A gas deviates maximum from the ideal gas laws at

Options

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

Answer

To determine the conditions under which a gas deviates the most from the ideal gas laws, we need to analyze the behavior of real gases compared to ideal gases.

### Step-by-Step Solution:

1. **Understand the Ideal Gas Law**: The ideal gas law is given by the equation \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the universal gas constant, and \( T \) is the temperature. Ideal gases follow this equation perfectly under certain conditions.

**Hint**: Remember that the ideal gas law assumes no intermolecular forces and that gas particles occupy no volume.

2. **Conditions for Ideal Behavior**: Real gases behave ideally at high temperatures and low pressures. Under these conditions, the volume of the gas particles is negligible compared to the total volume, and intermolecular forces are minimal.

**Hint**: Think about how increasing temperature increases kinetic energy and reduces the effect of intermolecular forces.

3. **Conditions for Maximum Deviation**: Conversely, a gas deviates the most from ideal behavior under conditions of low temperature and high pressure. At low temperatures, the kinetic energy of gas molecules decreases, and they are more likely to be influenced by intermolecular forces. At high pressures, the volume of gas particles becomes significant compared to the total volume, and again, intermolecular forces play a larger role.

**Hint**: Consider what happens to gas molecules when they are close together (high pressure) and moving slowly (low temperature).

4. **Conclusion**: Therefore, the conditions under which a gas deviates maximally from the ideal gas laws are low temperature and high pressure.

**Final Answer**: The correct option is **low temperature and high pressure**.