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Gas deviates from ideal gas nature becau...

Gas deviates from ideal gas nature because molecules

A

have kinetic energy

B

are bound by covalent bonds

C

attract one another

D

show the Tyndall effect

Text Solution

Verified by Experts

The correct Answer is:
C
At high pressure, the molecules are close together and hence attractions between them are large. There is an inward pull on the molecules striking the wall. Hence, the observed pressure is less
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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' for gases within Boyle's temperature range 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 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 .

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