States of matter practice · Mixed difficulty

Helium has the van der Waal's constant $b=24 \mathrm{~mL} \mathrm{~mol}^{-1}$. The molecular diameter of helium will be

The equation, $\left[ {{P_r} + \frac{3}{{V_r^2}}} \right]\left[ {3{V_r} - 1} \right] = 8{T_r}:$

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?

The inversion temperature $T_i({~K})$ of hydrogen is (given van der Waal's constants $a$ and $b$ are $0.244 {~atm} {~L} {~mol}^{-2}$ and $0.027 {Lmol}^{-1}$ respectively)

The root mean square speed of the molecules of diatomic gas is $u$. When the temperature is doubled, the molecules dissociates into two atoms. The new speed of the atom is:

Statement I: In van der Waals' equation $\left(p+\frac{n^2 a}{V^2}\right)(V-n b)=n R T$ Pressure correction between molecules. $\left(\frac{n^2 a}{V^2}\right)$ is due to force of attraction

Statement II: Pressure of the gas is due to collisions of molecules against sides of the container

If "A" joule kinetic energy possess by $\mathrm{N}$ number of $\mathrm{O}_2$ molecules at $150 \mathrm{k}$ and " $2 \mathrm{~A}$ " joule kinetic energy possess by $\mathrm{O}_2$ molecules of another sample at $300 \mathrm{k}$, Find how many molecules of $\mathrm{O}_2$ present in another sample.

Under identical condition of temperature and pressure, which among the following gases has lowest density?

Van der Waal found that two assumptions made by kinetic theory of gases were wrong, one of them is that gas molecules are

If two molecules of A and B having mass 100 kg and 64 kg and rate of diffusion of A is $12 \times {10^{ - 3}}$ then what will be the rate of diffusion of B

Assertion (A): The value of van der Waals' constant '$a$' is higher for ammonia than for nitrogen.

Reason (R): Intermolecular hydrogen bonding is present in ammonia.

Which of the following statements on critical constants of gases are correct?

I. Larger the $T_c / p_c$ value of a gas, larger would be the excluded volume.

II. Critial temperature $\left(T_c\right)$ of a gas is greater than its Boyle temperature $\left(T_B\right)$.
III. At the critial point in the van der Waals' gas isotherm.

$\left(\frac{\partial p}{\partial V_m}\right)_{T_c}=0$

Select the correct answer using the codes given below.

$2\mathrm{g}$ of hydrogen diffuses from a container in 10 minute. How many gram of oxygen would diffused through the same container in the same time under similar conditions?

One mole of an ideal monoatomic gas is mixed with 1 mole of an ideal diatomic gas. The molar specific heat of the mixture at constant volume is:

Equal volumes of two gases which don’t react together are confined in separate vessels. Their pressure is 100 mm and 300 mm of Hg respectively. If the two vessels are joined together, then what will be the pressure of the resulting mixture? (Temperature remains constant)

When air is blown to balloon (at constant temperature) its pressure and volume both increases. This violates:

Dalton’s law of partial pressure will not apply to which of the following mixture

At what temperature will the volume of a gas at $0\,^\circ C$ double itself, pressure remaining constant?

The total kinetic energy associated with n moles of monoatomic gas is

At ordinary temperature and pressure, among halogens, the chlorine is a gas, bromine is a liquid and iodine is a solid. This is because:

Which pair of the gases diffuse through a small hole with the same rate of diffusion at same ‘P’ at ‘T’

Compressibility factor for a gas under critical conditions is

For one mole of an ideal gas, increasing the temperature from $10^\circ C$ to $20\,\,^\circ C$

Slope between $pV\,\,\mathrm{and}\,\,p$ at constant temperature is

Calculate the total pressure in a 10.0 L cylinder which contains 0.4 g helium, 1.6 g oxygen and 1.4 g nitrogen at $27\,^\circ C$.

The average speed of an ideal gas molecule at ${27^0}C$ is $0.3\mathrm{m}{\sec ^{ - 1}}$. The average speed at $\mathrm{9}{27^0}C$ will be $\mathrm{m}{\sec ^{ - 1}}$

${O_2}$ is collected over water at $20\,^\circ C$. The pressure inside shown by the gas is 740 mm of Hg. What is the pressure due to ${\mathrm{O}_2}$ alone if vapour pressure of ${\mathrm{H}_2}\mathrm{O}$ is 18 mm at $20\,\,^\circ C$ ?

Which gas can be most readily liquefied?

Value of universal gas constant ($R$) depends upon

The concept of critical temperature for a gas was given by: