States of matter practice · Mixed difficulty

As the temperature is raised from ${20^0}C\,\mathrm{to}\,{40^0}C$ the average kinetic energy of neon atoms changes by a factor of which of the following?

If saturated vapours are compressed slowly at constant temperature to half the initial volume, the vapour pressure will

Statement I: The order of viscosities of hexane, water glycerol is hexane $<$ water $<$ glycerol.

Statement II: Hexane has weakest intermolecular force and glycerol the strongest.

Vapour pressure of liquid does/do not depend(s) on

Which of the following statements is not true?

Given below are two statements. One is labelled as Assertion A and the other is labelled as Reason
R.
Assertion A: Activated charcoal adsorbs $\mathrm{SO}_2$ more efficiently than $\mathrm{CH}_4$.

Reason R: Gases with lower critical temperatures are readily adsorbed by activated charcoal.
In the light of the above statements, choose the correct answer from the options given below.

Joule-Thomson expansion of an ideal gas is an

A bottle of dry ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be

What is the temperature at which the kinetic energy of 0.3 mole of helium is equal to the kinetic energy of 0.4 mole of argon at 400 K?

The speed possessed by majority of gaseous molecules is:

S-I: $\mathrm{CH}_4, \mathrm{CO}_2$ has value of $\mathrm{Z}$ (compressibility factor) less than one at $0^{\circ} \mathrm{C}$.

S-II: $\text{Z} < 1$ is due to the attractive forces dominate among the molecules.

Where is the pressure less than 1 atm?

Equal masses of ${O}_2$ and ${CH}_4$ have been taken in same container of volume ${V}$ at $25^{\circ} {C}$. The ratio of volume of gases effuses out initially from vessel is

Energy of sublimation of solid helium is much lower than that of ice because

Most probable velocity $\left(u_{\mathrm{mp}}\right)$, average velocity $\left(u_{\mathrm{av}}\right)$ and root mean square velocity $\left(u_{\mathrm{rms}}\right)$ of a sample of argon are equal, then

The temperature of a gas in a closed container is $27^{\circ} \mathrm{C}$. If the temperature is raised to $327^{\circ} \mathrm{C}$, the pressure exerted is

The density of a gas is equal to? (P = pressure; V = volume; T = temperature, R = gas constant, n = number of moles and M = molecular wt.)

Assertion (A): Compressibility factor for hydrogen varies with pressure with positive slope at all pressures.

Reason (R): Even at low pressures, repulsive forces dominate hydrogen gas.

At what temperature is the rms speed of hydrogen molecules the same as that of oxygen molecules at $1327\,\,^\circ C$ ?

The mean free path $\left( \lambda \right)$ of a gas sample is given by:

Calculate the radius of He atoms if its Vander Waal&rsquo;s constant &lsquo;b&rsquo; is 24 ml $mo{l^{ - 1}}$: (Note $ml$ =cubic centimeter)

A gas such as carbon monoxide would be most likely to obey the ideal gas law at:

A gas can be liquefied at temperature T and pressure P provided

In Vander Wal’s equation, the constant ‘b’ is the measure of:

The critical temperature of a gas is related to van der Waal’s constants as

The rates of diffusion of ${\mathrm{O}_2}$ and ${\mathrm{H}_2}$ at same $P$ and $T$ are in the ratio:

A human adult breathes in approximately $0.50 \mathrm{~dm}^3$ of air at $1.00 \mathrm{~bar}$ with each breath. If an air tank holds $100 \mathrm{~dm}^3$ of air at $200 \mathrm{~bar},$ how many breathes the tank will supply?

The density of gas is found to be $1.41 \mathrm{~g} / \mathrm{L}$ at $700 \mathrm{~mm} \mathrm{~Hg}$ pressure and $350 \mathrm{~K}$ temperature. Gas can be

Assertion: Dalton's law of partial pressure is a special case of Raoult's law.

Reason: Dalton's law applies only to ideal gas mixtures, whereas Raoult's law applies to solutions.

If volume containing gas is compressed to half, how many moles of gas remained in the vessel?