If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,the pressure must be ............. $atm$.

Calculate the density of a gaseous mixture which consists of $3.01 \times 10^{24}$ molecules of $N_2$ and $32 \ g$ of $O_2$ gas at $3 \ atm$ pressure and $860 \ K$ temperature. (Given: $R = 1/12 \ atm \ L \ mol^{-1} \ K^{-1}$) ............. $g/L$

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

At $298 \, K$ temperature,$4 \, g$ of $H_2$ gas is filled in a $500 \, mL$ vessel. Due to a small hole in the vessel,after some time,the pressure in the vessel becomes $50 \, bar$. Find the number of $H_2$ molecules that have escaped from the vessel? $(R = 8.314 \times 10^{-2} \, L \, bar \, mol^{-1} \, K^{-1})$

At $300 \ K$,$22 \ g$ of $CO_2$ gas exerts a pressure of $5 \ atm$. What is the volume of the gas at the same temperature (in $dm^3$)? $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

The pressure and temperature of $4 \ dm^3$ of carbon dioxide gas are doubled. Then the volume of carbon dioxide gas would be ............. $dm^3$.