A real gas behaves like an ideal gas if its

Options

A. pressure and temperature are both high
B. pressure and temperature are both 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 characteristics of both types of gases.

### Step-by-Step Solution:

1. **Understanding Ideal Gas Behavior**:
- An ideal gas is defined by the following assumptions:
- The molecules do not attract or repel each other (no intermolecular forces).
- The volume of the gas molecules is negligible compared to the volume of the container.

2. **Conditions for Real Gases**:
- For a real gas to behave like an ideal gas, it must meet the conditions of negligible intermolecular forces and negligible molecular volume.
- These conditions are typically met under certain pressure and temperature conditions.

3. **Analyzing Pressure and Temperature**:
- **High Temperature**: At high temperatures, the kinetic energy of the gas molecules increases, which means that they move faster. This increased motion helps overcome any intermolecular forces that may be present, making them negligible.
- **Low Pressure**: At low pressures, the gas molecules are spread out over a larger volume. This means that the actual volume occupied by the gas molecules becomes negligible compared to the total volume of the gas, fulfilling the second condition.

4. **Conclusion**:
- Therefore, a real gas behaves like an ideal gas when the temperature is high and the pressure is low. This corresponds to the option: "pressure is low and temperature is high."

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