1 mole of a ciatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm `L^(2)//mol^(2)`).
The compressibility factor for definite amount of van der Waals' gas at 0^(@)C and 100 atm is found to be 0.5 . Assuming the volume of gas molecules negligible, the van der Waals' constant a for gas is
The pressure exerted by 1 mol of CO_(2) at 273 K is 34.98 atm . Assuming that volume occupied by CO_(2) molecules is negligible, the value of van der Waals constant for attraction of CO_(2) gas is
The compression factor (compressibility factor) for 1 mol of a van der Waals gas at 0^(@)C and 100 atm pressure is found to be 0.5 . Assuming that the volume of a gas molecule is neligible, calculate the van der Waals constant a .
The compression factor (compressibility factor) for 1 mol of a van der Waals gas at 0^(@)C and 100 atm pressure is found to be 0.5 . Assuming that the volume of a gas molecule is neligible, calculate the van der Waals constant a .
One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:
A sample of an ideal gas occupies 20 L under a pressure of "0.5" atm and under isothermal condition.On increasing its pressure to 1.0 atm. Its volume will be
