1 mole of each of `X_(1),X_(2),X_(3)` with van der Waal's constants a (in atm `L^(3) mol^(-2)`) 1.0, 3.8, 2.1 respectively is kept separately in three different vessels of equal volume at identical temperature. Their pressures are observed to `P_(1),P_(2),` and `P_(3)` respectively. On the basis of this data alone, select the correct option (neglect the effect of 'b') :
0.1 M NaCl and 0.1 M CH_(3)COOH are kept in separate containers. If their osmotic pressures are P_(1) and P_(2) respectively then what is the correct statement ?
The values of the van der Waals constants for a gas a = 4.10 dm^(6) "bar" mol^(-2) and b = 0.035 dm^(3) mol^(-1) . Calculate the values of the critical temperature and critical pressure for the gas.
If three unrective gases having partial pressures P P_(B) and P_(C) and theire moles are 1,2 and 3 respectively then their total pressure will be
The van der Waal's constants for a gas are a=1.92 atm L^(2) "mol"^(-2),b=0.06 L "mol"^(-1) . If R = 0.08 L atm K^(-1) "mol"^(-1) , what is the Boyle's temperature (in K) of this gas ?
If three unreactive gases having partial pressures , P_(A) , P_(B) and P_(C) and their moles are 1 , 2 and 3 respectively then their total pressure will be
The van der Waal's constants a & b of CO_(2) are 3.64 L^(2) mol^(-2) bar & 0.04 L mol^(-1) respectively. The value of R is 0.083 bar dm^(3)mol^(-1)K^(-1) . If one mole of CO_(2) is confined to a volume of 0.15L at 300 K , then the pressure (in bar) eaxerted by the gas is :
For one mole of any van der Waal's gas a =0.27 atm- "litre"^(2)//"mol"^(2) and b=1.218 cm^(3)//"mol" . Select the correct statement(s).
