A gas such as carbon monoxide would be most likely to obey the ideal gas law at?
1. High temperature and low pressure
2. Low temperature and high pressure
3. High temperature and high pressure
4. Low temperature and low pressure

Equal masses of H₂, O₂ and CH₄ have been taken in a container of volume V at temperature 27 ºC in identical conditions. The ratio of the volumes of gases H₂:O₂ : CH₄ would be:

1. 8:16:1
2. 16:8:1
3. 16:1:2
4. 8:1:2

50 mL of each gas A and of gas B takes 200 and 150 s respectively for effusing through a pinhole under the similar conditions. If the molecular mass of gas B is 36, the molecular mass of gas A will be:

1. 96

2. 128

3. 32

4. 64

A certain gas takes three times as long to effuse out as helium. Its molecular mass will be:

1.  36 u
2.  64 u
3.  9 u
4.  27 u

For real gases van der Waals equation is written as

$(P+\frac{a{n}^2}{V^2})$ $(V-nb)$ $=$ $nRT$

where 'a' and 'b' are van der Waals constants.

Two sets of gases are:
(I) $O_2,$ $C{O}_2$ $,$ $H_2$ $and$ $He$        (II)$C{H}_4,$ $O_2$ $$ $and$ $H_2$ 
The gases given in set-I are in increasing order of 'b' and gases given in set-II are in decreasing order of 'a'. Select the correct order from the following:

1. $($ $I)O_2<He<H_2<C{O}_2(II)$ $H_2>O_2>C{H}_4$

2. $($ $I)H_2<He<O_2<C{O}_2(II)$ $C{H}_4>O_2>H_2$

3. $($ $I)H_2<O_2<He<C{O}_2(II)$ $O_2>C{H}_4>H_2$

4. $($ $I)He<H_2<C{O}_2<$ $$ $O_2\left(II\right)$ $C{H}_4>H_2>O_2$

By what factor does the average velocity of a gaseous molecule increase when the temperature (in Kelvin) is doubled?

1.  2.8
2.  4.0
3.  1.4
4.  2.0