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When two gaseous molecules of equal radius r collide,
- a)their centres are separated by 2r at the point of contact
- b)effective volume occupied by two molecules is eight times of the volume of each molecule
- c)excluded volume is four times of the volume of each molecule
- d)greater the excluded volume, greater the deviation from ideal behaviour
Correct answer is option 'A,B,C,D'. Can you explain this answer?
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Verified Answer
When two gaseous molecules of equal radius r collide,a)their centres a...
From the figure, their centres are separated by 2r at the point of contact
Volume of 1 molecule = 4/3 πr3 = Vmol
Effective volume = 4/3 π(2r)3 = 8 4/3πr3 = 8Vmol
Excluded volume per molecule = ½ 4/3 π(2r)3 = ½ 8 4/3πr3 = 4Vmol
Greater the excluded volume, greater the deviation from ideal behaviour.
Most Upvoted Answer
When two gaseous molecules of equal radius r collide,a)their centres a...
Explanation:
Collision of Gaseous Molecules:
When two gaseous molecules of equal radius r collide, their centres are separated by 2r at the point of contact. This means that the distance between the two molecules is equal to the sum of their radii.
Effective Volume:
The effective volume occupied by two molecules is eight times the volume of each molecule. This is because the volume of each molecule is πr^3, and when two molecules come together, the total volume they occupy is 8(πr^3).
Excluded Volume:
The excluded volume is four times the volume of each molecule. This means that the volume that cannot be occupied by the two molecules due to their physical size is four times the volume of each molecule.
Deviation from Ideal Behavior:
Greater the excluded volume, greater the deviation from ideal behavior. This is because in ideal gas behavior, molecules are assumed to have zero volume and no intermolecular forces. When the excluded volume is significant, it indicates that the molecules have a finite size and interact with each other, leading to deviations from ideal behavior.
Collision of Gaseous Molecules:
When two gaseous molecules of equal radius r collide, their centres are separated by 2r at the point of contact. This means that the distance between the two molecules is equal to the sum of their radii.
Effective Volume:
The effective volume occupied by two molecules is eight times the volume of each molecule. This is because the volume of each molecule is πr^3, and when two molecules come together, the total volume they occupy is 8(πr^3).
Excluded Volume:
The excluded volume is four times the volume of each molecule. This means that the volume that cannot be occupied by the two molecules due to their physical size is four times the volume of each molecule.
Deviation from Ideal Behavior:
Greater the excluded volume, greater the deviation from ideal behavior. This is because in ideal gas behavior, molecules are assumed to have zero volume and no intermolecular forces. When the excluded volume is significant, it indicates that the molecules have a finite size and interact with each other, leading to deviations from ideal behavior.
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When two gaseous molecules of equal radius r collide,a)their centres are separated by 2r at the point of contactb)effective volume occupied by two molecules is eight times of the volume of each moleculec)excluded volume is four times of the volume of each moleculed)greater the excluded volume, greater the deviation from ideal behaviourCorrect answer is option 'A,B,C,D'. Can you explain this answer?
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