$3.4$ moles of an ideal gas occupies a volume of $68 \ mL$ at $300 \ K$. What would be the pressure of the gas? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

$N_2$ gas at $100 \, kPa$ pressure is filled in a $1 \, L$ flask and $O_2$ gas at $320 \, kPa$ pressure is filled in another $3 \, L$ flask. If both flasks are connected,what will be the resultant pressure in $kPa$?

At what pressure will a quantity of gas occupy a volume of $60 \, mL$,if it occupies a volume of $100 \, mL$ at a pressure of $720 \, mm$ (assuming temperature is constant)?

For one mole of an ideal gas, the slope of $V$ vs. $T$ curve at a constant pressure of $2 \ atm$ is $X \ L \ mol^{-1} \ K^{-1}$. The value of the ideal universal gas constant '$R$' in terms of $X$ is

$34.05 \, mL$ of phosphorus vapour weighs $0.0625 \, g$ at $546^{\circ} C$ and $0.1 \, bar$ pressure. What is the molar mass of phosphorus?

$A$ monoatomic ideal gas,initially at temperature $T_1$,is enclosed in a cylinder fitted with a frictionless piston. The gas is allowed to expand adiabatically to a temperature $T_2$ by releasing the piston suddenly. $L_1$ and $L_2$ are the lengths of the gas columns before and after the expansion,respectively. The ratio $\frac{T_2}{T_1}$ is: