If $N_2$ gas is compressed at $2 \text{ atm}$ from $9.0 \text{ L}$ to $3.0 \text{ L}$ at $300 \text{ K}$, find the final pressure at the same temperature. (in $\text{ atm}$)

Calculate the new volume of a gas at constant pressure when temperature is increased to $546 \ K$.
[Initial volume of a gas at $273 \ K$ is $4 \ dm^3$] (in $dm^3$)

$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

Starting out on a trip into the mountains,you inflate the tires on your automobile to a recommended pressure of $3.21 \times 10^5 \ Pa$ on a day when the temperature is $-5.0 \ ^\circ C$. You drive to the beach,where the temperature is $28 \ ^\circ C$. Assume that the volume increased by $3 \%$. What is the final pressure in the tires?

One mole of an ideal gas occupies $12 \ L$ at $297^{\circ} C$. What is the pressure of the gas?

Consider the figure provided. $1 \ mol$ of an ideal gas is kept in a cylinder,fitted with a piston,at the position $A$,at $18^{\circ} C$. If the piston is moved to position $B$,keeping the temperature unchanged,then '$x$' $L \ atm$ work is done in this reversible process. $x=$ . . . . . . $L \ atm$. (nearest integer) [Given : Absolute temperature $=^{\circ} C + 273.15$,$R=0.08206 \ L \ atm \ mol^{-1} \ K^{-1}$]