Two moles of real gas confined in a 5 L flask exerts pressure 9.1 atm at a temperature of 27 °C. Calculate the value of 'a' given the value of 'b' is 0.052 L ​mol⁻¹

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Please find the solution to the asked query:

$$\begin{gathered} Volume =5L \\ Pressure =9.1 atm \\ Temperature ={27}^{o}C =300K \\ b =0.052L /mol \\ n =2 \\ Vander waal equation for n mole of gas \\ [p +\frac{a{n}^2}{v^2}][v-nb] =nRT \\ [9.1 +\frac{4.a}{5^2}][5-2\times 0.052] = 2\times 300\times 0.0821 \\ [9.1+\frac{4a}{25}][4.896] =49.26 \\ 44.5 +0.78a =49.26 \\ 0.78a =4.76 \\ a=6.10 atm litr{e}^{2}mo{l}^{-1} \end{gathered}$$


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