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Physics MCQs for NEET — Practice Questions with Answers

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At lower temperatures, all gases except H2 and He show:

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500 mL of nitrogen at 27°C is cooled -5°C at the same pressure. The new volume becomes      

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Explanation

(b) Initial volume, V1 = 500 mL

Initial temperature,

              T1 = 27°C = 27 + 273 = 300 K

Final temperature,

             T2 = -5 + 273 = 268 K

             V2 = ?

             V1/T1 = V2/T2

             V2 = V1T2/T1 = (500 x 268)/300 = 446.66 mL

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In case of hydrogen and helium the van der Waals' forces are:

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Explanation

(c) H2 and He possess minimum molar mass among all gases.

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With increase of pressure, the mean free path:

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Explanation

(a) Increase of pressure decreases volume and molecules come closer to each other.

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The compressibility factor of a gas is defined Z=PV/nRT. The compressibility factor of an ideal gas is:

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Explanation

(c) For ideal gases PV = nRT, ... Z =1; because Z = PV/nRT

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 Air at sea level is dense. This is a practical application of:

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Explanation

(a) V∝1/P or density ∝P (... d∝1/V),Boyle's law 

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In van der Waals' equation of state of the gas, the constant 'b' is a measure of:

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Explanation

(c) b = 4 x N x volume of one molecule in rest.

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For 1 mole of gas, the average kinetic energy is given as E. The urms of gas is :

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Explanation

(a) Average kinetic energy, E = (3/2)RT

 urms = 3RTM = 2EM

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600 cc of a gas at a pressure of 750 mm is compressed to 500 cc. Taking the temperature to remain constant, the increase in pressure is                                           

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Explanation

(a) According to Boyle's law,

           p1V1 = p2V2

          750 x 600 =p2 x 500

                    p2 = (750 x 600)/500 = 900 mm

   So, the increase in pressure = 900-750 =150 mm

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At which one of the following temperature pressure conditions, the deviation of a gas from ideal behaviour is expected to be minimum?                                     

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Explanation

(b) A real gas behave as an ideal gas at low pressure and high temperature.

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