Element X forms five stable oxides with oxygen of formula `X_(2) O, XO , X_(2) O_(3) , X_(2) O_(5)` . The formation of these oxides explains

Options

A. Law of definite proportions
B. Law of partial pressures
C. Law of multiple proportions
D. Law of reciprocal proportions

Answer

To solve the problem, we need to analyze the information given about the element X and its oxides.

### Step-by-Step Solution:

1. **Identify the Oxides**: The oxides of element X are given as:
- \( X_2O \)
- \( XO \)
- \( X_2O_3 \)
- \( X_2O_5 \)

2. **Understanding the Composition**:
- In these oxides, the number of oxygen atoms varies while the number of atoms of X in each oxide is fixed in a certain ratio.
- For instance, in \( X_2O \), there are 2 atoms of X for every 1 atom of oxygen.
- In \( XO \), there is 1 atom of X for every 1 atom of oxygen.
- In \( X_2O_3 \), there are 2 atoms of X for every 3 atoms of oxygen.
- In \( X_2O_5 \), there are 2 atoms of X for every 5 atoms of oxygen.

3. **Law of Multiple Proportions**:
- The key concept here is that when two elements combine to form more than one compound, the ratios of the masses of the second element that combine with a fixed mass of the first element can be expressed in small whole numbers.
- In this case, the mass of element X remains constant while the mass of oxygen varies in different oxides.

4. **Conclusion**:
- Since we observe that a fixed amount of element X combines with varying amounts of oxygen to form different stable oxides, this scenario illustrates the **Law of Multiple Proportions**.

### Final Answer:
The formation of these oxides explains the **Law of Multiple Proportions**.

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