What is the volume of a gas at $1.032 \times 10^5 \ Nm^{-2}$ if it occupies $1 \ dm^3$ of volume at normal temperature and pressure (in $dm^3$)?

The correct gas equation is:

At $300 \ K$,a sample of $3.0 \ g$ of gas $A$ occupies the same volume as $0.2 \ g$ of hydrogen $(H_2)$ at $200 \ K$ at the same pressure. The molar mass of gas $A$ is $...... \ g \ mol^{-1}$ (nearest integer). Assume that the gases behave as ideal gases.

Find the pressure of $5 \ mol$ $Cl_2$ gas filled in a $2 \ L$ vessel at $27 \ ^oC$ temperature. (in $bar$)

$A$ balloon filled with an air sample occupies $3 \,L$ volume at $35^{\circ} C$. On lowering the temperature to $T$, the volume decreases to $2.5 \,L$. The temperature $T$ is (in $^{\circ} C$)? [Assume $p$-constant]

For an ideal gas,what is the nature of the $pV$ versus $p$ graph at a constant temperature?