At $0\, ^\circ C$,$4\, g$ of $O_2$ and $2\, g$ of $H_2$ are filled in a $1\, L$ bulb. What will be the total pressure of the mixture (in $, atm$)?

Calculate the number of moles of the gas having volume $2.5 \ L$ at $300 \ K$ and $4.5 \ atm$? $(R=0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1})$

$A$ certain mass of a gas occupies a volume of $2 \ dm^{3}$ at $STP$. At what temperature will the volume of the gas become double,keeping the pressure constant (in $^{\circ} C$)?

Match the following graphs of an ideal gas with their respective axes ($X$ and $Y$).
$(A)$ $P$ vs $V$ (at constant $T$)
$(B)$ $V$ vs $T$ (at constant $P$)
$(C)$ $P$ vs $T$ (at constant $V$)
List-$I$:
$(1)$ $P$ on $Y$-axis,$T$ on $X$-axis
$(2)$ $P$ on $Y$-axis,$1/V$ on $X$-axis
$(3)$ $V$ on $Y$-axis,$T$ on $X$-axis

State Avogadro's Law and Gay-Lussac's Law.

At $400 \, K$ temperature,$200 \, mL$ of $N_2$ gas has a pressure of $1.5 \, bar$. Find the volume of $N_2$ gas at $STP$. (in $, mL$)