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At Boyle’s temperature, the value of com...

At Boyle’s temperature, the value of compressibility factor `Z = (pV_(m)//RT= V_("real")//V_("real"))` has a value of 1, over a wide range of pressure. This is due to the fact that in the van der Waal’s equation

A

the constant 'a' is negligible and not 'b'

B

the constant 'b' is negligible and not 'a'

C

both the constant 'a' and 'b' are negligible

D

the effect produced due to the molecular attraction compensates the effect produced due to the molecular volume

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The correct Answer is:
D
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At Boyle's temperature the value of compressibility factro Z = (PV_(m(//RT = V_(real)//V_(ideal)) has a value of 1 over a wide range of pressure. This is due to the fact that in the van der Waal's equation

Compressibility factor, Z of a gas is given as Z=(pV)/(nRT) (i) What is the value of Z for an ideal gas ? (ii) For real gas what will be the effect on value of Z above boyle's temperature ?

One of the important approach to the study of real gases involves the analysis of parameter Z called the compressibility factor Z = (PV_(m))/(RT) where P is pressure, V_(m) is molar volume, T is absolute temperature and R is the universal gas constant. such a relation can also be expressed as Z = ((V_(m)real)/(V_(m)ideal)) (where V_(m ideal) and V_(m real) are the molar volume for ideal and real gas respectively). Gas corresponding Z lt 1 have attractive forces amoung constituent particles. As the pressure is lowered or temperature is increased the value of Z approaches 1. (reaching the ideal behaviour) For a real gas G Z gt 1 at STP Then for 'G': Which of the following is true:

One of the important approach to the study of real gases involves the analysis of parameter Z called the compressibility factor Z = (PV_(m))/(RT) where P is pressure, V_(m) is molar volume, T is absolute temperature and R is the universal gas constant. such a relation can also be expressed as Z = ((V_(m)real)/(V_(m)ideal)) (where V_(m ideal) and V_(m real) are the molar volume for ideal and real gas respectively). Gas corresponding Z lt 1 have attractive forces amoung constituent particles. As the pressure is lowered or temperature is increased the value of Z approaches 1. (reaching the ideal behaviour) {:("Observation",,"Conclusion"),(I.Z =1,,I."The gas need not be showing the ideal behaviour"),(II. Zgt1,, II. "On applying pressure the gas will respond by"),(,,"increasing its volume"),(III. Z lt 1,, III. "The gas may be liquefied"),(IV. Z rarr1 "for low" P,, IV. "The gas is approaching the ideal behaviour") :}

The compressibility factor (Z) of real gas is usually less than 1 at low temperature and low pressure because

For a real gas , the compressibility factor Z has different values at different temperatures and pressures . Which of the following is not correct under the given conditions ?

At a high pressure, the compressibility factor (Z) of a real gas is usually greater than one. This can be explained from van der Waals equation by neglecting the value of:

Boyle's temperature or Boyle point is the temperature at which a real gas starts behaving like an ideal gas over a particular range of pressure. A graph is plotted between compressibility factor Z and pressure P. What is the deviation of real gas from ideal behaviour in terms of compressibility factor , Z ?

Boyle's temperature or Boyle point is the temperature at which a real gas starts behaving like an ideal gas over a particular range of pressure. A graph is plotted between compressibility factor Z and pressure P. What is the variation of Z with pressure ?

Ideal gas equation is represented as PV=nRT . Gases present in universe were fond ideal in the Boyle's temperature range only and deviated more from ideal gas behavior at high pressure and low temperature. The deviation are explained in term of compressibility factor z . For ideal behavior Z=(PV)/(nRT)=1 . the main cause to show deviavtion were due to wrong assumptions made about forces oif attractions (which becomes significant at high pressure ) and volume V occupied by molecules in PV=nRT is supposed to be volume of gas or the volume of container in which gas is placed by assuming that gaseous molecules do not have appreciable volume. Actually volume of the gas is that volume in which each molecule of gas can move freely. If volume occupied by gaseous molecule is not negligible, then the term V would be replaced by the ideal volume which by available for free motion of each molecule of gas in 1 mole gas. V_("actual")= volume of container -volume occupied by molecules =v-b Where b represent the excluded volume occupied by molecules present in one mole of gas. Similarly for n mole gas V_("actual")=v-nb The ratio of coefficient of thermal expansion alpha=(((delV)/(delT))_(P))/V and the isothermal compressibility beta=-((delV)/(delP)_(T)) for an ideal gas is:

RESONANCE ENGLISH-GASEOUS STATE-Exercise
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  12. In the van der Waals equation

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  13. Which of the following statements are correct?

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  14. Which of the following is correct for critical temperature ?

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  15. The vander waal gas constant ‘a’ is given by :

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  16. Which of the following are correct statements?

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  17. Select the correct statements(s):

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  18. Which is/are correct for real gases?

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  19. Which of the following statements are incorrect?

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  20. One of the important approach to the study of real gases involves the ...

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