For each of the following balanced oxidation-reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. 1. Identify the oxidation numbers for all the elements in the reactants and products for I2O5 (s) + 5CO (g) ? I2 (s) + 5CO2 (g) 2. Identify the oxidation numbers for all the elements in the reactants and products for 2Hg2 + (aq) + N2H4 (aq) ?2Hg (l) + N2 (g) + 4H + (aq) 3. Identify the oxidation numbers for all the elements in the reactants and products for 3H2S (aq) + 2H + (aq) + 2NO?3 (aq) ?3S (s) + 2NO (g) + 4H2O (l)

1. 10 e⁻

Oxidation numbers

I₂O₅ (s) : I (5+); O (2-)

CO (g) : C (2+); O (2-)

I₂ (s) : I (0)

CO₂ (g) : C (4+); O (2-)

2. 4 e⁻

Oxidation numbers

Hg²⁺ (aq) : Hg (2+)

N₂H₄ (aq) : N (2-); H (1+)

Hg (l) : Hg (0)

N₂ (g) : N (0)

H⁺ (aq) : H (1+)

3. 6 e⁻

Oxidation numbers

H₂S (aq) : H (1+); S (2-)

H⁺ (aq) : H (1+)

NO₃⁻ (aq) : N (5+); O (2-)

S (s) : S (0)

NO (g) : N (2+); O (2-)

H₂O (l) : H (1+); O (2-)

Explanation:

In order to state the total number of electrons transferred we have to identify both half-reactions for each redox reaction.

1. I₂O₅ (s) + 5 CO (g) → I₂ (s) + 5 CO₂ (g)

Oxidation: 10 e⁻ + 10 H⁺ (aq) + I₂O₅ (s) → I₂ (s) + 5 H₂O (l)

Reduction: 5 H₂O (l) + 5 CO (g) → 5 CO₂ (g) + 10 H⁺ (aq) + 10 e⁻

2. 2 Hg²⁺ (aq) + N₂H₄ (aq) → 2 Hg (l) + N₂ (g) + 4 H⁺ (aq)

Oxidation: N₂H₄ (aq) → N₂ (g) + 4 H⁺ (aq) + 4 e⁻

Reduction: 2 Hg²⁺ (aq) + 4 e⁻ → 2 Hg (l)

3. 3 H₂S (aq) + 2H⁺ (aq) + 2 NO₃⁻ (aq) → 3 S (s) + 2 NO (g) + 4H₂O (l)

Oxidation: 3 H₂S (aq) → 3 S (s) + 6 H⁺ (aq) + 6 e⁻

Reduction: 8 H⁺ (aq) + 2 NO₃⁻ (aq) + 6 e⁻ → 2 NO (g) + 4 H₂O