A real gas behaves like an ideal gas if its

Options

A. both pressure and temperature are high
B. both pressure and temperature are low
C. pressure is high and temperature is low
D. pressure is low and temperature is high

Explanation

To determine under what conditions a real gas behaves like an ideal gas, we need to consider the fundamental assumptions of the ideal gas law and the behavior of real gases.

### Step-by-Step Solution:

1. **Understanding Ideal Gas Behavior**:
- Ideal gases are defined by certain assumptions: they have no intermolecular forces, and the volume of the gas particles is negligible compared to the volume of the container. This means that the gas molecules are far apart from each other.

2. **Conditions for Real Gases**:
- Real gases deviate from ideal behavior under certain conditions, particularly at high pressures and low temperatures. At high pressures, gas molecules are forced closer together, and intermolecular forces become significant. At low temperatures, the kinetic energy of the molecules decreases, allowing these forces to have a more pronounced effect.

3. **High Temperature and Low Pressure**:
- A real gas behaves more like an ideal gas when the temperature is high and the pressure is low. At high temperatures, the kinetic energy of the gas molecules is high, which means they move rapidly and can overcome intermolecular forces. At low pressures, the molecules are farther apart, reducing the impact of these forces.

4. **Conclusion**:
- Therefore, a real gas behaves like an ideal gas when both the pressure is low and the temperature is high. This allows the assumptions of the ideal gas law to hold true, as the effects of intermolecular forces become negligible.

### Final Answer:
A real gas behaves like an ideal gas if its **pressure is low and temperature is high**.

---