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2 mol of gas is kept in a 4 litre flask....

2 mol of gas is kept in a 4 litre flask. The pressure of the gas at 300 K is 11 atm. If the value of 'b' for the gas is 0.05 `L*mol^(-1)`, then determine the value of 'a' by using van der waals equation.

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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, P=11 atm, V=4 L, T=300K, n=2 mol,
b=0.05 `L*mol^(-1)`
`therefore [11+((2)^(2)xxa)/(4)](4-2xx0.05]=2xx0.0821xx300`
or, `(11+0.25xa)(3.9)=49.26 or, 11+0.25xxa=12.63`
`thereforea=6.52L^(2)*atm*mol^(-2)`.
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