States of matter practice · Mixed difficulty

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.

An open vessel containing air is heated from 300 K to 400 K. The fraction of air originally present which goes out of it is:

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

Relative density of a volatile substance with respect to $O_2$ is 8. Its molecular weight would be

S.I units of gas constant R is

The minimum pressure required to compress $200 \mathrm{~dm}^3$ of air at $2 \mathrm{~atm}$ to $50 \mathrm{dm}^3$ at $25^{\circ} \mathrm{C}$ 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.

To an evacuated vessel with movable piston under external pressure of 1 atm, 0.1 mole of He and 1.0 mole of an unknown compound (vapour pressure 0.68 atm at $0\,\,^\circ C$ ) are introduced. Considering the ideal gas behaviour, the total volume (in litre) of the gases at $0\,^\circ C$  is close to

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 $\left(\mathrm{N}_0=6 \times 10^{23} \mathrm{~mol}^{-1}\right)$.

The compressibility factor for an ideal gas is

“One gram molecule of a gas at N.T.P occupies 22.4 lit” This fact was derived from

With increase of pressure, the mean free path

If temperature of 1 mole of gas is increased by $50\,^\circ C$ calculate the change in kinetic energy of the system

The temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is

The interaction force present between $\mathrm{H}_2$ molecules are

Find the ratio of moles of $\mathrm{SO}_2$ to $\mathrm{CH}_4$ after fifth diffusion steps if their initially mole ratio is $8: 1.$

Vander waal constant “b” is very high for the following gas

The relative rates of diffusion of ${\mathrm{U}^{235}}{\mathrm{F}_6}$ and ${\mathrm{U}^{238}}{\mathrm{F}_6}$ are

The van der Waals’ equation for a real gas is given by the formula $\left( {p + \frac{{{n^2}a}}{{{V^2}}}} \right)\left( {V - nb} \right) = nRT,\mathrm{where}p,V,T\mathrm{and}n$ are the pressure, volume, temperature and the number of moles of the gas. Which one is the correct interpretation for the parameter a?

A mixture of Ne and Ar kept in a closed vessel at $250 \mathrm{~K}$ has a total K.E. $=3 \mathrm{~kJ}$. The total mass of $\mathrm{Ne}$ and $\mathrm{Ar}$ is $30 \mathrm{~g}$. Find mass % of $\mathrm{Ne}$ in gaseous mixture at $250 \mathrm{~K}$.