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 question regarding the formation of five stable oxides of element X with oxygen, we need to analyze the given formulas and determine which law of chemical combination they illustrate.

### Step-by-Step Solution:

1. **Identify the Oxides**: The oxides formed by element X are:
- XO
- X₂O
- X₂O₃
- X₂O₅

2. **Determine the Ratios of X to O**:
- For XO: 1 atom of X combines with 1 atom of O.
- For X₂O: 2 atoms of X combine with 1 atom of O.
- For X₂O₃: 2 atoms of X combine with 3 atoms of O.
- For X₂O₅: 2 atoms of X combine with 5 atoms of O.

3. **Analyze the Ratios**:
- In XO, the ratio of X to O is 1:1.
- In X₂O, the ratio is 2:1.
- In X₂O₃, the ratio is 2:3.
- In X₂O₅, the ratio is 2:5.

4. **Identify the Pattern**:
- The number of oxygen atoms in the compounds varies while the number of X atoms remains constant at 2 in the last three oxides (X₂O, X₂O₃, X₂O₅).
- The ratios of the oxygen atoms (1, 1, 3, 5) can be seen as multiples of the basic oxide XO.

5. **Apply the Law of Multiple Proportions**:
- The fact that when element X combines with oxygen, it can form different compounds (with different ratios of oxygen) indicates that these compounds are formed in simple whole number ratios.
- This is a classic example of the law of multiple proportions, which states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers.

### Conclusion:
The formation of these oxides by element X explains the **law of multiple proportions**.