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

The density of oxygen at $STP$ is $1.43 \, g \, L^{-1}$. What will be its density at $27 \, ^\circ C$ temperature and $700 \, torr$ pressure?

Molecular attraction and size of the molecules in a gas are negligible at :-

At $273\,K$,$Pd$ vs $P$ is plotted for various gases $1, 2, 3, 4$. Assuming ideal behaviour for four gases $N_2, He, CO_2$ & $H_2$. The correct combination is [$P$ denotes pressure in atmosphere & $d$ denotes density in $g/L$]

Find the number of moles of $CO_2$ present in a sample occupying $4 \times 10^{-3} \text{ m}^3$ at $1.104 \times 10^5 \text{ Nm}^{-2}$ pressure. Given: $R \times T = 2208 \text{ J mol}^{-1}$. (in $\text{ mole}$)

What is the new temperature of a gas when its initial volume $3 \ dm^3$ at $300 \ K$ is doubled at constant pressure (in $K$)?