Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at `37^(@)C`. Given that the van der Waals constants are a=3.59 `L^(2) atm mol^(-2)` and b=0.0427 L `mol^(-1)`. Compare the value with the calculated value if the gas were considered as ideal.

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel

1.	Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at `37^(@)C`. Given that the van der Waals constants are a=3.59 `L^(2) atm mol^(-2)` and b=0.0427 L `mol^(-1)`. Compare the value with the calculated value if the gas were considered as ideal.
Answer» According to van der Waals equation, `(p+(an^(2))/(V^(2)))(v-nb)=nRT "or "P=(nRT)/(V-nb)-(an^(2))/(V^(2))` Here, `n=(110)/(44)=2.5` moles. Substituting the given values, we get `P=((2.5 mol)(0.0821" L atm "K^(-1) mol^(-1)))/((2 L-2.5 molxx0.0427 L mol^(-1)))-((3.59 L^(2) atm" mol"^(-2))(2.5 mol^(-2)))/((2 L)^(2))` `33.61 atm-5.61 atm=28.0` If the gas were considered is ideal gas, applying ideal gas equation, PV=nRT, we get `P=(nRT)/(V)=((2.5 mol)(0.0821" L atm mol"^(-1))(310 K))/(2 L)=31.8 atm`

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Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at `37^(@)C`. Given that the van der Waals constants are a=3.59 `L^(2) atm mol^(-2)` and b=0.0427 L `mol^(-1)`. Compare the value with the calculated value if the gas were considered as ideal.

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