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Match column-I with column-II : {:((A)...

Match column-I with column-II :
`{:((A)" Real gas at high pressure",(p)PV=RT+Pb),((B)" Force of attraction among gas Molecules is negligible",(q)PV=nRT),((C)" At high temp. and low pressure",(r)Z=1),((D)" Real gas at NTP",(s) (P+(an^(2))/(V^(2)))(V-nb)=nRT):}`

Text Solution

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`A rarr (p), B rarr (q), C rarr (q,r), D rarr (s)`
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The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT

The unit of the van der Waals gas equation parameter 'a' in (P+(an^(2))/(V^(2)))(V-nb)=nRT is :

Knowledge Check

  • {:(,"Column-I",,"Column-II"),("(P)","If volume of gas molecules be negligible",,(1)(P+a/V_(2))(V-b)=RT),("(Q)","At very high pressure",,"(2)PV=RT+Pb"),("(R)","At low pressure and high temperature",,(3)PV=RT-a/V),("(S)","van der Waal's gas",,"(4)PV=RT"):}

    A
    `{:("P Q R S"),("3 2 4 1"):}`
    B
    `{:("P Q R S"),("2 4 1 3"):}`
    C
    `{:("P Q R S"),("3 4 1 2"):}`
    D
    `{:("P Q R S"),("2 3 1 4"):}`

  • Read the paragraph carefully and answer the following questions: Real gases deviate from ideal behaviour because of the following two faulty assumptions of kinetic theory. (I) The actual volume occupied by molecules is negligible as compared to the total volume of the gas. (II) The forces of attraction and repulsion between molecules of the gas are negligible. The extent of deviation of a real gas from ideal behaviour is expressed in terms of compressibility factor (z). Hence, suitable corrections were applied to the ideal gas equation so that it can also explain the behaviour of real gases. The equation obtained by applying the two corrections to the usual gas equation is known as van der Waal equation. A Volume correction Corrected (ideal) volume = (V - b) Where b is the effective volume of the molecules. B. Pressure correction (intermolecular attraction corection). Corrected (ideal) pressure = P + P However, P=(a)/(V^(2)) therefore The van der Waal's equation becomes (P+(an^(2))/(V^(2)))(V-nb)=nRT The pressure correction used on the ideal gas behaviour is generally indicated by P +P what does this P' stand for

    A
    the pressure not involved in striking the wall
    B
    the pressure already present in the vessel
    C
    the inward force exerted on molecules about to strike the wall
    D
    the outward force exerted on molecules about to strike the wall

  • Assertion (A) : At high pressure , for one mole of a real gas , the compression factor Z is (1 + (Pb)/(RT)) Reason (R) : At high pressure , for one mole of a real gas , vanderwall equation is modified as P(V-b) = RT

    A
    Both Assertion and Reason are true and Reason is the correct explanation of the Assertion.
    B
    Both Assertion and Reason are true but Reason is not the correct explanation of Assertion .
    C
    Assertion is true but Reason is wrong .
    D
    Both Assertion and Reason are wrong .

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    {:(,"List-I(Van der Waals equation)",,"List-II(given by)"),("(a)","high pressure and low temperature",,"(p)PV=RT+Pb"),("(b)","low pressure",,(q)PV=RT-a//V),("(c)","Force of attraction is negligible",,"(r)PV=RT+aV"),("(d)","volume of molecule is negligible",,"(s)[P+a/V^(2)](V-b)=RT):}

    Real gases obey the gas equation : PV=nRT more correctly at low temperature and high pressure.

    Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT Calculate the value of 'a' assuming volume of molecules to be negligible.

    Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the value of Z for an ideal gas?

    Deviation of real gases from ideal behaviour can be studied by plots of compressibility factor (Z) vs p. The copressibility factor is Z=(pV)/(nRT) The compressibility factor for 1 mole of a gas obeying van der Waals gas equation at 0^(@)C and 100 atm pressure is found to be 0.5. The van der Waals gas equation is (p(an^(2))/(V^(2)))(V-nb)=nRT What is the volume of the gas?

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