(C) The Van der Waals constant '$a$' is a measure of the magnitude of the attractive forces between the gas molecules.Greater the value of '$a$',stron

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(C) The Van der Waals constant '$a$' is a measure of the magnitude of the attractive forces between the gas molecules.Greater the value of '$a$',stronger are the intermolecular forces of attraction.Stronger intermolecular forces make it easier for a gas to be liquefied.Comparing the given values: $a(NH_3) = 4.170 > a(CH_4) = 2.253 > a(N_2) = 1.390 > a(O_2) = 1.3$.Since $NH_3$ has the highest value of '$a$',it can be most easily liquefied.

Class 11 Chemistry States of Matter Real gases and Vander waal’s equation

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The Van der Waals constant '$a$' for the gases $O_2$,$N_2$,$NH_3$ and $CH_4$ are $1.3$,$1.390$,$4.170$ and $2.253 \ L^2 \ atm \ mol^{-2}$ respectively. The gas which can be most easily liquefied is

IIT 1989 All IIT

A
$O_2$
B
$N_2$
C
$NH_3$
D
$CH_4$

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States of Matter

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Real gases and Vander waal’s equation

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IIT 1989 Paper All IIT years →

For $1$ mol of a real gas kept at constant temperature $T$,the graph of $PV$ vs $P$ intersects the $PV$ axis at $20$. Hence,the temperature $T$ is ($R$ = universal gas constant).

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The graph between $P$ and $V$ below the critical temperature is:

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At high pressure,the van der Waals equation for a real gas reduces to:

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Consider the van der Waals constants,$a$ and $b$,for the following gases:

Gas $Ar$ $Ne$ $Kr$ $Xe$

$a / (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$

$b / (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$

Which gas is expected to have the highest critical temperature?

Gas	$Ar$	$Ne$	$Kr$	$Xe$
$a / (atm \ dm^6 \ mol^{-2})$	$1.3$	$0.2$	$5.1$	$4.1$
$b / (10^{-2} \ dm^3 \ mol^{-1})$	$3.2$	$1.7$	$1.0$	$5.0$

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If the compressibility factor $Z < 1$ at $STP$,what will be the molar volume?

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The Van der Waals constant '$a$' for the gases $O_2$,$N_2$,$NH_3$ and $CH_4$ are $1.3$,$1.390$,$4.170$ and $2.253 \ L^2 \ atm \ mol^{-2}$ respectively. The gas which can be most easily liquefied is

Similar Questions

For $1$ mol of a real gas kept at constant temperature $T$,the graph of $PV$ vs $P$ intersects the $PV$ axis at $20$. Hence,the temperature $T$ is ($R$ = universal gas constant).

The graph between $P$ and $V$ below the critical temperature is:

At high pressure,the van der Waals equation for a real gas reduces to:

Consider the van der Waals constants,$a$ and $b$,for the following gases: Gas $Ar$ $Ne$ $Kr$ $Xe$ $a / (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$ $b / (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$ Which gas is expected to have the highest critical temperature?

If the compressibility factor $Z < 1$ at $STP$,what will be the molar volume?

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Consider the van der Waals constants,$a$ and $b$,for the following gases:

Gas $Ar$ $Ne$ $Kr$ $Xe$

$a / (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$

$b / (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$

Which gas is expected to have the highest critical temperature?