States of matter practice · Medium

A perfect gas of a given mass is heated first in a small vessel and then in a large vessel, such that their volume remains unchanged. The $P - T$ curves are:

Following properties will decrease with increase in temperature except

If the assumption that there is no force of attraction between the molecules of a gas is correct, what will be the consequences?

$X \mathrm{~mL}$ of $\mathrm{H}_2$ gas effuse through a hole in a container in $5 \mathrm{~s}$. The time taken for the effusion of the same volume of the gas specified below under ideal conditions is

A gas of unknown identity effuses at the rate of $83.3\,\,\mathrm{mL}{\mathrm{s}^{ - 1}}$ in an effusion apparatus in which carbon dioxide effuses at the rate of $102\,\,\mathrm{mL}{\mathrm{s}^{ - 1}}$. Calculate molar mass of the unknown gas

Equal masses of $C{H_4}$ and ${O_2}$ are mixed in a container at $25^\circ \,C$. Fraction of total pressure exerted by ${O_2}$ is

In two separate bulbs containing ideal gases $A$ and $B$ respectively, the density of gas $A$ is twice that of gas $B$ while molecular weight of gas $A$ is half that of gas $B$ at the same temperature, pressure ratio ${P_A}/{P_B}$ will be:

$4.0\mathrm{g}$ of argon has pressure $P$ and temperature $T\,\,\mathrm{K}$ in a vessel. On keeping the vessel at $50^\circ$ higher temperature, $0.8\mathrm{g}$ of argon was given out to maintain the pressure $P$. The original temperature was:

Assertion : Compressibility factor $(Z)$ for non-ideal gases can be greater than 1 .

Reason : Non-ideal gases always exert higher pressure than expected.

Correct order of van der Waals constant b of given gases is

Dipole-Dipole interaction energy b/w polar molecule in solid depends on the radius of the molecule $\left( r \right)$ and it is directly proportional to

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of $1\mathrm{mol}\,\,\mathrm{litr}{\mathrm{e}^{ - 1}}$ ? $(\;R = 0.082$ litre atm $\mathrm{mo}{\mathrm{l}^{ - 1}}{\deg ^{ - 1}})$

A closed cylinder having volume $20 \mathrm{~L}$ contains $56 \mathrm{~g} {~N}_2$ and $16 \mathrm{~g} {~He}$ gases. If pressure exerted by the gaseous mixture is $8.2 \mathrm{~atm}$ then the temperature of the gas molecules will be

If pressure of a fixed quantity of a gas is increased 4 times keeping the temperature constant, the r.m.s. velocity will be

Which of the assumption of the kinetic molecular theory best explains the observation that a balloon collapses when exposed to liquid nitrogen (which is much colder than a cold winter day)?

2 moles of ${NH}_3(\mathrm{g})$ and 1 mole of ${HCl}(\mathrm{g})$ are taken in a container of capacity 8.21 lit at $300 \mathrm{~K}$ to produce ${NH}_4{Cl}(\mathrm{s})$. Find the total pressure after the reaction.

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

Active mass of 14 grams of Nitrogen at STP is '$\mathrm{X}$'. Active mass of 8 grams of oxygen at STP is '$\mathrm{Y}$'. Ratio of $\mathrm{X}$ to $\mathrm{Y}$ is

S-I: Compressibility factor for hydrogen varies with pressure with positive slope at all pressures at $0^{\circ} \mathrm{C}$.
S-II: Even at low pressures, repulsive forces dominate hydrogen gas at $0^{\circ} \mathrm{C}$.

The density of a gas $A$ is 4 times to that of a gas $B$ If the molecular mass of $A$ is $M$ what is the molecular mass of $B$

Assertion (A): Different gases at the same conditions of temperature and pressure have same root mean square speed.

Reason (R): Average kinetic energy of a gas is directly proportional to temperature in kelvin scale.

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:

A glass bulb of $2 \mathrm{~L}$ capacity is filled by helium gas at $10 \mathrm{~atm}$ pressure. Due to a leakage the gas leaks out. What is the volume of gas leaked if the final pressure in container is $1 \mathrm{~atm}.$

A quantity of gas is collected in a graduated tube over the mercury. The volume of gas at $18^{\circ} \mathrm{C}$ is $50.0 \mathrm{~mL}$ and the level of mercury in the tube is $100 \mathrm{~mm}$ above the outside mercury level. The barometer reads 750 torr. Hence, volume at STP is approximately

Equal masses of $\mathrm{H}_2, \mathrm{O}_2$ and methane have been taken in a container of volume $\mathrm{V}$ at temperature $27^{\circ} \mathrm{C}$ in identical conditions. The ratio of the volumes of gases $\mathrm{H}_2: \mathrm{O}_2$ : methane would be :

Equal masses of $C{H_4}$ and ${H_2}$ are mixed in an empty container at $25^\circ C$. The fraction of the total pressure exerted by ${H_2}$ is

S.I units of gas constant R is

Assertion: The molecules of the dissolved gas present in a liquid gain kinetic energy as temperature is raised.

Reason : Gases tends to be more soluble in liquids as the temperature is raised.

At the top of the mountain the thermometer reads $0^{\circ} \mathrm{C}$ and the barometer reads $710 \mathrm{~mm}$ of $\mathrm{Hg}$. At the bottom of the mountain the temperature is $30^{\circ} \mathrm{C}$ and pressure is $760 \mathrm{~mm}$ of $\mathrm{Hg}$. Density of air at the top with that at the bottom is

A flask contains $12 \mathrm{~g}$ of a gas of relative molecular mass 120 at a pressure of $100 \mathrm{~atm}$ was evacuated by means of a pump until the pressure was $0.01 \mathrm{~atm}$. Which of the following is the best estimate of the number of molecules left in the flask $\left(\mathrm{N}_0=6 \times 10^{23} \mathrm{~mol}^{-1}\right)$.