Two samples of lead oxide were separately reduced to metallic lead by heating in a current of hydrogen. The weight of lead from one oxide was half the weight of lead obtained from the other oxide. The data illustrates

Options

A. law of reciprocal proportions
B. law of constant proportions
C. law of multiple proportions
D. law of equivalent proportions.

Explanation

To solve the problem, we need to analyze the information given about the two samples of lead oxide and the resulting lead obtained from their reduction.

### Step-by-Step Solution:

1. **Understanding the Problem**:
- We have two samples of lead oxide (let's call them Sample 1 and Sample 2).
- When reduced by heating in hydrogen, Sample 1 yields a certain amount of lead (let's denote it as \( x \) grams).
- Sample 2 yields twice that amount, which is \( 2x \) grams of lead.

2. **Identifying the Chemical Reaction**:
- The reduction of lead oxide (PbO or PbO₂) to lead (Pb) involves the removal of oxygen.
- Sample 1 could be lead(II) oxide (PbO), and Sample 2 could be lead(IV) oxide (PbO₂).

3. **Applying the Law of Multiple Proportions**:
- According to the law of multiple proportions, when two elements (like lead and oxygen) form different compounds, the masses of one element that combine with a fixed mass of the other element are in a simple ratio.
- In this case, if we consider the two oxides:
- For PbO: 1 part of Pb combines with 1 part of O.
- For PbO₂: 1 part of Pb combines with 2 parts of O.
- The ratio of lead obtained from these two compounds (when fixed with respect to oxygen) shows that the mass of lead from PbO is half that from PbO₂.

4. **Conclusion**:
- Since the mass of lead from one oxide is half that from the other, this illustrates the law of multiple proportions.
- Therefore, the correct answer is **Option C: Law of Multiple Proportions**.