indicate whether or not it is a redox reaction. If it is, indicate which atom is being oxidized, which atom is being reduced, what the oxidizing agent is, and what the reducing agent is.

Question

a. CO2 + H2 > CO + H2O

b. 3Cu + 2HNO3 + 6H+ > 3Cu2+ + 2NO + 4H2O

c. Zn + 2MnO2 > ZnO + Mn2O3

d. FeCI3 + 3NaOH > Fe(OH)3 + 3NaCI

e. 2Fe + 3 V2O3 > Fe2O3 + 6VO

Answer 1

In terms of electrons remember OIL RIG.

Oxidation is Loss (is the reducing agent),

Reduction is Gain (is the oxidizing agent)

Charge balance in each reaction is determined from oxidation state and stoichiometry

a)

C(⁺⁴) + O(^-2)*2 + H(⁰)*2 = C(⁺²) + O(^-2) + H(⁺¹)*2 + O(^-2)

Carbon's oxidation number is reduced from +4 to +2 (gaining two electrons, oxidizing agent)

Hydrogen's oxidation number is increased from 0 to +1 (losing 1 electron, reducing agent)

b)

Cu(⁰) + 2[H(⁺¹) + N(⁺⁵)O(^-2)*3] + 6[H(⁺)] = 3[Cu(⁺²)]+ 2[N(⁺²) + O(^-2)] + 4[H(⁺¹)*2 + O(^-2)]

Copper's oxidation number is increased from 0 to +3 (losing 3 electrons, reducing agent)

Nitrogen's oxidation number is reduced from +5 to +2 (gaining 3 electrons, oxidizing agent)

c)

Zn(0) + 2[Mn(⁺⁴) + O(^-2)*2] = Zn(⁺²) + O(^-2) + Mn(⁺³)*2 + O(^-2)*3

Zinc's oxidation number is increased from 0 to +2 (losing 2 electrons, reducing agent)

Manganese's oxidation number is reduced from +4 to +3 (it gains 1 electron, oxidizing agent)

d)

Fe(⁺³) + CI(^-1)*3 + 3[Na(⁺¹) + O(^-2) + H(⁺¹) = Fe(⁺³) + 3[O(^-2) + H(⁺¹)] + 3[Na(⁺¹) + CI(^-1)

Not a red-ox reaction.

e)

2[Fe(⁰)]+ 3[V(⁺³)*2 + O(^-2)*3] = Fe(⁺³)*2 + O(^-2)*3 + 6[V(⁺²) + O(^-2)]

Iron's oxidation number is increased from 0 to +3 (losing 3 electrons, reducing ageng)

Vanadium's oxidation number is reduced from +3 to +2 (gaining 1 electron, oxidizing agent)