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Standard XII

Chemistry

Real Gases

Calculate the...

Question

Calculate the pressure exerted by one mole of ${C O}_{2}$ gas at 273K, if the van der Waals constant a=3.592 ${d m}^{6} a t m {m o l}^{- 2}$ . Assume that the volume occupied by ${C O}_{2}$ molecules is negligible.

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Solution

According to van der Waals equation of state for 1 mole of as gas,
( P + $\frac{a}{V^{2}}$ ) (V-b) =0
Since, the volume occupied by $C O_{2}$ molecules is negligible, b =0
So,
( P + $\frac{a}{V^{2}}$ ) V = RT
or,
P = $\frac{R T}{V^{2}}$ - $\frac{a}{V^{2}}$

= $\frac{0.082 \times 273}{22.4}$ - $\frac{3.592}{(22.4)^{2}}$
= 0.999375 - 0.0071588
= 0.9922 atm

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Calculate the pressure exerted by one mole of CO2 gas at 273K, if the van der Waals constant a=3.592 dm6 atm mol−2. Assume that the volume occupied by CO2 molecules is negligible.

According to van der Waals equation of state for 1 mole of as gas,( P +aV2 ) (V-b) =0Since, the volume occupied by CO2 molecules is negligible, b =0So,( P +aV2 ) V = RTor,P = RTV2 - aV2= 0.082×27322.4 - 3.592(22.4)2= 0.999375 - 0.0071588= 0.9922 atm

Calculate the pressure exerted by one mole of ${C O}_{2}$ gas at 273K, if the van der Waals constant a=3.592 ${d m}^{6} a t m {m o l}^{- 2}$ . Assume that the volume occupied by ${C O}_{2}$ molecules is negligible.