Real gases do not follow I.Boyle's law II. Charles's law II.Avogadro law identify the correct option

Options

A. I and II
B. II and III
C. I and II
D. all of the above

Answer

To solve the question regarding the behavior of real gases in relation to Boyle's law, Charles's law, and Avogadro's law, we can follow these steps:

### Step 1: Understand the Laws
- **Boyle's Law** states that for a given mass of gas at constant temperature, the volume (V) of the gas is inversely proportional to the pressure (P). Mathematically, it can be expressed as \( PV = k \) (where k is a constant).

- **Charles's Law** states that the volume of a gas is directly proportional to its absolute temperature (T) when pressure is held constant. This can be expressed as \( \frac{V}{T} = k \).

- **Avogadro's Law** states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules. This can be expressed as \( V \propto n \) (where n is the number of moles).

### Step 2: Identify the Characteristics of Real Gases
- Real gases do not perfectly adhere to these laws due to intermolecular forces and the volume occupied by gas molecules. These deviations become significant at high pressures and low temperatures.

### Step 3: Analyze the Options
- The question asks whether real gases follow Boyle's law, Charles's law, and Avogadro's law. Since real gases deviate from these ideal behaviors, we conclude that:

1. Real gases do not follow Boyle's law.
2. Real gases do not follow Charles's law.
3. Real gases do not follow Avogadro's law.

### Step 4: Conclusion
- Since real gases do not follow any of the three laws mentioned, the correct option is **all of the above**. Therefore, the answer is **option D**.

### Final Answer
The correct option is **D: all of the above**.

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