Calculate the temperature of the gas if it obeys van der Waal's equation from the following data. A flask of 2.5 litre contains 10 mole of a gas under 50 atm. Given `a = 5.46 atm "litre"^(2) mol^(-2) " and " b = 0.031 " litre " mol^(-1)`

Explanation

Given that,
`P = 50 atm, V = 2.5 " litre ", n = 10, a = 5.46 atm "litre"^(2) mol^(-2), b = 0.031 " litre " mol^(-1) , R - 0.0821 "litre" - atm K^(-1) mol^(-1)`
Applying van der Waal's equation
`(P + (an^(2))/(V^(2))) (V - nb) = nRT`
or `T ((P + (an^(2))/(V^(2)) (V - nb)))/(nR)`
`= (((50 + (5.46 xx 100))/((2.5)^(2)))(2.5 - 10 xx 0.031))/(10 xx 0.0821) = 366.4 K`