If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,what is the pressure of the ideal gas at $546 \ K$ (in $atm$)? $(R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1})$

The density of a gas at $-23 \ ^oC$ temperature and $780 \ \text{torr}$ pressure is $1.40 \ g/L$. Identify the gas.

What is the numerical value of gas constant $R$ in terms of $L \ atm \ K^{-1} \ mol^{-1}$?

What will be the molar volume of nitrogen $(N_2)$ and argon $(Ar)$ at $273.15 \ K$ and $1 \ atm$?

If $20 \ cm^3$ of gas at $1 \ atm$ is expanded to $50 \ cm^3$ at constant $T$,what is the final pressure?

Two containers $A$ and $B$ contain $CO_2$ gas. Pressure, volume, and absolute temperature of the gas in $A$ are $4$ times more compared to that in $B$. If the mass of the gas in $B$ is $x \ g$, then the mass of the gas in $A$ will be: