Why do real gases deviate from Boyle's law?

Explanation

**Step-by-Step Solution:**

1. **Understanding Boyle's Law**: Boyle's law states that for a given mass of an ideal gas at constant temperature, the volume of the gas is inversely proportional to its pressure. Mathematically, this can be expressed as \( PV = k \), where \( P \) is the pressure, \( V \) is the volume, and \( k \) is a constant.

2. **Ideal vs. Real Gases**: Ideal gases are hypothetical gases that perfectly follow Boyle's law under all conditions. They are characterized by the absence of intermolecular forces and occupy no volume. Real gases, on the other hand, do not perfectly follow Boyle's law due to the presence of intermolecular forces and the finite volume of gas particles.

3. **Intermolecular Forces**: In real gases, there are attractive and repulsive forces between gas molecules. These intermolecular forces can affect the behavior of the gas, especially at high pressures and low temperatures. At high pressures, the volume of the gas is reduced, and the molecules are closer together, leading to stronger intermolecular attractions.

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