A plot of volume versus temperature (T) for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in the figure given below.

       

The correct order of pressure is -

         Temperature (K) 

1. ${\mathrm{p}}_1>{\mathrm{p}}_2>{\mathrm{p}}_3>{\mathrm{p}}_4$

2. ${\mathrm{p}}_1={\mathrm{p}}_2={\mathrm{p}}_3={\mathrm{p}}_4$

3. ${\mathrm{p}}_1<{\mathrm{p}}_2<{\mathrm{p}}_3<{\mathrm{p}}_4$

4. ${\mathrm{p}}_1<{\mathrm{p}}_2={\mathrm{p}}_3<{\mathrm{p}}_4$

Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the particles. Following are the critical temperatures of some gases.

From the above data, the order of liquefaction of the given gases is-
(write the order from the gas liquefying first)
1. ${\mathrm{H}}_2,$ $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{N}}_2$
2. $\mathrm{He},$ ${\mathrm{O}}_2,$ ${\mathrm{H}}_2,$ ${\mathrm{N}}_2$
3. ${\mathrm{N}}_2,$ ${\mathrm{O}}_2,$ $\mathrm{He,}$ ${\mathrm{H}}_2$
4. ${\mathrm{O}}_2,$ ${\mathrm{N}}_2,$ ${\mathrm{H}}_2,$ $\mathrm{He}$

The SI unit of viscosity coefficient $\left(\mathrm{\eta }\right)$ is-

1. Pascal

2. Nsm^-2

3. km^-2s

4. Nm^-2

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

1. Remains same

2. Decreases

3. Increases

4. No regular pattern is followed

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

 Among water, ether, and acetone, water has the maximum boiling point and ether has the minimum boiling point. The correct order of vapour pressure of water, acetone and ether at $30°\mathrm{C}$ is-

1. Water<ether<acetone

2. Water<acetone<ether

3. Ether<acetone<water

4. Acetone<ether<water

Van der Waals parameter 'a' signifies -

1.The magnitude of intermolecular attractive forces.

2. The magnitude of intermolecular repulsive forces.

3. The volume of a gas molecule.

4. All of the above.

The pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm³ flask at 27 °C would be -

$1.$ $8.31$ $\times$ ${10}^4$ $\mathrm{Pa}$
$2.$ $7.43$ $\times$ ${10}^{-4}$ $\mathrm{Pa}$
$3.$ $6.87$ $\times$ ${10}^3$ $\mathrm{Pa}$
$4.$ $8.31$ $\times$ ${10}^6$ $\mathrm{Pa}$

At 0^°C, the density of a certain oxide of a gas at 2 bar is the same as that of dinitrogen at 5 bar.

The molecular mass of the oxide would be -

1. 35 g/mol

2. 45 g/mol

3. 70 g/mol

4. 60 g/mol

The temperature of 4.0 mole of a gas occupying 5 dm³ at 3.32 bar is -
(R = 0.083 bar dm³ K^–1 mol^–1).

1. 40 K 

2. 30 K 

3. 20 K

4. 50 K