(A) In the graph of compressibility factor $Z$ versus pressure $P$,a positive deviation from ideal behavior occurs when $Z > 1$. This indicates that t

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(A) In the graph of compressibility factor $Z$ versus pressure $P$,a positive deviation from ideal behavior occurs when $Z > 1$. This indicates that the gas is less compressible than an ideal gas. From the given graph,the curves for gases $a$,$b$,and $c$ lie entirely above the line $Z = 1$ for all pressures. Therefore,gases $a$,$b$,and $c$ show only positive deviation from ideal behavior.

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

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

AP EAMCET 2022 All AP EAMCET

A
$a$,$b$,$c$ only
B
$b$,$c$ only
C
$d$,$e$ only
D
$d$,$e$,$f$ only

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States of Matter

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Real gases and Vander waal’s equation

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For the following gases,the values of $'a'$ (van der Waals constant) are given in parentheses: $CH_4 (2.25)$,$N_2 (1.35)$,$O_2 (1.36)$,and $CO (1.46)$. Which gas will be the most difficult to liquefy?

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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

MediumIIT 1989

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The units of constant $a$ in the Van der Waals equation are:

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

MediumAIIMS 2019

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The pressure of real gases is less than that of ideal gas because of:

EasyKCET 2017

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

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For the following gases,the values of $'a'$ (van der Waals constant) are given in parentheses: $CH_4 (2.25)$,$N_2 (1.35)$,$O_2 (1.36)$,and $CO (1.46)$. Which gas will be the most difficult to liquefy?

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

The units of constant $a$ in the Van der Waals equation are:

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?

The pressure of real gases is less than that of ideal gas because of:

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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?