States of matter practice · Mixed difficulty

What is the pressure of 2 moles of $N{H_3}$ at $27^\circ C$ when its volume is 5 L in van der Waals’ equation $\left( {a = 4.17,b = 0.03711} \right)$

(a) Find the total pressure of components if a container of volume 8.21 lit. contains 2 moles of $\mathrm{A}$ and 3 mole of $\mathrm{B}$ at $300 \mathrm{~K}$

(b) What will be the partial pressure of component $\text{C}$ if 5 moles of $\mathrm{C}$ is also added to the container at same temperature.

At what temperature, both Celsius and Fahrenheit scale read the same value?

According to the Avogadro’s Law, equal volumes of two different gases, under same conditions of temperature and pressure, contain equal number of:

The root mean square velocity of a gas is doubled when temperature is

The behavior of a real gas is usually depicted by plotting compressibility factor $Z$ versus $P$ at a constant temperature. At high temperature and high pressure, $Z$ is usually more than one. This fact can be explained by van der Waals equation when

A gas cannot be liquefied if:

Which of the following represents the value of gas constant, $\mathrm{R}$ in $\mathrm{cal} / \mathrm{K} \mathrm{~mol}$ ?

Which is a postulate of kinetic theory of gases?

As the speed of molecules increases, the number of collisions per second:

Assertion: The pressure of a gas is directly proportional to the density of gas at a constant temperature and molecular mass.

Reason: The molecular weight of a vapour of a substance can be calculated using the expression $M=\frac{d R T}{P}$, where $M$ is the molecular weight of the vapour, $d$ is its density and $P$ is the pressure of the vapour, ${R}$ is the gas constant and ${T}$ is the temperature.

The rms speed of hydrogen is $\sqrt 7$ times the rms speed of nitrogen. If $T$ is the temperature of the gas, then

When $r,p\,\,\mathrm{and}\,\,M$  represent rate of diffusion, pressure and molecular mass, respectively, then the ratio of the rates of diffusion $\left( {{r_A}/{r_B}} \right)$ of two gases $A\,\,\mathrm{and}\,\,B$  is given as

If temperature (in Kelvin) is quadrupled then rms speed of gaseous molecules become

At relatively high pressure, van der Waals’ equation reduces to:

Equal moles of ${H_2}$ and ${O_2}$ gases are placed in a container with a pin hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the ${H_2}$ to escape

One mole of $\mathrm{N}_2$ and 3 moles of $\mathrm{H}_2$ are taken in a container of capacity 8.21 lit. at $300 \mathrm{~K}$ to produce $\mathrm{NH}_3.$ Find the partial pressures of $\mathrm{N}_2$ and $\mathrm{H}_2$ if partial pressure of $\mathrm{NH}_3$ after sufficient time was found to be $3 \mathrm{~atm}$.

At critical state, the compressibility factor $(Z)$ for a real gas is equal to

A flask containing air at $107^{\circ} \mathrm{C}$ and $722 \mathrm{~mm}$ of $\mathrm{Hg}$ is cooled to $100 \mathrm{~K}$ and $760 \mathrm{~mm}$ of $\mathrm{Hg}$. If density in the initial condition $1 \mathrm{~g} / \mathrm{cm}^3$, then what is the final density $\left(\mathrm{g} / \mathrm{cm}^3\right)$ ?

The ratio of most probable velocity, average velocity, root mean square velocity is

Ideal gas equation in terms of KE per unit Volume, E is

Which one, among the following, is the van der Waals’ equation, describing the behaviour of one mole of a real gas over wide ranges of temperature and pressure?

Dalton’s law of partial pressure is not applicable to

A gas will approach ideal behaviour at

Solid $\mathrm{C}{\mathrm{H}_4}$ is:

The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends on

The density of ${N_2}$ gas at 0.821 atmospheric pressure and ${7^0}C$

If the pressure at the triple point of a substance is greater than $1\,\,atm$, we expect:

In case of hydrogen and helium the van der Waals’ forces are:

Maximum deviation from ideal gas is expected for