Chemistry NCERT Exemplar Solutions Class 11th Chapter Five

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This is a short answer type question as classified in NCERT Exemplar

1. At low pressure, the curve of real gas coincides  with that of ideal gas, this shows that the deviation of  behaviour of real gas with respect to ideal gas is small or negligible.

2. At high pressure, the curve of real gas is far apart from  ideal gas, this shows that the deviation of  behaviour of real gas with respect to ideal gas is large.

3. The  pressure p₁ and volume V₁  are  the point where real gas behaves as an ideal gas. 

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1. According to Boyle's law,  

Pressure of a gas is inversely proportional  to volume of gas at constant temperature. So, the volume decreases with increase in pressure at constant temperature.

2. According to Charles's law,

Volume of a gas is directly proportional to temperature when the pressure is constant. So, the volume of gas increases with increase in temperature.

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The increase in temperature increases the kinetic energy of the molecules which decreases the intermolecular forces operating between its particles and hence, the viscosity of a liquid decreases. So, the viscosity of a liquid  decreases if its temperature is increased.

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Hexane is a  nonpolar molecule which has london force between the molecules, which is a weak force. 

Water and glycerine have  O atoms which is an electronegative atom that forms H bonding between the molecules along with dipole-dipole interaction. 

Glycerine has three  O atoms, so it forms more H bonding and hence, has stronger  intermolecular forces.

So the increasing order of intermolecular forces is Hexane   <   Water  <  Glycerin. Stronger the  intermolecular forces, the greater is the viscosity, so the increasing order of their viscosities is: 

Hexane   <   Water  <  Glycerin

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The two phenomena that can be explained on the basis of surface tension are:

1. Spherical shape of rain droplets.

2. Capillary action due to which the liquid in capillary rises and falls.

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Unit of 'P'  =  N m^-2

Unit of 'a'   =  N m^-2  X   (m³)²  / (mol)²

= N-m⁴ mol^-2

Unit of 'a' when pressure is in atm, and volume in dm³   

Unit  of 'P' =  atm

Unit of 'a'   =  atm  X  (dm³)²  / (mol)²

= atm-dm⁶ mol^-2

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The CO₂ gas cannot be liquified at the 32°C and 80 atm pressure as the given temperature and pressure are above critical temperature (T_c) and critical pressure (p_c) which are 30.98°C and 73 atm respectively.

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(i) The value of Z for an ideal gas is 1. 

(ii) For real gas, the value of Z > 1 above Boyle's temperature