The density of a gas is found to be 5.46 g/dm³ at 27^°C at 2 bar pressure. The density of gas at STP would be -

$1. 2.0 \mathrm{g} {\mathrm{dm}}^{-3}$
$2. 3.0 \mathrm{g} {\mathrm{dm}}^{-3}$
$3. 4.5 \mathrm{g} {\mathrm{dm}}^{-3}$
$4. 1.5 \mathrm{g} {\mathrm{dm}}^{-3}$

34.05 mL of phosphorus vapour weighs 0.0625 g at 546 °C and 0.1 bar pressure. The molar mass of phosphorus would be -

$1.$ $1247.5$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$2.$ $2234.7$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$3.$ $3126.9$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$
$4.$ $1134.6$ $\mathrm{g}$ ${\mathrm{mol}}^{-1}$

The minimum pressure required to compress 600 dm³ of a gas at 1 bar to 150 dm³ at 40°C is

1. 4.0 bar

2. 0.2 bar

3. 1.0 bar

4. 2.5 bar

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

A bubble of air is underwater at a temperature15°C and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is 25°C and the pressure is 1.0 bar, what will happen to the volume of the bubble?

1. Volume will become greater by a factor of 2.5
2. Volume will become greater by a factor of 1.6
3. Volume will become greater by a factor of 1.1
4. Volume will become smaller by a factor of 0.70

The pressure exerted by 6.0 g of methane gas in a 0.03 m³ vessel at 129 ºC is:
(Atomic masses : C = 12.01, H = 1.01 and R = 8.314 JK^–1mol^–1)

1. 13409 Pa

2. 41648 Pa

3. 31684 Pa

4. 215216 Pa

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

The state of a gas can be described by quoting the relationship between:

1.  Pressure, volume, temperature

2.  Temperature, amount, pressure

3.  Amount, volume, temperature

4.  Pressure, volume, temperature, amount

With increase in temperature the surface tension of a liquid will:

1. Remains same

2. Decreases

3. Increases

4. No regular pattern is followed

 In the given figure, the curve representing an ideal gas is-

1.  B only

2.  C and D only

3.  E and F only 

4.  A and B only