A gas described by van der Waals equation
(A) behaves similar to an ideal gas in the limit of large molar volumes
(B) behaves similar to an ideal gas in the limit of large pressures
(C) is characterised by van der Waals coefficients that are dependent on the identity of the gas but are independent of the temperature
(D) has the pressure that is lower than the pressure exerted by the same gas behaving ideally
(A) behaves similar to an ideal gas in the limit of large molar volumes
(B) behaves similar to an ideal gas in the limit of large pressures
(C) is characterised by van der Waals coefficients that are dependent on the identity of the gas but are independent of the temperature
(D) has the pressure that is lower than the pressure exerted by the same gas behaving ideally
- (A)behaves similar to an ideal gas in the limit of large molar volumes✓ Correct
- (B)behaves similar to an ideal gas in the limit of large pressures
- (C)is characterised by van der Waals coefficients that are dependent on the identity of the gas but are independent of the temperature✓ Correct
- (D)has the pressure that is lower than the pressure exerted by the same gas behaving ideally✓ Correct
Answer: (A), (C), (D)
Solution
The van der Waals equation is:
(A) True: At large molar volumes (low pressure), molecules are far apart, intermolecular forces become negligible, and the gas behaves ideally.
(B) False: At high pressures (small volumes), deviations from ideal behavior are significant.
(C) True: The van der Waals constants and are characteristic of each gas and are independent of temperature.
(D) True: The term represents the pressure correction due to intermolecular attractions. The actual pressure is lower than the ideal pressure by this amount.
(A) True: At large molar volumes (low pressure), molecules are far apart, intermolecular forces become negligible, and the gas behaves ideally.
(B) False: At high pressures (small volumes), deviations from ideal behavior are significant.
(C) True: The van der Waals constants and are characteristic of each gas and are independent of temperature.
(D) True: The term represents the pressure correction due to intermolecular attractions. The actual pressure is lower than the ideal pressure by this amount.
JEE Advanced · 2008 · 13 Apr 2008 · Paper 1 · One or more correct options