Compressibility Factor

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 ?

The isotherms of a gas are shown below :

Among the following,

(i) At ${\mathrm{T}}_1$, the gas cannot be liquefied

(ii) At point $\mathrm{B}$, liquid starts to appear at ${\mathrm{T}}_2$

(ii) ${\mathrm{T}}_{\mathrm{C}}$ is the highest temperature at which the gas can be liquefied

(iv) At point $\mathrm{A}$, a small increase in pressure condenses the whole system to a liquid

The correct statements are :

For an ideal gas, the compressibility factor is

For one mole of a van der Waals' gas, the compressibility factor $Z=\left(\frac{pV}{RT}\right)$ at a fixed volume will certainly decrease, if
[Given : " a " and " b " are standard parameters for van der Waals' gas]
 

Which of the following represents a plot of compressibility factor $\left(\mathrm{Z}\right)$ vs pressure $\left(\mathrm{P}\right)$ at room temperature for ${\mathrm{O}}_2?$

At same temperature and pressure, for $\text{'}\mathrm{n}\text{'}$ moles of both ${\mathrm{H}}_2$ and $\mathrm{He}$ occupied volumes are ${\mathrm{V}}_1$ and ${\mathrm{V}}_2$ respectively. If both gases are non-ideal then,

Compressibility factor $\left(\mathrm{Z}\right)$ of gas at critical conditions :

From given $\mathrm{Z} \mathrm{v}/\mathrm{s} \mathrm{P}$ curve for a gas, select the temperature at which gas will show positive deviation in low pressure region -

At moderate pressure, the compressibility factor for a gas is given by

$\mathrm{Z}=1+0.34\mathrm{P}-\frac{160\mathrm{P}}{\mathrm{T}}(\mathrm{P}$ in bar &  $\mathrm{T}$ in Kelvin $)$

What is the Boyle temperature of gas?

The equation of state for a given gas is $\mathrm{P}(\mathrm{V}-\mathrm{nb})=\mathrm{nRT}$, where $\mathrm{b} \& \mathrm{R}$ are constant, if the pressure and temperature are such that ${\mathrm{V}}_{\mathrm{m}}=11\mathrm{b}$, then what is the compressibility factor of gas in this condition:

The density of steam at $27°\mathrm{C}$ and $8.314\times {10}^4$ pascal is $0.8 \mathrm{kg} {\mathrm{m}}^{-3}$. The compressibility factor would be:

At moderate pressure, the compressibility factor for a gas is given by $\mathrm{Z}=1+0.34\mathrm{P}-\frac{160\mathrm{P}}{\mathrm{T}}(\mathrm{P}$ in bar & $\mathrm{T}$ in Kelvin$)$. What is the Boyle temperature of gas ?

If observed volume of one mole of gas is $32$ litre at a pressure of $10 \mathrm{atm}$ and at temperature of $3000 \mathrm{K},$ then value of compressibility factor $\text{'}\mathrm{Z}\text{'}$ will be :-

At low pressure, van der Waals' equation is reduced to $\left[\mathrm{P}+\frac{\mathrm{a}}{{\mathrm{V}}^2}\right]\mathrm{V}=\mathrm{RT}$. The compressibility factor $\left(\mathrm{Z}\right)$ can be given as:

In the following compressibility factor v/s pressure graph, which is true?

For ${\mathrm{H}}_2$ gas, the compressibility factor, $\mathrm{Z}=\mathrm{PV}/\mathrm{nRT}$ is:

Critical temperature of a gas is ..... Boyle temperature:

At the critical point for ${\mathrm{H}}_2$ gas, value of $\mathrm{Z}=3/8 .$ Then, the value of $\mathrm{Z}$ for the similar conditions of ${\mathrm{CO}}_2, {\mathrm{O}}_2, {\mathrm{SO}}_2$  at their respective critical points will be:

Compressibility factor $\left(\mathrm{Z}\right)$ for ${\mathrm{N}}_2$ at $-23°\mathrm{C}$ and $820 \mathrm{atm}$ pressure is $1.9.$ Find the number of moles of ${\mathrm{N}}_2$ gas required to fill a gas cylinder of $95 \mathrm{L}$ capacity under the given conditions.