Calculate the pressure of $1.5 \ mol$ of gas having volume $3 \ dm^3$ at $300 \ K$ $(R=0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1})$. (in $atm$)

$A$ certain mass of a gas occupies a volume of $2 \ dm^{3}$ at $STP$. At what temperature will the volume of the gas become double,keeping the pressure constant (in $^{\circ} C$)?

When a graph of the product of pressure and volume $(PV)$ versus pressure $(P)$ is plotted for a fixed amount of gas at a constant temperature,what type of line is obtained?

$A$ 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:

If $2.5$ moles of an ideal gas at a certain temperature are allowed to expand isothermally and reversibly from an initial volume of $2$ $dm^3$ to $20$ $dm^3$,the work done by the gas is $-16.5$ $kJ$. The temperature (in $K$) of the gas is (Round off to the nearest value). $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

At $300 \ K$ temperature and $1 \ atm$ pressure,the weight of $1 \ L$ of a gas is $2 \ g$. If the pressure is changed to $0.75 \ atm$,at what temperature in $K$ will the weight of $1 \ L$ of the same gas be $1 \ g$?