Home
Class 11
CHEMISTRY
Gases tend to behave non-ideally at low ...

Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction.
Select incorrect statement(s) :

A

Volume correction is due to finite size of molecules and pressure correction is due to force of attraction between molecules.

B

At high temperatures, molecules have greater kinetic energy, and attractive forces are smaller and he behaviour of gases is close to the ideal gas behaviour

C

Volume correction is also called covolume or excluded volume and is four times the volume of spherical molecules present in one mole of the gas

D

At very low pressure, force of attraction is effective and pressure correction needs further resolution.

Text Solution

Verified by Experts

At very ow `P, Z ~~ 1`.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • STATES OF MATTER

    AAKASH SERIES|Exercise LECTURE SHEET - EXERCISE - IV (LEVEL - II ADVANCED)(MATRIX MATCHING TYPE QUESTIONS)|3 Videos

  • STATES OF MATTER

    AAKASH SERIES|Exercise LECTURE SHEET - EXERCISE - IV (LEVEL - II ADVANCED)(INTEGER TYPE QUESTIONS)|4 Videos

  • STATES OF MATTER

    AAKASH SERIES|Exercise LECTURE SHEET - EXERCISE - IV (LEVEL - II ADVANCED)(MORE THAN ONE CORRECT ANSWER TYPE QUESTIONS)|9 Videos

  • SATURATED HYDROCARBONS

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|10 Videos

  • STOICHIOMETRY

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|59 Videos

Similar Questions

Explore conceptually related problems

Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Following represents equation of state for a mules of real gas [P + (n^2a)/(V^2)][V-nb] = nRT .Select incorrect statement for a real gas

Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Which assumption of kinetic theory is not followed when a real gas shows non-ideal behaviour ?

Knowledge Check

  • Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Following represents equation of state for n moles of real gas. [P + (n^(2)a)/V^(2)][V-nb] = nRT Select incorrect statement for a real gas

    A
    Constant 'a' is a measure of force of attraction among gas molecules
    B
    a is expressed in atm `L^(2) "mol"^(-2)` b is expressed in L `"mol"^(-1)`
    C
    At high pressure, compression factor is `(1+ (Pb)/(RT))`
    D
    `(n^(2)a)/V^(2)` is also called internal volume.

  • (A): A gas behaves as an ideal gas at high temperature and low pressure. (R): Helium behaves as an ideal gas under all conditions.

    A
    Both A and R are correct and R is the correct explanation of A.
    B
    Both A and R are correct but R is not the correct explanation of A
    C
    A is true but R is false.
    D
    A is false but R is true.

  • Consider following statements : (A) Tfie Sas whose critical temperature is above room temperature can be liquified by applying sufficient pressure to the gas. (B): The gas whose critical temperature is below room temperature can be liquified by the temperature below Tc. Select correct statement:

    A
    A
    B
    B
    C
    both
    D
    none

    • Similar Questions

    Explore conceptually related problems

    Ideal gas equation is represented as PV=nRT . Gases present in the universe were found ideal n the Boyle's temperature range only. The compressibility factor for an ideal gas, Z= (PV)/(nRT) . The main cause to show deviations were due to wrong assumptions made bout forces of attractions (which becomes significant at high pressure). olume occupied by molecules V, in PV = nRT, is supposed to be volume of as or, the volume of container in which gas is placed by assuming that aseous molecules do not have appreciable volume. Actual volume of the as is that volume in which each molecule of a gas can move freely. If olume occupied by gaseous molecule is not negligible, then the term V hould be replaced by the ideal volume which is available for free motion of ach molecule of gas. Similarly for n moles of gas V_("actual") = V-nb The excluded volume can be calculated by considering bimolecular collisions. The excluded volume is the volume occupied by the sphere of 2r for each pair of molecule. Thus, excluded volume for one pair of molecules = 4/3 pi (2r)^3 = (4 xx 8 pi r^3)/3 The excluded volume for 1 molecule = 2/3 xx 8 pi r^3 = 4 xx (4/3 pi r^3) = 4V The excluded volume for N molecules = 4NV = b (where N is Avogadro's No.) The compressibility factor for N_2 at -50^@C and 800 atm pressure is 1.95. Number of moles of N_2 required to fill a balloon of 100 L capacity is :

    Consider following statements : (A): The gas whose critical temperature is above room temperature can be liquified by applying sufficient pressure to the gas. (B): The gas whose critical temperature is below room temperature can be liquified by the temperature below T_c . Select correct statement

    (A) : A gas behaves more closely as an ideal gas at low pressure and high temperature. ( R) : Boyle's law is valid at low pressure and high temperature.

    Two identical vessels A and B with frictionless pistons contain the same ideal gas at the same temperature and the same volume V. The masses of gas in A and B are m_A and m_B respectively. The gases are allowed to expand isothermally to the same final volume 3 V. The change in pressures of the gas in A and B are found to be Delta P and 1.5 Delta P respectively. Then

    When some amount of non-volatile solute is dissolved in a solvent to prepare a dilute solution, the vapour pressure of the solvent is lowered and it is directly proportional to the mole fraction of solvent in the solution . Relative lowering in vapour pressure is equal to mole fraction of solute . Elevation in boiling point of solvent is a collgative property like lowering in vaour pressure of solvent in solution , K_(b) i.e., molal elevation constant is calculated by the formula, K_(b)=DeltaT_(b)// molality and also by the expression, K_(b)=RT_(b)^(2)//1000l_(v) where T_(b) is boiling point of solvent and I_(v) is latent heat of vapourisation for 1 gm solvent . Abnormal elevation is boiling point =iX elevation in boiling point in ideal solution where i=van't Hoff factor Which of the following relation /statements is correct?

    Home
    Profile