The compressibility factor for a real gas at high pressure is f

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 Multiple Choice QuestionsMultiple Choice Questions

1.

Which among the following gases can be liquified easily?

  • Chlorine

  • Nitrogen

  • Oxygen

  • Hydrogen


2.

If average velocity of a sample of gas molecules at 300 K is 5 cm s-1, what is RMS velocity of same sample of gas molecules at the same temperature? (Given, α: u: v = 1:1.224: 1.127)

  • 6.112 cm/s

  • 4.605 cm/s

  • 4.085 cm/s

  • 5.430 cm/s


3.

Two closed bulbs of equal volume (V) containing an ideal gas initially at pressure pi and temperature T1 are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to T2. The final pressure pf is:

  • 2 straight p subscript straight i open parentheses fraction numerator straight T subscript 1 over denominator straight T subscript 1 plus straight T subscript 2 end fraction close parentheses
  • 2 straight p subscript straight i open parentheses fraction numerator straight T subscript 2 over denominator straight T subscript 1 plus straight T subscript 2 end fraction close parentheses
  • 2 straight p subscript straight i space open parentheses fraction numerator straight T subscript 1 straight T subscript 2 over denominator straight T subscript 1 plus straight T subscript 2 end fraction close parentheses
  • 2 straight p subscript straight i space open parentheses fraction numerator straight T subscript 1 straight T subscript 2 over denominator straight T subscript 1 plus straight T subscript 2 end fraction close parentheses
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4.

The intermolecular interaction that is dependent on the inverse cube of the distance between the molecule is:

  • ion-ion interaction

  • ion-dipole interaction

  • London force

  • London force

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5.

If Z is a compressibility factor, Vander Waal's equation at low pressure can be written as 

  • straight Z space equals 1 plus RT over pb
  • straight Z space equals space 1 minus straight a over VRT
  • straight Z space equals space 1 minus pb over RT
  • straight Z space equals space 1 minus pb over RT
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6.

For the gaseous state, if most probable speed is denoted by C*, average speed by C and mean square speed by C, then for a large number of molecules the ratios of these speeds are:

  • straight C asterisk times colon stack space straight C with bar on top space colon thin space straight C space equals space 1.225 space colon 1.128 space space colon 1
  • straight C to the power of asterisk times space colon thin space straight C with bar on top space colon space straight C space equals space 1.128 space colon thin space 1.225 space colon space 1
  • straight C to the power of asterisk times space colon thin space straight C with bar on top space colon space straight C space equals space 1.28 space colon thin space 1.225 space colon space
  • straight C to the power of asterisk times space colon thin space straight C with bar on top space colon space straight C space equals space 1.28 space colon thin space 1.225 space colon space
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7.

The compressibility factor for a real gas at high pressure is

  • 1 plus RT over pb
  • 1
  • 1 plus pb over RT
  • 1 plus pb over RT


C.

1 plus pb over RT

Vander Waal's equation for one mole of real gas is

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8.

'a' and 'b' are van der Waals constants for gases. Chlorine is more easily liquefied than ethane because :

  • a and b for Cl2 > a and b for C2H6

  • a and b for Cl2 < a and b for C2H6

  • a and Cl2 < a for C2H6 but b for Cl2 > b for C2H6

  • a and Cl2 < a for C2H6 but b for Cl2 > b for C2H6

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9.

If 10–4 dm3 of water is introduced into a 1.0 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 J K–1 mol–1)

  • 5.56 x 10-3 mol

  • 1.53 x 10-2 mol

  • 4.46 x 10-2 mol

  • 4.46 x 10-2 mol

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10.

Assuming that water vapour is an ideal gas, the internal energy change(∆U) when 1 mol of water is vapourised at 1 bar pressure and 100°C, (Given: Molar enthalpy of vapourisation of water at 1 bar and 373 K = 41 kJ mol-1 and R = 8.3 J mol–1K–1 will be) –

  • 4.100 kJ mol–1

  • 3.7904 kJ mol–1

  • 37.904 kJ mol–1

  • 37.904 kJ mol–1

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