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 $\text{ atm}$)

At $T \ (K)$ for one mole of an ideal gas,the graph of $P$ (on $y$-axis) and $V^{-1}$ (on $x$-axis) gave a straight line with a slope of $32.8 \ L \ atm \ mol^{-1}$. What is the temperature (in $K$)? $\left(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}\right)$

If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be:

$4 \ g$ of an ideal gas $A$ (molar mass $= M_A$) present in a vessel of a volume $V \ L$ exerted a pressure of $5 \ atm$ at $300 \ K$. When $16 \ g$ of another ideal gas $B$ (molar mass $= M_B$) was introduced into this vessel at the same temperature, the pressure increased to $10 \ atm$. What is the correct relationship between $M_A$ and $M_B$?

$A$ rigid nitrogen tank stored inside a laboratory has a pressure of $30 \ atm$ at $06:00 \ am$ when the temperature is $27^{\circ} C$. At $03:00 \ pm$, when the temperature is $45^{\circ} C$, the pressure in the tank will be $...... \ atm.$ [nearest integer]

When does $Z = 1$ occur?