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Van der Waal's Forces

Using van der...

Question

Using van der Waals' equation, calculate the constant $^{'} a^{'}$ when two moles of a gas confined in a four litre flask exerts a pressure of $11 a t m$ at a temperature of $300 K$ . The value of $^{'} b^{'}$ is $0.05 l i t r e m o l^{- 1}$

6.46 a t m l i t r e^{2} m o l^{- 2}

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5.46 a t m l i t r e^{2} m o l^{- 2}

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6.64 a t m l i t r e^{2} m o l^{- 2}

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5.64 a t m l i t r e^{2} m o l^{- 2}

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Solution

The correct option is B $6.46 a t m l i t r e^{2} m o l^{- 2}$
Vander waal's equation for $n$ moles of gas is, $[P + a \frac{n^{2}}{v^{2}}] [v - n b] = n R T .$
Given, $v = 4 L, P = 11 a t m, T = 300 K, b = 0.05 l i t r e / m o l$
$n = 2$
Thus , $[11 + a \frac{2^{2}}{4^{2}}] [4 - 2 (0.05)] = 2 \times 0.082 \times 300$
$a = 6.46 a t m {l i t r e}^{2} {m o l}^{- 2}$

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Similar questions

^{'} a^{'}

^{'} b^{'}

{m o l}^{- 1}

a

- l i t r e

b

l i t r e m o l^{- 1}

a

a t m

L^{2} m o l^{- 2}

4 L

11.0

300 K

b

0.05 L m o l^{- 1}

(R = 0.082 a t m L / K m o l)

^{2}

^{- 2}

^{- 1}

^{'} a^{'}

a t m

L^{2} m o l^{- 2}

4 L

11.0

300 K

b

0.05 L m o l^{- 1}

(R = 0.082 a t m L / K m o l)

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