The isotherms of a gas are shown below:Among | vedclass

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(D) All given statements are correct.$(i)$ At temperatures above the critical temperature $(T_c)$,such as $T_1$,the gas cannot be liquefied by applyin

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$(i), (ii), (iii)$ and $(iv)$

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(D) All given statements are correct.$(i)$ At temperatures above the critical temperature $(T_c)$,such as $T_1$,the gas cannot be liquefied by applying pressure alone.$(ii)$ At $T_2$,point $B$ represents the onset of condensation where the gas begins to liquefy.$(iii)$ $T_c$ (critical temperature) is defined as the highest temperature at which a gas can be liquefied by pressure.$(iv)$ At point $A$,the substance is entirely in the liquid state; further compression leads to a sharp increase in pressure as liquids are nearly incompressible.

Gas	$a$ (atm $L^2$ mol$^{-2}$)	$b$ ($L$ mol$^{-1}$)
$W$	$4.0$	$0.027$
$X$	$8.0$	$0.030$
$Y$	$6.0$	$0.032$
$Z$	$12.0$	$0.027$

Similar Questions

For gases $W, X, Y$ and $Z$,the van der Waals constants are given below. Which gas has the highest critical temperature?
Gas $a$ (atm $L^2$ mol$^{-2}$) $b$ ($L$ mol$^{-1}$)
$W$ $4.0$ $0.027$
$X$ $8.0$ $0.030$
$Y$ $6.0$ $0.032$
$Z$ $12.0$ $0.027$

Critical temperature for carbon dioxide and methane are $31.1^{\circ} C$ and $-81.9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?

Gases can be liquefied by:

The compressibility factor $(Z)$ of a gas at critical state is $(T_c = \frac{8 a}{27 R b}; p_c = \frac{a}{27 b^2}; V_c = 3 b)$.

What is the relationship between the liquefaction of gases,compression,and temperature?

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