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Which of the following is NOT a postulat...

Which of the following is NOT a postulate of the kinetic molecular theory of gases?

A

The gas molecules are in random motion.

B

The collisions between the molecules are perfectly elastic.

C

The average kinetic energy per molecule of different gases is equal at a given temperature.

D

The pressure exerted by a gas is due to intermolecular forces.

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The correct Answer is:
D
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TARGET PUBLICATION-STATES OF MATTER (GASES AND LIQUIDS) -EVALUATION TEST
  1. Which of the following is NOT a postulate of the kinetic molecular the...

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  2. At constant temperature and pressure which of the following gases will...

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  3. At 1 atm and 273 K the density of gas, whose molecular weight is 45, i...

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  4. For a closed system consisting of a reaction N(2) O(4(g)) rarr 2NO(2(g...

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  5. Three different gases X, Y and Z of molecular masses 2, 16 and 64 were...

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  6. At a constant pressure, the density of a certain amount of an ideal ga...

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  7. What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm press...

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  8. At what temperature, the r.m.s. velocity of a gas measured at 50^(@)C ...

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  9. At 25^(@)C and 1 atm, a vessel contains 20 L of an ideal gas. If the v...

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  10. Which set of conditions represents easiest way to liquefy a gas ?

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  11. Volume of the air that will be expelled from a vessel of 300 cm^(3) wh...

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  12. At what temperature do the average speed of CH(4)(g) molecules equal t...

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  13. A bubble of gas released at the bottom of a lake increases to four t...

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  14. At a constant volume, a quantity of an ideal gas has a pressure of 80...

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  15. At critical point, the surface tension is "".

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  16. Vapour pressure of a liquid depends upon its

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  17. The boiling point of inert gases increases with the increase in atomic...

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  18. Each gas exhibit "" deviation from ideal behaviour.

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  19. Which of the following statements is INCORRECT for a real gas ?

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  20. Many real gases behave as ideal gases at "".

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  21. What is the relationship between the average velocity (v), root mean s...

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