Q. Three identical adiabatic containers and contain helium, neon and oxygen respectively at equal pressure. The gases are pushed to half their original volumes :

Kinetic Theory Report Error

A

The final temperature in the three containers will be the same.

B

The final pressures in the three containers will be the same.

C

The pressure of helium and neon will be the same but that of oxygen will be different.

D

The temperature of helium and neon will be the same but that of oxygen will be different.

Solution:

As gas volumes are reduced to half for both and containers as gases are monoatomic their pressure and temperatures will also change by same amount but in as the gas is diatomic, its changes will be different.

Questions from Kinetic Theory

1. Which one of the following is not an assumption in the kinetic theory of gases?

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2. A gas at one atmosphere and 100 mL is mixed with another gas of equal moles at 0.5 atm and having volume 50 mL in flask of 1 L. What is their final pressure?

3. Two moles of monoatomic gas is mixed with three moles of a diatomic gas. The molar specific heat of the mixture at constant volume is

4. At what temperature is the root mean square speed of an atom in an argon gas cylinder equal to the rms speed of a helium gas atom at - ? (Atomic mass of and )

5. In a process, temperature and volume of one mole of an ideal monoatomic gas are varied according to the relation , where is a constant. In this process the temperature of the gas is incresed by . The amount of heat absorbed by gas is (R is gas constant) :

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