Given the lead acid battery reaction:
`2PbSO_(4)+2H_(2)OhArrPb+PbO_(2)+H_(2)SO_(4)`
Charege `rarr" "larr` Discharge
Which species is oxidized during battery discharge?

Options

A. `SO_(4)^(2-)`
B. `H_(2)O`
C. `Pb`
D. `PbO_(2)`

Answer

To determine which species is oxidized during the discharge of a lead-acid battery, we can follow these steps:

### Step 1: Write the Discharge Reaction
The discharge reaction of the lead-acid battery can be written as:
\[ \text{Pb} + \text{PbO}_2 + \text{H}_2\text{SO}_4 \rightarrow 2\text{PbSO}_4 + 2\text{H}_2\text{O} \]

### Step 2: Assign Oxidation States
Next, we need to assign oxidation states to all the elements in the reaction:
- In elemental lead (Pb), the oxidation state is 0.
- In lead oxide (PbO₂), the oxidation state of lead (Pb) is +4 (since O is -2 and there are two O atoms, the total contribution from O is -4, making Pb +4 to balance to 0).
- In sulfuric acid (H₂SO₄), hydrogen (H) has an oxidation state of +1 and sulfur (S) has an oxidation state of +6, while oxygen (O) has -2.
- In lead sulfate (PbSO₄), lead (Pb) has an oxidation state of +2 (to balance with SO₄²⁻ which has a -2 charge).

### Step 3: Compare Oxidation States
Now, we compare the oxidation states of lead in the reactants and products:
- Lead (Pb) changes from 0 (in the reactants) to +2 (in PbSO₄).
- Lead oxide (PbO₂) has lead at +4, but it is not being oxidized; it is acting as an oxidizing agent.

### Step 4: Identify Oxidation
Since oxidation is defined as the loss of electrons (or an increase in oxidation state), we see that:
- Lead (Pb) is oxidized because its oxidation state increases from 0 to +2.

### Conclusion
Thus, the species that is oxidized during the battery discharge is:
**Lead (Pb)**

### Final Answer
The correct answer is **Lead (Pb)**.

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