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Liquids diffuse slowly as compared to ga...

Liquids diffuse slowly as compared to gases because;- liquids have no definite śhape , the molecules of liquid are heavy, the molecules of liquid move fast, the molecules are held together by strong intermolecular forces

A

liquids have no definite śhape

B

the molecules of liquid are heavy

C

the molecules of liquid move fast

D

the molecules are held together by strong intermolecular forces

Text Solution

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The correct Answer is:
D
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Knowledge Check

  • Assertion : All the gases should be cooled below their critical temperature for liquification. Reason : Cooling slows down the movement of molecules therefore, intermolecular forces may hold the slowly moving molecules together and the gas liquifies.

    A
    If both (A) and (R) are correct and (R) is the correct explanation of (A).
    B
    If both (A) and (R) are correct, but (R) is not the correct explanation of (A).
    C
    If (A) is correct, but (R) is incorrect.
    D
    If both (A) and (R) are incorrect.

  • The molecules of a gas move in all directions with various speeds, The speeds of the molecules of the gas increase with rise in temperature. During its random motion, a fast molecule often strikes against the walls of the container of the gas. The collisions are assumed to be perfectly elastic,i.e, the molecule bounces back with the same speed with which it strikes the wall. Since the number of molecules is very large, billions of molecules strike against the walls of the container every second. These molecules exert a sizable force on the wall. The force exerted per unit area is the pressure exerted by the gas on the walls. According to kinetic theory, the pressure of the gas of density p at absolute temperature T is given by P=1/3 pv_(rms)^2 where r_(rms) is the root mean square speed of the gas molecule and is given by v_(rms)=sqrt((3kT)/m) where m is the mass of the molecule and k is Boltzmann constant Choose the only correct statement from the following

    A
    The pressure of a gas is equal to the total kinetic energy of its molecules per unit volume of the gas
    B
    The product of pressure and volume of a gas is always constant
    C
    The average kinetic energy of the molecules of a gas is proportional to its absolute temperature
    D
    The root mean square speed of a molecule is proportional to the absolute temperature of the gas

  • The molecules of a gas move in all directions with various speeds, The speeds of the molecules of the gas increase with rise in temperature. During its random motion, a fast molecule often strikes against the walls of the container of the gas. The collisions are assumed to be perfectly elastic,i.e, the molecule bounces back with the same speed with which it strikes the wall. Since the number of molecules is very large, billions of molecules strike against the walls of the container every second. These molecules exert a sizable force on the wall. The force exerted per unit area is the pressure exerted by the gas on the walls. According to kinetic theory, the pressure of the gas of density p at absolute temperature T is given by P=1/3 pv_(rms)^2 where r_(rms) is the root mean square speed of the gas molecule and is given by v_(rms)=sqrt((3kT)/m) where m is the mass of the molecule and k is Boltzmann constant The root mean square speed of oxygen gas molecule at T =320K is very nearly equal to (the molar mass of oxygen M=0.0320kg per mole and gas constant = R=8.31 J mol^-1 K^-1 )

    A
    `300 ms^-1`
    B
    `500 ms^-1`
    C
    `700 ms^-1`
    D
    `900 ms^-1`

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    The molecules of a gas move in all directions with various speeds, The speeds of the molecules of the gas increase with rise in temperature. During its random motion, a fast molecule often strikes against the walls of the container of the gas. The collisions are assumed to be perfectly elastic,i.e, the molecule bounces back with the same speed with which it strikes the wall. Since the number of molecules is very large, billions of molecules strike against the walls of the container every second. These molecules exert a sizable force on the wall. The force exerted per unit area is the pressure exerted by the gas on the walls. According to kinetic theory, the pressure of the gas of density p at absolute temperature T is given by P=1/3 pv_(rms)^2 where r_(rms) is the root mean square speed of the gas molecule and is given by v_(rms)=sqrt((3kT)/m) where m is the mass of the molecule and k is Boltzmann constant IF the temperature of a gas is increased from 27^@C to 927^@C the root mean square speed of its molecules

    The molecules of a gas move in all directions with various speeds, The speeds of the molecules of the gas increase with rise in temperature. During its random motion, a fast molecule often strikes against the walls of the container of the gas. The collisions are assumed to be perfectly elastic,i.e, the molecule bounces back with the same speed with which it strikes the wall. Since the number of molecules is very large, billions of molecules strike against the walls of the container every second. These molecules exert a sizable force on the wall. The force exerted per unit area is the pressure exerted by the gas on the walls. According to kinetic theory, the pressure of the gas of density p at absolute temperature T is given by P=1/3 pv_(rms)^2 where r_(rms) is the root mean square speed of the gas molecule and is given by v_(rms)=sqrt((3kT)/m) where m is the mass of the molecule and k is Boltzmann constant From the relation v_(rms)=sqrt((3kT)/m_1) if follows that the constant k should be expressed in units of

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