A gas that follows Boyle's law, Charle's law and Avogadro's law is called an ideal gas. Under what conditions a real gas would behave ideally ?

Options

A. Under low pressure and temperature
B. Under high pressure and temperature
C. Under high pressure and low temperature
D. Under low pressure and high temperature

Answer

To determine the conditions under which a real gas behaves ideally, we can follow these steps:

### Step 1: Understand Ideal Gas Behavior
An ideal gas is one that perfectly follows Boyle's law, Charles's law, and Avogadro's law. This means that the gas particles do not exert any intermolecular forces on each other and occupy no volume.

### Step 2: Identify Conditions for Real Gases
Real gases deviate from ideal behavior due to intermolecular forces and the volume occupied by gas particles. To behave ideally, these deviations must be minimized.

### Step 3: Minimize Intermolecular Forces
Intermolecular forces are minimized when:
- The temperature is high: At higher temperatures, gas particles have more kinetic energy, which allows them to overcome attractive forces between them.
- The pressure is low: At lower pressures, gas particles are farther apart, reducing the effect of intermolecular forces.

### Step 4: Negligible Volume of Gas Particles
The volume of gas particles becomes negligible compared to the volume of the container when:
- The gas is at low pressure: This allows the gas particles to spread out more, making their individual volumes insignificant relative to the total volume of the container.

### Step 5: Conclusion
Thus, a real gas behaves ideally under the following conditions:
- **High temperature** (to minimize intermolecular attractions)
- **Low pressure** (to ensure the volume of gas particles is negligible)

### Final Answer
A real gas would behave ideally under conditions of **low pressure and high temperature**.

---