$60 \ cm^3$ 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

Two flasks of equal volume contain $O_2$ and $CH_3OH$ vapor respectively at $120\,^oC$ and $1.15\, atm$ pressure. Which of the following will be the same for both?

At $STP$,a closed vessel contains $1 \ mole$ each of $He$ and $CH_4$. Through a small hole,$2 \ L$ of $He$ and $1 \ L$ of $CH_4$ escaped from the vessel in '$t$' minutes. What are the mole fractions of $He$ and $CH_4$ respectively remaining in the vessel? (Assume $He$ and $CH_4$ as ideal gases. At $STP$,one mole of an ideal gas occupies $22.4 \ L$ of volume.)

$A$ vessel of volume $1.2 \, L$ contains a gas at $1000 \, torr$ pressure. Another vessel of volume $3.8 \, L$ contains the same gas at $500 \, torr$ pressure. If both vessels are connected by a tube of negligible volume,what will be the resultant pressure in $torr$ when equilibrium is established?

$CH_4$ diffuses two times faster than a gas $X$. The number of molecules present in $32 \ g$ of gas $X$ is ($N$ is Avogadro number).

If hydrogen gas travels a distance of $10.5 \ cm$ in $5 \ s$ through a long narrow tube at a pressure of $1 \ atm$,what distance (in $cm$) will oxygen gas travel in $5 \ s$ at a pressure of $2 \ atm$?