Chapter: State of Matter

A mixture of one mole each of \(\begin{align}{{H}_{2}}\end{align}\), He and \(\begin{align}{{O}_{2}}\end{align}\) each are enclosed in a cylinder of volume] at temperature. If the partial pressure of \(\begin{align}{{H}_{2}}\end{align}\) is 2 atm, the total pressure of the gases in the cylinder is:

A spherical balloon of radius 3 cm containing helium gas has a pressure of\(\begin{align}48\times {{10}^{{-3}}}\end{align}\)bar. At the same temperature, the pressure, of a spherical balloon of radius 12 cm containing the same amount of gas will be ______ \(\begin{align}\times {{10}^{6}}\end{align}\) bar.

Which one of the following graphs is not correct for ideal gas?

d = Density, P = Pressure, T = Temperature

Match the type of interaction in column A with the distance dependence of their interaction energy in column B:
A                                                    B
(I) ion-ion                             (A) \(\begin{align}\frac{1}{r}\end{align}\)
(II) dipole-dipole                 (B) \(\begin{align}\frac{1}{{{{r}^{2}}}}\end{align}\)
(III) London dispersion      (C) \(\begin{align}\frac{1}{{{{r}^{3}}}}\end{align}\)
.                                                (D) \(\begin{align}\frac{1}{{{{r}^{6}}}}\end{align}\)

The predominant intermolecular forces present in ethyl acetate, a liquid, are:

The relative strength of interionic/ intermolecular forces in decreasing order is:

0.5 moles of gas A and x moles of gas B exert a pressure of 200 Pa in a container of volume 10 \(\begin{align}{{m}^{3}}\end{align}\) at 1000 K. Given R is the gas constant in J \(\begin{align}{{K}^{{-1}}}mo{{l}^{{-1}}}\end{align}\), x is:

An open vessel at 27°C is heated until two fifth of the air (assumed as an ideal gas) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant, the temperature at which the vessel has been heated is:

Assuming ideal gas behaviour, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is: (Atomic wt. of Cl = 35.5u)

10. Among the following, the incorrect statement is:

At 300 K, the density of a certain gaseous molecule at 2 bar is double to that of dinitrogen (\(\begin{align}{{N}_{2}}\end{align}\)) at 4 bar. The molar mass of gaseous molecule is:

Two closed bulbs of equal volume (\(\begin{align}V\end{align}\)) containing an ideal gas initially at pressure \(\begin{align}{{p}_{i}}\end{align}\) and temperature \(\begin{align}{{T}_{1}}\end{align}\) are connected through a narrow tube of negligible volume. The temperature of one of the bulbs is then raised to \(\begin{align}{{T}_{2}}\end{align}\). The final pressure \(\begin{align}{{p}_{f}}\end{align}\) is:

When does a gas deviate the most from its ideal behaviour?

The initial volume of a gas cylinder is 750.0 mL. If the pressure of gas inside the cylinder changes from 840.0 mm Hg to 360.0 mm Hg, the final volume the gas will be:

Sulphur dioxide and oxygen were allowed to diffuse through a porous partition. 20 \(\begin{align}d{{m}^{3}}\end{align}\) of \(\begin{align}S{{O}_{2}}\end{align}\) diffuses through the porous partition in 60 seconds. The volume of \(\begin{align}{{O}_{2}}\end{align}\) in \(\begin{align}d{{m}^{3}}\end{align}\) which diffuses under the similar condition in 30 seconds will be (atomic mass of sulphur = 32 u):

For 1 mol of an ideal gas at a constant temperature \(\begin{align}T\end{align}\), the plot of (log \(\begin{align}P\end{align}\)) against (log \(\begin{align}V\end{align}\)) is a (\(\begin{align}P\end{align}\): Pressure, \(\begin{align}V\end{align}\): Volume)

When \(\begin{align}C{{O}_{2}}\end{align}\) (g) is passed over red hot coke it partially gets reduced to CO(g). Upon passing 0.5 L of \(\begin{align}C{{O}_{2}}\end{align}\) (g) over red hot coke, the total volume of the gases increased to 700 mL. The composition of the gaseous mixture at STP is

An open vessel at 300 K is heated till 2/5th of the air in it is expelled. Assuming that the volume of the vessel remains constant, the temperature to which the vessel is heated, is

The intermolecular interaction that is dependent on the inverse cube of distance between the molecules is:

