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2 mol of a van der waals gas at 27^(@)C ...

2 mol of a van der waals gas at `27^(@)C` occupies a volume of 20 L. what is the pressure of the gas? [a=6.5 `atm*L^(-2)*mol^(-2),b=0.056L*mol^(-1)`]

Text Solution

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van der waals equation for 'n' mol of a real gas:
`(P+(n^(2)a)/(V^(2)))(V-nb)=nRT`
Given, `n=2mol,V=20L,T=(273+27)=300K`,
`a=6.5 atm*L^(-2)*mol^(-2) and b=0.056L*mol^(-1)`
`thereforeP=(nRT)/(V-nb)-(n^(2)a)/(V^(2))=(2xx0.0821xx300)/((20-1xx0.056))-((2)^(2)xx6.5)/((20)^(2))`
`=(2.477-0.065)atm=2.412atm`
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