When there can be more deviation in the behaviour of a gas from the ideal gas equation PV = nRT

Options

A. At hight temperature and low pressure
B. At low temperature and high pressure
C. At high temperature and high pressure
D. At low tmeperature and lwo pressure

Answer

**Step-by-Step Solution:**

1. **Understanding Ideal Gas Behavior**: The ideal gas equation is given by PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Ideal gases are hypothetical gases that perfectly follow this equation under all conditions.

2. **Conditions for Deviation**: Real gases deviate from ideal behavior under certain conditions. The deviations are more pronounced at high pressures and low temperatures.

3. **High Pressure**: At high pressures, gas molecules are forced closer together. The volume occupied by the gas molecules themselves becomes significant compared to the volume of the container. This results in a deviation from the ideal gas behavior because the ideal gas law assumes that gas molecules have no volume.

4. **Low Temperature**: At low temperatures, gas molecules have lower kinetic energy, which means they move slower. This can lead to increased intermolecular forces (such as van der Waals forces) becoming significant, causing the gas to deviate from ideal behavior. The ideal gas law assumes no intermolecular attractions, which is not the case at low temperatures.

5. **Conclusion**: Therefore, the behavior of a gas deviates more from the ideal gas equation (PV = nRT) at high pressures and low temperatures.

**Final Answer**: The gas will deviate more from the ideal gas equation at high pressure and low temperature.

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