric coefficients; they don’t affect your calculation of oxidation states.)

Atom/s that is/are reduced:

Atom/s that is/are oxidized:

Reducing agent:

Oxidizing agent:

Reactions Given:

2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

C2H4(g) + 3O2(g) → 2 CO2(g) + 2 H2O(g)

2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g)

2 C2H6O(g) + 2 O2(g) → 2 CO(g) + 3 H2O(g)

2 Cr(s) + 3 Ni(aq) 2+ → 2 Cr(aq) 3+ + 3 Ni(aq)

2 Ca(s) + O2(g) → 2 CaO(s)

N2(g) + 3 H2(g) → 2 NH3(g)

2 NO(g) → N2(g) + O2(g)

Cl2(g) + 2 KI(aq) → 2 KCl(aq) + I2(s)

3 HNO2(aq) → HNO3(aq) + H2O(l) + 2 NO(g)

3 ClO(aq) − + 2 Fe(s) → Fe2O3(s) + 3 Cl(aq)

Answer 1