States of matter practice · Mixed difficulty

Critical temperature of a gas is the temperature

A closed container containing $\mathrm{O}_2$ and some liquid water was found to exert $740 \mathrm{~mm}$ pressure at $27^{\circ} \mathrm{C}.$

(a) Then calculate the pressure exerted by $\mathrm{O}_2$ if aqueous tension at $27^{\circ} \mathrm{C}$ is $20 \mathrm{~mm}$

(b) What will be the final pressure if volume is reduced to half.

(consider volume of liquid water negligible)

In which molecule the van der Waals’ force is likely to be the most important in determining the m.p. and b.p.?

At absolute zero:

Which of the following gases will have highest rate of diffusion

The volume of gas A is twice than that of gas B. The compressibility factor of gas A is thrice then that of gas B at same temperature. The pressures of the gases for equal number of moles are

Which one of the following is correct about surface tension (ST) and viscosity $(\eta )$?

The forces present in the crystals of naphthalene are:

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

The partial pressure of a dry gas is:

A bottle of dry $\mathrm{N}{\mathrm{H}_3}$ and bottle of dry $\mathrm{HCl}$ connected through a long tube are opened simultaneously at both ends, the white $\left( {\mathrm{N}{\mathrm{H}_4}\mathrm{Cl}} \right)$ ring first formed will be:

How does the surface tension of a liquid vary with increase in temperature

Iron crystallises in a bcc system with a lattice parameter of 2.861 Å. Calculate the density of iron in the bcc system (atomic weight of ${Fe}=56, N_A=6.02 \times 10^{23} \mathrm{~mol}^{-1}$ )

S.I units of gas constant R is

If for two gases of molecular weights $M_A$ and $M_B$ at temperature $T_A$ and $T_B, T_A M_B=T_B M_A$, then which property has the same magnitude for both the gases.

When a sample of gas is compressed at constant temperature from 15 atm to 60 atm, its volume changes from $76\,\,\mathrm{c}{\mathrm{m}^3}\,\,\mathrm{to}\,\,20.5\,\,\mathrm{c}{\mathrm{m}^3}$. Which of the following statements are possible explanations of this behaviour? 1. The gas behaves non-ideally. 2. The gas dimerises. 3. The gas is absorbed into the vessel walls.

Two identical cylinders contain helium at $2.5atm$ and argon at $1atm$ respectively. if both the gases are filled in one of the cylinders, the pressure would be:

Ratio of root mean square speed of ${O_2}$ at 200 K and ${N_2}$ at 400 K will be

32 g of ${\mathrm{O}_2}$ 2 g of ${H_2}$ and 28 g of ${N_2}$ at STP occupy separately a volume of

The gas which has lowest critical temperature is

The most probable velocity (in cm/s) of hydrogen molecule at $27\,^\circ C$ will be

If $1\,\,\mathrm{litre}$ of a gas $A$ at 600 mm and 0.5 litre of gas $B$ at 800 mm are taken in a $2\,\,\mathrm{litre}$ bulb. The resulting pressure is:

The term that corrects for the attractive forces present in a real gas in the van der Waals’ equation is

For the type of interactions; (I) Covalent bond, (II) van der Waals’ forces, (III) Hydrogen bonding, (IV) Dipole-dipole interaction, which represents the correct order of increasing stability?

Assertion (A): For a fixed amount of gas, the product PV is always constant.

Reason (R): Gases deviate more from ideal behavior at high pressure and low temperatures.

The relationship between ${P_c},{V_c}$ and ${T_c}$ is:

Boyle’s law is applicable in:

The ratio $a/b$ (the terms used in van der Waals’ equation) has the unit:

Vapour pressure of a liquid depends upon:-

A monoatomic ideal gas undergoes a process in which the ratio of $P$ to $V$ at any instant is constant and equal to unity. The molar heat capacity of the gas is