The three states of matter are the result of what?

Equal masses of $H_{2(g)}$ and $He_{(g)}$ are enclosed in a container at constant temperature. The ratio of partial pressure of $H_2$ to $He$ is

$60 \ cm^3$ of $SO_2$ gas diffused through a porous membrane in '$x$' min. Under similar conditions $360 \ cm^3$ of another gas (molar mass $4 \ g \ mol^{-1}$) diffused in '$y$' min. The ratio of $x$ and $y$ is

In a closed flask of $5 \ L$,$1.0 \ g$ of $H_2$ is heated from $300 \ K$ to $600 \ K$. Which statement is not correct?

Match gases under specified conditions listed in Column-$I$ with their properties/laws in Column-$II$.

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	$s$. $P(V_m-b)=RT$

$1 \text{ mole}$ of gas $A$ and $1 \text{ mole}$ of gas $B$ at $27^{\circ} C$ were pumped into a $24.6 \ L$ volume pre-evacuated isolated flask. The catalyst coated inside the flask catalyses the following reaction $A_{(g)} + B_{(g)} \longrightarrow 2 D_{(g)}$. The kinetic energy of $D$ is $98.03 \ L \ atm$. Calculate the pressure realized at the end of the reaction. (in $atm$)