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

Question

Calculate the pressure exerted by one mole of CO2 gas at 273 K if the van der Waals' constant a = 3.592 dm6 atm mol-2. Assume that the volume occupied by CO2 molecules is negligible. (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

In case of negligible molecular volume, b=0 and van der Waals' equation reduces to (p+(n2 a/V2)) V =n R T ⇒ p =(R T/V)-(a/V2) (n=1 text mole ) =(0.082 × 273/22.4)-(3.592/(22.4)2)=0.99 atm

Q. Calculate the pressure exerted by one mole of $C O_{2}$ gas at $273 K$ 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.

In case of negligible molecular volume, $b = 0$ and van der Waals' equation reduces to
$(p + \frac{n ^{2} a}{V ^{2}}) V = n RT$
$\Rightarrow p = \frac{RT}{V} - \frac{a}{V ^{2}} (n = 1 mole)$
$= \frac{0.082 \times 273}{22.4} - \frac{3.592}{( 22.4 ) ^{2}} = 0.99 a t m$

Q. Calculate the pressure exerted by one mole of CO2​ gas at 273K if the van der Waals' constant a=3.592dm6atmmol−2. Assume that the volume occupied by CO2​ molecules is negligible.

In case of negligible molecular volume, b=0 and van der Waals' equation reduces to (p+V2n2a​)V=nRT ⇒p=VRT​−V2a​(n=1 mole ) =22.40.082×273​−(22.4)23.592​=0.99atm

Q. Calculate the pressure exerted by one mole of $C O_{2}$ gas at $273 K$ 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.

In case of negligible molecular volume, $b = 0$ and van der Waals' equation reduces to
$(p + \frac{n ^{2} a}{V ^{2}}) V = n RT$
$\Rightarrow p = \frac{RT}{V} - \frac{a}{V ^{2}} (n = 1 mole)$
$= \frac{0.082 \times 273}{22.4} - \frac{3.592}{( 22.4 ) ^{2}} = 0.99 a t m$