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(A) The ideal gas equation is $pV = nRT$. Since $V$ and $T$ are constant,$p \propto n$. Therefore,the substance with the least number of moles $(n)$ w

Vedclass · Accepted Answer

$0.0355 \ g$

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(A) The ideal gas equation is $pV = nRT$. Since $V$ and $T$ are constant,$p \propto n$. Therefore,the substance with the least number of moles $(n)$ will exert the least pressure. Note: The molar mass of chlorine gas $(Cl_2)$ is $71 \ g/mol$. $(A)$ $n = \frac{0.0355 \ g}{71 \ g/mol} = 0.0005 \ mol = 5 	imes 10^{-4} \ mol$. $(B)$ $n = \frac{0.071 \ g}{71 \ g/mol} = 0.001 \ mol = 1 	imes 10^{-3} \ mol$. $(C)$ $n = \frac{6.023 	imes 10^{21}}{6.023 	imes 10^{23}} = 0.01 \ mol$. $(D)$ $n = 0.02 \ mol$. Comparing the values,$5 	imes 10^{-4} \ mol$ is the smallest. Thus,$0.0355 \ g$ of chlorine exerts the least pressure.

Column-$I$	Column-$II$
$A$. Hydrogen gas $(P=200 \ atm, T=273 \ K)$	$p$. Compressibility factor $Z \neq 1$
$B$. Hydrogen gas $(P \approx 0, T=273 \ K)$	$q$. Attractive forces are dominant
$C$. $CO_2$ $(P=1 \ atm, T=273 \ K)$	$r$. $PV=nRT$
$D$. Real gas with very large molar volume	$s$. $P(V_m-b)=RT$

In which one of the following,does the given amount of chlorine exert the least pressure in a vessel of capacity $1 \ dm^{3}$ at $273 \ K$?

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