Van der Waals' real gas, acts as an ideal gas at which condition?
Van der Waals' real gas, acts as an ideal gas at which condition?
The correct option is A High temperature, low pressure
Ideal gases are gases that have elastic collisions between their molecules and there are no intermolecular attractive forces. In reality, there is no such thing as ideal gases. The gases just show ideal behavior under certain conditions of temperature and pressure.
Formula used:
PV=nRT
where P is pressure, V is volume, R is the universal gas constant, n is no. of moles and T is temperature.
Gases behave very ideally at high temperature and low pressure. High temperature means the molecules are moving around faster and have less chance of sticking together. Lower pressure means that the molecules are far apart from each other and won't interact as much.
Thus, At higher temperatures and low-pressure real gas acts as an ideal gas and obeys the pV=nRT relation.
The correct option is A High temperature, low pressure
Ideal gases are gases that have elastic collisions between their molecules and there are no intermolecular attractive forces. In reality, there is no such thing as ideal gases. The gases just show ideal behavior under certain conditions of temperature and pressure.
Formula used:
PV=nRT
where P is pressure, V is volume, R is the universal gas constant, n is no. of moles and T is temperature.
Gases behave very ideally at high temperature and low pressure. High temperature means the molecules are moving around faster and have less chance of sticking together. Lower pressure means that the molecules are far apart from each other and won't interact as much.
Thus, At higher temperatures and low-pressure real gas acts as an ideal gas and obeys the pV=nRT relation.
