Calculate the pressure exerted by one mole of CO 2 gas at 273 K if the van der Waa ls‟ constant a = 3.592 dm 6 atm mol – 2 . Assume that the volume occupied by CO 2 molecules is negligible.

Question

Vikas TU · Answer

Since Volume of container is not specified the Real gas eqn. would get remained in terms of volume. Negligible molecules volume would only led the b constant to zero. Mention the Volume of container in which the whole process / chemialc reaction would takes place.

Balaji Krishnamachari · Answer

but this question is an iit jee advanced 2000 chemistry question....they too have not specified the volume...

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Calculate the pressure exerted by one mole of CO 2 gas at 273 K if the van der Waa ls‟ constant a = 3.592 dm 6 atm mol – 2 . Assume that the volume occupied by CO 2 molecules is negligible.

Calculate the pressure exerted by one mole of CO
2
gas at 273 K if the van der Waa
ls‟ constant
a = 3.592 dm
6
atm mol
–
2
. Assume that the volume
occupied by CO
2
molecules is negligible.

2 Answers

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Calculate the pressure exerted by one mole of CO 2 gas at 273 K if the van der Waa ls‟ constant a = 3.592 dm 6 atm mol – 2 . Assume that the volume occupied by CO 2 molecules is negligible.

Calculate the pressure exerted by one mole of CO2gas at 273 K if the van der Waals‟ constanta = 3.592 dm6atm mol–2. Assume that the volumeoccupied by CO2molecules is negligible.

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Calculate the pressure exerted by one mole of CO
2
gas at 273 K if the van der Waa
ls‟ constant
a = 3.592 dm
6
atm mol
–
2
. Assume that the volume
occupied by CO
2
molecules is negligible.