If the density of a gas at $27\,^{\circ}C$ and $2\, atm$ is $5.46\, g/L$,then calculate the density of the gas at $STP$. (in $, g/L$)

Volume of $0.5 \ mole$ of a gas at $1 \ atm$ pressure and $273 \ K$ is ............. $litres$.

$A$ 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

The density of oxygen gas at $5 \text{ atm}$ and $127^{\circ} C$ will be (in $\text{ g/L}$)

$A$ $10 \, L$ cylinder contains $0.4 \, g$ of helium,$1.6 \, g$ of oxygen,and $1.4 \, g$ of nitrogen at $27 \, ^\circ C$. Calculate the total pressure of the mixture and the partial pressure of helium gas. Assume ideal gas behavior. $(R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1})$

For $1 \ mol$ of an ideal gas at a constant temperature $T,$ the plot of $(\log \ P)$ against $(\log \ V)$ is a ($P :$ Pressure,$V:$ Volume)