At $27\,^{\circ}C$ temperature and $4\, bar$ pressure,$CO_2$ is filled in a $2\, L$ vessel. Find the pressure if it is filled in a $4\, L$ vessel at $77\,^{\circ}C$ temperature. (in $, bar$)

The vapors of $1 \ g$ of an element occupy $2.5625 \ L$ exerting a pressure of $0.5 \ atm$ at $1000 \ K$. What is the molar mass (in $g \ mol^{-1}$) of the element? (Assume vapors follow ideal gas equation. Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

The density of vapours of a particular volatile diatomic species $A_2$ was found to be $10 \ mg/mL$ at $1 \ atm$ and $273 \ K$. Its atomic weight is given by: [Assume ideal gas behaviour].

At what temperature in $K$ will $28 \ g$ of $N_2$ gas occupy a volume of $10.0 \ L$ at $2.46 \ atm$ pressure?

$N_2$ is found in a $1 \ L$ flask under $100 \ kPa$ pressure and $O_2$ is found in another $3 \ L$ flask under $320 \ kPa$ pressure. If the two flasks are connected,the resultant pressure is $............... \ kPa$.

At temperature $t \, ^oC$,the pressure exerted by $12 \, g$ of an ideal gas in a container of volume $V \, L$ is $1 \, atm$. When the temperature is increased by $10 \, ^oC$ without changing the volume,the pressure increases by $10 \%$. Find the temperature $t$ and volume $V$ in $L$. (Molar mass of the gas = $120 \, g/mol$)