If of water is introduced into a 1.0 \(\begin{align}\text{d}{{\text{m}}^{3}}\end{align}\) flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established? (Given: Vapour pressure of H2O at 300 K is 3170 Pa; Y = 8.314 J\(\begin{align}{{\text{K}}^{{-1}}}\text{ }mol{{~}^{{-1}}}\end{align}\))

For an ideal gas, number of moles per litre in terms of its pressure \(\begin{align}P\end{align}\), gas constant \(\begin{align}R\end{align}\) and temperature \(\begin{align}T\end{align}\) is

Value of gas constant\(\begin{align}R\end{align}\) is

Identify the correct labels of A, B and C in the following graph from the options given below:
image6 Root mean square speed (\(\begin{align}{{V}_{{rms}}}\end{align}\)); most probable speed (\(\begin{align}{{V}_{{mp}}}\end{align}\)); average speed (\(\begin{align}{{V}_{{av}}}\end{align}\))

Points I, II and III in the following plot respectively correspond to (\(\begin{align}{{V}_{{mp}}}\end{align}\): most probable velocity)

Initially, the root mean square (rms) velocity of \(\begin{align}{{N}_{2}}\end{align}\) molecules at certain temperature is u. If this temperature is doubled and all the nitrogen molecules dissociate into nitrogen atoms, then the rms velocity will be:

Which of the following is not an assumption of the kinetic theory of gases?

The ratio of masses of oxygen and nitrogen in a particular gaseous mixture is 1: 4. The ratio of number of their molecules is:

The temperature at which oxygen molecules have the same root mean square speed as helium atoms have at 300 K is: Atomic masses: He = 4 u, O = 16 u)

For gaseous state, if most probable speed is denoted by C*, average speed by \(\begin{align}\bar{C}\end{align}\) and mean square speed by C, then for a large number of molecules the ratios of these speeds are:

By how many folds the temperature of a gas would increase when the root mean square velocity of the gas molecules in a container of fixed volume is increased from \(\begin{align}5\text{ }\times \text{ }{{10}^{4}}\text{ }cm/s\end{align}\) to \(\begin{align}10\times \text{ }{{10}^{4}}\text{ }cm/s\end{align}\)?

Which one of the following is the wrong assumption of kinetic theory of gases?

\(\begin{align}\alpha ,v\end{align}\) and \(\begin{align}u\end{align}\) represent most probable velocity, average velocity and root mean square velocity respectively of a gas at a particular temperature. The correct order among the following is

The relationship among most probable velocity, average velocity and root mean square velocity is respectively

When r, \(\begin{align}P\end{align}\) and \(\begin{align}M\end{align}\) represent rate of diffusion, pressure and molecular mass, respectively, then the ratio of the rates of diffusion \(\begin{align}\left( {{{r}_{A}}/{{r}_{B}}} \right)\end{align}\) of two gases \(\begin{align}A\end{align}\) and \(\begin{align}B\end{align}\), is given as

The molecular velocity of any gas is:

Which one of the following statements is NOT true about the effect of an increase in temperature on the distribution of molecular speeds in a gas?

As the temperature is raised from 20 ºC to 40 ºC, the average kinetic energy of neon atoms changes by which factor

According to the kinetic theory of gases, in an ideal gas, between two successive collisions a gas molecule travels

Kinetic theory of gases proves

Consider the following table:

a and b are van der waals constants. The correct statement about the gases is:

Consider the van der Waals constants, a and b, for the following gases,

Which gas is expected to have the highest critical temperature?

At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behaviour. Their equation of state is given as \(\begin{align}P=\frac{{RT}}{{V-b}}\end{align}\) at T. Here, b is the van der Waals constant. Which gas will exhibit steepest increase in the plot of Z (compression factor) vs P?

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

At very high pressures, the compressibility factor of one mole of a gas is given by:

If Z is a compressibility factor, van der Waals equation at low pressure can be written as:

van der Waals equation for a gas is stated as, \(\begin{align}P=\frac{{nRT}}{{V-nb}}-a{{\left( {\frac{n}{V}} \right)}^{2}}\end{align}\). This equation reduces to the perfect gas equation, \(\begin{align}P=\frac{{nRT}}{V}\end{align}\) when,

The compressibility factor for a real gas at high pressure is:

In van der Waals equation of state of the gas law, the constant ‘b’ is a measure of