Home
Class 12
CHEMISTRY
Read the paragraph carefully and answer ...

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`
0.5 value of compressibility factor (z) indicates that the gas

A

shows positive deviation from the ideal gas

B

negative deviation from the ideal gas behaviour

C

either of the two

D

the factor is insufficient

Text Solution

Verified by Experts

The correct Answer is:
B
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • GASEOUS STATE

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) LEVEL-II COMPREHENSION-II|4 Videos

  • GASEOUS STATE

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) LEVEL-II COMPREHENSION-III|5 Videos

  • GASEOUS STATE

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) LEVEL-II|20 Videos

  • ENVIRONMENTAL CHEMISTRY

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) LEVEL -II (MULTIPLE CORRECT QUESTIONS)|20 Videos

  • GENERAL ORGANIC CHEMISTRY

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTIONS|14 Videos

Similar Questions

Explore conceptually related problems

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 van der Waal equation is obeyed by the real gases

Real gases deviate from an ideal behaviour because gas molecules

Knowledge Check

  • 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 At low pressure, the van der waal equation is

    A
    `P=RT+(a)/(V)`
    B
    `P=RT-(a)/(V)`
    C
    `P=RT+(a)/(V^(2))`
    D
    `P=RT-(a)/(V^(2))`

  • 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

  • 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 values of van der Waal's constant 'a' ("atm"^(2) L^(2)" mol"^(2)) for the gases N_(2), H_(2) NH_(3) and SO_(2) are given 0.25, 3.5, 4,9 and 6.9 respectively. Which will have the highest ease of liquefaction?

    A
    `SO_(2)`
    B
    `NH_(3)`
    C
    `N_(2)`
    D
    `H_(2)`

    • Similar Questions

    Explore conceptually related problems

    A real gas show ideal behaviour at :-

    Gas deviates from ideal gas bahaviour because molecules

    Real gases show deviations from, ideal behaviour when

    Gases deviate from the ideal gas behaviour because their molecules

    The deviation from ideal behaviour of a gas can be expressed as

    Home
    Profile