The energy absorbed by each molecule (A₂) of a substance is 4.4 x 10^-19 J and bond energy per molecule is 4.0 x 10^-19 J. The kinetic energy of the molecule per atom will be

A gas at 350 K and 15 bar has molar volume 20 percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor (Z) is:

A certain sample of gas has a volume of 0.2 litre measured at 1 atm pressure and 0$°\mathrm{C}$. At the same pressure but at
273$°\mathrm{C}$, its volume will be:

Which is the correct curve for Charle's law, when the curve is plotted at 0.821 atm pressure for a 10-mole ideal gas?

Which is not correct curve for gay-lusacc's law?

A certain hydrate has the formula ${\mathrm{MgSO}}_4. {\mathrm{xH}}_2\mathrm{O}$. A quantity of 54.2 g of the compound is heated in an oven to drive off the water. If the water vapour generated exerts a pressure of 24.8 atm in a 2.0 L container at 120$°\mathrm{C}$, the value of x is-

A mixture of Ne and Ar at 250 K has a total K.E.=3 kJ in a closed vessel, the total mass if Ne and Ar is 30 g. Find mass % of Ne in a gaseous mixture at 250 K.

In two vessels of 1 litre each at the same temperature 1 g of ${\mathrm{H}}_2$ and 1 g of ${\mathrm{CH}}_4$ are taken, for these:

Four particles have speed 2, 3, 4 and 5 cm/s respectively. Their rms speed is:

A gaseous mixture contains 4 molecules with a velocity of $6 \mathrm{cm} {\sec }^{-1}$, 5 molecules with a velocity of $2 \mathrm{cm} {\sec }^{-1}$ and 10 molecules with a velocity of $3 \mathrm{cm} {\sec }^{-1}$. What is the RMS velocity of the gas:

The ratio between the root mean square velocity of ${\mathrm{H}}_2$ at 50 K and that of ${\mathrm{O}}_2$ at 800 K is:

If ${\mathrm{C}}_1, {\mathrm{C}}_2, {\mathrm{C}}_3...$ represent the speeds of ${\mathrm{n}}_1, {\mathrm{n}}_2, {\mathrm{n}}_3...$ molecules respectively, then the root mean square speed will be:

At what temperature will average speed of the molecules of the second member of the series ${\mathrm{C}}_{\mathrm{n}}{\mathrm{H}}_{2\mathrm{n}}$ be the same of ${\mathrm{Cl}}_2$ at $627°\mathrm{C}$?

If ${\mathrm{U}}_{\mathrm{RMS}}$ of a gas is $30 {\mathrm{R}}^{1/2} {\mathrm{ms}}^{-1} \mathrm{at} 27°\mathrm{C}$ then the molar mass of gas is:

The compressibility factor for nitrogen at 330 K and 800 atm is 1.90 and at 570 K and 200 atm is 1.10. A certain mass of ${\mathrm{N}}_2$ occupies a volume of $1 {\mathrm{dm}}^3$ at 330 K and 800 atm. Calculate volume occupied by same quantity of ${\mathrm{N}}_2$ gas at 570 K and 200 atm:

Consider the following statements. If the van der Waals' parameters of two gases are given as

$$\begin{gathered} \mathrm{a}/{\mathrm{dm}}^6 \mathrm{bar} {\mathrm{mol}}^{-2} \mathrm{b}/{\mathrm{dm}}^3 {\mathrm{mol}}^{-1} \\ \mathrm{Gas} \mathrm{A} 6.5 0.055 \\ \mathrm{Gas} \mathrm{B} 2 0.01 \end{gathered}$$

then:

1.  Critical volume of A > Critical volume of B
2.  Critical pressure A > Critical temperature of B
3.  Critical temperature of A > Critical temperature of B

Which of the above statement is incorrect?

 The van der Waals parameters for gases W, X, Y and Z are

Which one of these gases has the highest critical temperature?

Pressure remaining the same, the volume of a given mass of an ideal gas increase for every degree centigrade rise in temperature by definite fraction of its volume at:

The critical temperature of a substance is:

The excluded volume of a gas will be larger, if $\frac{{\mathrm{T}}_{\mathrm{C}}}{{\mathrm{P}}_{\mathrm{C}}}$ is:

The correct order of temperature of a real gas is-

I. Boyle's temperature

II. Critical temperature

III. Inversion temperature

The temperature at which the second virial coefficient of real gas is zero is called:

However great the pressure, a gas cannot be liquified above its:

The temperature at which real gases obey the ideal gas laws over a wide range of low pressure is called:

What will happen to gas if it is adiabatically expanded at 600 K if its Boyle's temperature is 290 K?

The van der Waal's equation of law of corresponding states for 1 mole of gas is:

In water-saturated air, the mole fraction of water vapor is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is-

The volume occupied by 1.8 g of water vapour at 374 ${}^{\mathrm{o}}\mathrm{C}$ and 1 bar pressure will be -

[Use R=0.083 bar ${\mathrm{LK}}^{-1} {\mathrm{mol}}^{-1}$]

A mixture of ${\mathrm{N}}_2$ and Ar gases in a cylinder contains 7 g of ${\mathrm{N}}_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of ${\mathrm{N}}_2$ is:

[Use atomic masses (in g ${\mathrm{mol}}^{-1}$): N=14, Ar=40]