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Gas deviates from ideal gas nature becau...

Gas deviates from ideal gas nature because molecules

A

are colourless

B

attract each other

C

contain covalent bond

D

show Brownian movement

Text Solution

Verified by Experts

The correct Answer is:
B
For gases to show ideal behaviour there should be no attractive or repulsive forces among the molecules
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The gases obey the different gas laws only theoretically. Practically all of them show some deviation from these laws. These are called real gases. The deviation are maximum under high pressyre and at low temperature. These are comparatively small when the conditions are reversed. It has been found that the easily liquefiable gases show more deviations from the ideal gas beheviour as compared to the gases which are liqufied with diffculty. Gas deviates from ideal gas beheviour because molecules

Real gases deviate from an ideal behaviour because gas molecules

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The ratio of Z at Boyle's temperature and at critical conditions for 1 mole of a given gas is .

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The gas which always shows predominative repulsive forces .

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The numerical value of Z is greater than 1 for gases usually at .

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The compressibility factor SO_(20 is 0.711 then .

The ideal gas behaviour has been expressed in terms of ideal gas equation PV =nRT Since none of the gas in univers is ideal one and deviations are noticed from ideal gas nature The deviations from ideal gas nature has been explained in terms of compressiblity factor Z = (Z =(PV)/(nRT)) Usually when Z gt1 repulsive forces among molecules predominates and when Z lt1 attraction forces predominates. However almost all the gases show ideal gas behaviour within Boyle s temperature range The numberical value of Z for 1 mole of gas at critical conditions is (3)/(8) The numerical value of 'Z' for gases within Boyle's temperature range is .

DINESH PUBLICATION-STATE OF MATTER (GASEOUS AND LIQUID STATE)-Revision question from competitive exams
  1. The pressure of 2 mole of ideal gas at 546 K having volume 44.8 L is

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  2. The average kinetic energy of an ideal gas per molecule in SI units at...

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  3. Gas deviates from ideal gas nature because molecules

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  4. The value of compressibility factor (Z) for an ideal gas is

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  5. van der Waal's equation is true for

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  6. If the volume of 2 moles of an ideal gas at 540 K is 44.8 litres then ...

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  7. A gaseous mixture of three gases A, B and C has a pressure of 10 atm. ...

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  8. The volume of 2.8 g of carbon monoxide at 27^(@) C and 0.821 atm press...

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  9. At 25^(@)C and 730 mm pressure, 380 mL of dry oxygen was collected. If...

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  10. Which one of the following statement is wrong for gases ?

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  11. The value of universal gas constant R depends on :

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  12. Two moles of an ideal gas at 1 atm are compressed to 2 atm at 273 K. T...

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  13. In a mole of water vapours at STP, the volume actually occupied or tak...

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  14. At STP, a container has 1 mole of Ar, 2 mole of CO(2), 3 moles of O(2)...

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  15. If two moles of an ideal gas at 546 K occupy volume of 44.8 L, then pr...

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  16. The relationship which describes the variation of vapour pressure with...

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  17. Gas equation PV = nRT is obeyed by

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  18. The temperature below which a gas does not exist is called its

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  19. Van der Waal's equation reduces itself to the ideal gas equation at :

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  20. In a flask of volume V litres, 0.2 mol of oxygen 0.4 mol of nitrogen,...

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