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 provided formulas: \(X_2O\), \(XO\), \(X_2O_3\), and \(X_2O_5\).

### Step-by-Step Solution:

1. **Identify the Oxide Formulas**:
- The oxides given are \(X_2O\), \(XO\), \(X_2O_3\), and \(X_2O_5\).

2. **Determine the Ratios of X to O**:
- For \(X_2O\): The ratio of X to O is \(2:1\).
- For \(XO\): The ratio of X to O is \(1:1\).
- For \(X_2O_3\): The ratio of X to O is \(2:3\).
- For \(X_2O_5\): The ratio of X to O is \(2:5\).

3. **Analyze the Ratios**:
- The ratios of X to O in these oxides are \(2:1\), \(1:1\), \(2:3\), and \(2:5\).
- Notice that the ratios of the amounts of oxygen in the oxides are in simple whole number ratios.

4. **Apply the Law of Multiple Proportions**:
- According to the law of multiple proportions, 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 a ratio of small whole numbers.
- Here, the different oxides of element X with oxygen demonstrate that the ratios of the number of oxygen atoms can be expressed as simple whole numbers.

5. **Conclusion**:
- The formation of these oxides explains the law of multiple proportions, as the ratios of the oxides formed by element X with oxygen are consistent with this law.

### Final Answer:
The formation of these oxides explains the **law of multiple proportions**.

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