Deviation from Ideal Behaviour

Van der Waal’s real gas, act as an ideal gas, at which conditions ?

At which one of the following temperature – pressure conditions the deviation of a gas from ideal behaviour is expected to be minimum ?

A gas has a compressibility factor of $0.5$ and a molar volume of $0.4 {\mathrm{dm}}^3 {\mathrm{mol}}^{-1}$ at a temperature of $800 \mathrm{K}$ and pressure $\mathrm{x} \mathrm{atm}$. If it shows ideal gas behaviour at the same temperature and pressure, the molar volume will be  $\mathrm{y} {\mathrm{dm}}^3 {\mathrm{mol}}^{-1}$ . The value of$\mathrm{x}/\mathrm{y}$ is _________

[Use: Gas constant, $\mathrm{R}=8\times {10}^{-2} \mathrm{L} \mathrm{atm} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$ ]

A certain quantity of real gas occupies a volume of $0.15 {\mathrm{dm}}^3$ at $100 \mathrm{atm}$ and $500 \mathrm{K}$ when its compressibility factor is $1.07.$ Its volume at $300 \mathrm{atm}$ and $300 \mathrm{K}$ (When its compressibility factor is $1.4$) is $\_\_\_\_\_\_\times {10}^{-4}{\mathrm{dm}}^3$(Nearest integer)

A gas at $350 \mathrm{K}$and $15 \mathrm{bar}$ has molar volume $20$percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor $\left(\mathrm{Z}\right)$ is :

For which of the following gases, the value of Z is greater than 1 at all pressures and at 273 K?

Following data is given for ${\mathrm{N}}_2$
$\mathrm{P}=800 \mathrm{atm}, \mathrm{Z} = 1.95, \mathrm{T}= 50°\mathrm{C}$
Calculate the mass (g) of ${\mathrm{N}}_2$ required to fill 500 mL flask under these conditions.
$[\mathrm{R}=.0821 \mathrm{atm} \mathrm{litre} {\mathrm{mole}}^{-1}{\mathrm{K}}^{-1})$

Consider the following statements :

I. Density and molar mass of gaseous substance are related as $\mathrm{M}=\frac{\mathrm{dRT}}{\mathrm{p}}$

II. Partial pressure in terms of molefraction is related as ${\mathrm{p}}_{\mathrm{i}}={\mathrm{\chi }}_{\mathrm{i}} {\mathrm{p}}_{\mathrm{total}}$

III. At constant temperature, $\mathrm{pV} \mathrm{vs} \mathrm{p}$ plot for real gases is a straight line 

IV. Real gases do not follow ideal gas equation perfectly under all conditions

Choose the correct statements and select the correct option

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

At $300 \mathrm{K}$ and $100$ bar pressure, the measured volume of $5$ mole of a gas is $2 \mathrm{L}$. The van der Waals constant $\mathrm{b}$ and compressibility factor $\mathrm{Z}$, respectively are

Among the gases $\mathrm{a}, \mathrm{b}, \mathrm{c}, \mathrm{d}, \mathrm{e}$ and $\mathrm{f}$, the gases that show only positive deviation from ideal behavior at all pressures in the graph are

Ideal gas is an imaginary gas but real gas deviate from ideal gas behaviour. How is it possible?

In the following isotherms, $\mathrm{I}$ (for ideal gas) and II (for real gas), points $\mathrm{X}$ and $\mathrm{Y}$ on $\mathrm{II}$ with respect to I indicate _____ deviation

Select the incorrect statement(s):

Gases are compressible because

Why gases are compressible?

The internal energy per mole of an ideal gas is denoted by ${\mathrm{E}}_{\mathrm{ideal}}$. The same for a real gas obeying van der Waals equation is ${\mathrm{E}}_{\mathrm{real}}$. Assuming the average kinetic energy of the molecules of the two gases at the same temperature to be equal, the correct statement for the gas at low pressure is

Regarding ${\mathrm{H}}_2$ gas, the correct statement(s) is/are

The correct statement(s) regarding compressibility factor $\left(\mathrm{Z}\right)$ is/are