The force $(F)$ required to maintain the flow of layers of a liquid is equal to

( $A=$ area of contact of layers

$d z=$ distance between the layers

$d u=$ change in velocity

$\eta=$ coefficient of viscosity)

At 298 K , a flask ' $A$ ' of unknown volume $(V)$ contains oxygen at 5 atm . Another flask ' $B$ ' of volume 2 L contains helium at 3 atm . Two flasks are connected together by a small tube of zero volume. After the two gases are completely mixed, if the resulting mixture is found to have the mole fraction of oxygen as 0.2 , the volume of flask ' $A$ ' (in L ) is

(Assume oxygen and helium as ideal gases)

At $T(\mathrm{~K})$ root mean square (rms) velocity of argon (molar mass $40 \mathrm{~g} \mathrm{~mol}^{-1}$ ) is $20 \mathrm{~ms}^{-1}$. The average kinetic energy of the same gas at $T(\mathrm{~K})$ (in $\mathrm{J} \mathrm{mol}^{-1}$ ) is

Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is

kept constant. The partial pressures of $A$ and $B$ respectively ( in atm ) are

The RMS velocity of dihydrogen is $\sqrt{7}$ times more than that of dinitrogen. If $T_{\mathrm{H}_2}$ and $T_{\mathrm{N}_2}$ are the temperatures of dihydrogen and dinitrogen, then the correct relationship between them is

Two containers $A$ and $B$ contain $\mathrm{CO}_2$ gas. Pressure, volume and absolute temperature of the gas in $A$ are 4 times more compared to that in $B$. The mass of the gas in $B$ is $x \mathrm{~g}$, then the mass of the gas in $A$ will be

The rate of diffusion of a gas $A$ is $\sqrt{5}$ times more than that of gas $B$. If the molar mass of $A$ is $x \mathrm{~g} \mathrm{~mol}^{-1}$, the molar mass of $B$ (in $\mathrm{g} \mathrm{mol}^{-1}$ ) is

4 g of an ideal gas $A$ (molar mass $=M_A$ ) present in a vessel of volume $V$ litre exerted a pressure of 5 atm at 300 K . When 16 g of another ideal gas $B$(molar mass $=M_B$ ) was introduced into this vessel at the same temperature, its pressure increased to 10 atm . What is the correct relationship between $M_A$ and $M_B$ ?

The ratio of rates of diffusion of gases $X$ and $Y$ of molecular weights 36 and 64 is

Certain volume of oxygen gas diffuses through a porous pot in 20 seconds. Same volume of another gas, $X$ diffuses in $Y$ seconds as that of oxygen, then $X$ and $Y$ respectively are

1 mole of a real gas is kept at high pressure of 100 bar at 300 K . If van der Waals' constant $b$ is $0.005 \mathrm{~L} / \mathrm{mol}$, what are the values of compressibility factor $Z$ of the gas and \% deviation of volume from ideality?

1 L closed flask contains a mixture of 4 g of methane and 4.4 g of carbon dioxide. The pressure inside the flask at $27^{\circ} \mathrm{C}$ is

[assume ideal behaviour of gases].

The rate of diffusion of methane at 1.0 atm pressure is twice than that of another gas ' $X$ ' kept at 1.45 atm . The molecular mass of the gas ' $X$ ' is

Which of the following gases has the maximum van der Waals' constant ' $a$ '?

The compressibility factor of a real gas at high pressure is

The compressibility factor $(\mathrm{Z})$ is lower for $\mathrm{NH}_3$ and $\mathrm{CO}_2$ gases than that of $\mathrm{N}_2$ gas because

A plot of the compressibility factor $(z)$ vs $p$ is shown below for $\mathrm{H}_2, \mathrm{He}, \mathrm{N}_2, \mathrm{CO}_2$ and $\mathrm{SO}_2$. Identify the plot for $\mathrm{CO}_2$ gas.

Dipole-induced dipole interactions are present between which of the following pairs?

A gaseous mixture of 2 moles of $A, 3$ moles of $B$, 5 moles of $C$ and 10 moles of $D$ is contained is contained in a vessel. Assuming that gases are ideal and partial pressure of $C$ is 1.5 atm , the total pressure is

Gases deviate from ideal behaviour at high pressures because the gas molecules

According to kinetic molecular theory of gases, which of the following statements are correct?

(A) The actual volume of the molecules is negligible in comparison to the empty space between them.

(B) Collisions of gas molecules are inelastic.

(C) At any particular time, different particles in the gas have same speed and same kinetic energies.

(D) Pressure is exerted by the gas as a result of collision of the particles with the walls of the container.

Equal amounts of two gases of molecular weights 4 and 40 are mixed. The pressure of the mixture is 1.1 atm . What will be the partial pressure of the lighter gas in the mixture?

Which of the curve ( $Z v s p$ ) will be followed by a real gas?

What is the ratio of kinetic energy of 7 grams of nitrogen and 4 grams of oxygen at $T(\mathrm{~K})$ ?

Equal amount of gases are kept in two separate containers. If densities of the two gases are in $1: 2$ ratio and their temperatures are in 2:1 ratio, calculate the ratio of their respective pressures.

Identify the correct observation with respect to the given graphs.

A gas is present at a pressure of 2 atm . What should be the increase in pressure, so that the volume of the gas can be decreased to $\frac{1}{4}$ th of the initial volume at constant temperature?

Root mean square ( rms ) speed of $\mathrm{O}_2$ is $500 \mathrm{~m} / \mathrm{s}$ at a constant temperature. Calculate the rms speed and the average kinetic energy of $\mathrm{H}_2$ at the same temperature. (Consider, $R=8.33 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ )

Which of the following describes an ideal gas?

(i) The volume occupied by a gas molecule is negligible.

(ii) The collision between ideal gases are elastic.

(iii) Particles are very small compared to the distance between each other.