$A$ gas occupies a volume of $300 \ mL$ at $27 \ ^oC$ temperature and $730 \ mm$ pressure. What will be its volume at $STP$ in $mL$ (in $.2$)?

If a gas expands from $20 \ cm^3$ to $50 \ cm^3$ at a constant temperature $(T)$ under a pressure of $1 \ atm$,what will be the final pressure?

If the density of gas $A$ is $1.5$ times that of gas $B$,and the molecular mass of $A$ is $M$,then the molecular mass of $B$ is:

For an ideal gas,the compressibility factor $(Z)$ is

What is the weight of $CH_4$ gas in a $9 \ L$ cylinder at $27 \ ^oC$ temperature and $1 \ atm$ pressure in $g$?

At $400\, K$ temperature,the volume and pressure of a gas are $200\, mL$ and $1.5\, bar$ respectively. Calculate the volume,weight (assuming the gas is $N_2$),and the number of molecules at $STP$. $[R = 8.31 \times 10^{-2}\, L\, bar\, K^{-1}\, mol^{-1}]$.