The density of a gas at $27\,^oC$ and $1\, atm$ is $d$. At constant pressure,which of the following temperatures will result in a gas density of $0.75\, d$?

$A$ container of volume $2.24 \, L$ can withstand a maximum pressure of $2 \, atm$ at $298 \, K$ before exploding. The maximum amount of nitrogen (in $g$) that can be safely put in this container at this temperature is closest to

$A$ dry gas occupied $127.4 \, mL$ at $STP$. If the same mass of the gas is collected over water at $27 \, ^\circ C$ and at a total pressure of $725 \, torr$,what volume does it occupy? The vapour pressure of water at $27 \, ^\circ C$ is $25 \, torr$. (Note: $1 \, bar = 750 \, torr$)

$A$ 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:

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?

The correct value of the gas constant $R$ is close to