At $T(\mathrm{~K})$, the $u_{\mathrm{rms}}$ of $\mathrm{CO}_2$ is $412 \mathrm{~ms}^{-1}$. What is its kinetic energy (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) at the same temperature ?

$ \left(\mathrm{CO}_2=44 \mathrm{u}\right) $

Identify the correct graph for an ideal gas $(y$-axis $=$ compressibility factor, $Z: x$-axis $=$ pressure, $p)$

Identify the correct statements from the following:

I. Glass is an extremely viscous liquid.

II. Increase in temperature decreases the surface tension of liquids.

III. Compressibility factor for an ideal gas is zero.

The correct equation for one mole of a real gas is $a, b$ are constants)

$A$ and $B$ are ideal gases. At $T(\mathrm{~K}), 2 \mathrm{~L}$ of ' $A^{\prime}$ 'with a pressure of 1 bar is mixed with 4 L of ' $B$ ' with a pressure $p_B$ bar in a 100 L flash. The pressure exerted by gaseous mixture is 0.1 bar. What is the value of $p_B$ in bar?

126. Consider the following

Statement I If thermal energy is stronger than intermolecular forces, the substance prefers to be in gaseous state.

Statement II At constant temperature, the density of an ideal gas is proportional to its pressure.

The correct answer is

At $27^{\circ} \mathrm{C}, 1 \mathrm{~L}$ of $\mathrm{H}_2$ with a pressure of 1 bar is mixed with 2 L of $\mathrm{O}_2$ with a pressure of 2 bar in a 10 L flask. What is the pressure exerted by gaseous mixture in bar? (Assume $\mathrm{H}_2$ and $\mathrm{O}_2$ as ideal gases)

Choose the incorrect statement from the following.

At $T(\mathrm{~K})$, hydrogen and oxygen gases are mixed in the ratio of $1: 2$ by mass in a closed vessel of volume ' $V$ ' litres. If the total pressure of gaseous mixture is ' $p$ ' atm, the partial pressure of oxygen (in atm) is

At what temperature (in K ) the rms velocity of $\mathrm{SO}_2$ molecules is equal to rms velocity of $\mathrm{O}_2$ molecules at $27^{\circ} \mathrm{C}$ ?

For one mole of an ideal gas an isochore is obtained. The slope of the isochore is $0.082 \mathrm{~atm} \mathrm{~K}^{-1}$. What will be its pressure (in atm) when the temperature is $12.2 \mathrm{~K} ?\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)$

At $\mathrm{T}(\mathrm{K})$, a gaseous mixture contains $\mathrm{H}_2$ and $\mathrm{O}_2$. The total pressure of the mixture is 2 bar. The partial pressure of $\mathrm{H}_2$ is 1.778 bar. What is the weight $(w / w)$ percentage of $\mathrm{H}_2$ in the mixture?

$ \text { Which of the following is correct for an ideal gas? } $

At 256 K , rms speed of $\mathrm{SO}_2$ gas molecules is $3.16 \times 10^2 \mathrm{~ms}^{-1}$. What is the most probable velocity (in $\mathrm{ms}^{-1}$ ) of same gas at same temperature?

Consider the following

Statement-I : If the intermolecular forces are stronger than thermal energy, the substance prefers to be in gaseous state.

Statement-II : Among all elements, the total number of elements available as gases at room temperature is 10 .

The correct answer is

Identify the conditions at which van der Waals' equation of state changes to ideal gas equation.

At STP, a closed vessel contains I mole each of He and $\mathrm{CH}_4$. Through a small hole, 2 L of He and LL of $\mathrm{CH}_4 \mathrm{WHS}$ escaped from vessel in ' $t$ ' minutes. What are the mole fractions of He and $\mathrm{CH}_4$ respectively remaining in the vessel? ( Assume He and $\mathrm{CH}_4$ as ideal gases. At STP one mole of an ideal gas occupies 22.4 L of volume.)

At $T(\mathrm{~K})$, the $p, V$ and $u_{\mathrm{rms}}$ of 1 mole of an ideal gas were measured. The following graph is obtained. What is it slope ( $m$ )?

( $x$-axis $=p V: y$-axis $u_{\mathrm{rms}}^2, M=$ Molar mass $)$

The RMS velocity ( $u_{\mathrm{rms}}$ ) of one mole of an ideal gas was measured at different temperatures and the following graph is obtained. What is the slope $(m)$ of straight line ?

$ \begin{aligned} & \left(X \text {-axis }=T(\mathrm{~K}): Y \text {-axis }=\left(u_{\mathrm{rms}}\right)^2: M=\right.\text { molar mass : } \\ & R=\text { gas constant } \end{aligned} $

Two statements are given below.

Statement I : Viscosity of liquid decreases with increase in temperature.

Statement II : The units of viscosity coefficient are pascal.

The correct answer is

Two statement are given below.

Statement I : The ratio of the molar volume of a gas to that of an ideal gas at constant temperature and pressure is called the compressibility factor.

Statement II : The rms velocity of a gas is directly proportional to square root of $T(\mathrm{~K})$.

The correct answer is

Given below are two statements.

Statement I : Viscosity of liquid decreases with increase in temperature.

Statement II : The units of viscosity are $\mathrm{kg} \mathrm{m}^{-1} \mathrm{~s}^{-1}$.

The correct answer is

Identify the correct variation of pressure and volume of a real gas $(A)$ and an ideal gas ($B$) at constant temperature. $(y=p ; x=V)$

The gaseous mixture used for welding of metals is

Among the gases a, b, c , d, e and f, the gases that show only positive deviation from ideal behaviour at all pressures in the graph are

When the temperature of a gas is increased from $30^{\circ} \mathrm{C}$ to $930^{\circ} \mathrm{C}$, the root mean square speed of the gas would

Three flasks of equal volume contain $\mathrm{CH}_4, \mathrm{CO}_2$ and $\mathrm{Cl}_2$ gases respectively. They will contain equal number of molecules, if

Which among the following statements is/are incorrect regarding real gases?

(i) Their compressibility factor is never equal to unity (Z $\ne$ 1).

(ii) The deviations from ideal behaviour are less at low pressures and high temperatures.

(iii) Intermolecular forces among gas molecules are equal to zero.

(iv) They obey van der Waals’ equation, $pV = nRT$

Among the following the maximum deviation from ideal gas behaviour is expected from

Which of the following graphs correctly represents Boyle’s Law?

The density of an ideal gas can be given by ........, where p, V, M, T and R respectively denote pressure, volume, molar-mass, temperature and universal gas constant.