Calculate the pressure exerted by one mole of CO2 gas at 273K if the Vander Waal’s constant a= 3.592dm6 atm mol-2. Assume the volume occupied by CO2 molecules are negligible.

p+aV2(V−b)=RT if ,b=0,P+aV2V=RTP=RTV−aV2P=0.082X27322.4−3.59222.42=0.99atm

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Calculate the pressure exerted by one mole of CO₂ gas at 273K if the Vander Waal’s constant a= 3.592dm⁶ atm mol^-2. Assume the volume occupied by CO₂ molecules are negligible.

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answer is 0.99.

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Detailed Solution

$\begin{array}{l} (p + \frac{a}{V^{2}}) (V - b) = RT \\ if, b = 0, (P + \frac{a}{V^{2}}) V = RT \\ P = \frac{RT}{V} - \frac{a}{V^{2}} \\ P = \frac{0.082 X 273}{22.4} - \frac{3.592}{22 . 4^{2}} = 0.99 atm \end{array}$

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