$A$ certain sample of gas occupies a volume of $0.2 \ L$ at $0 \ ^oC$ and $1 \ \text{atm}$ pressure. What will be its volume at the same pressure but at $273 \ ^oC$ (in $L$)?

When the applied pressure is $16 \ atm$,the temperature is $27 \ ^oC$,and the volume is $9 \ L$,what will be the weight of $CH_4$ gas in $gm$? (Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

For a fixed amount of gas at constant pressure,provide the plot of volume $(V)$ versus temperature $(T)$ in Kelvin. What does it represent?

In the ideal gas equation,the gas constant $R$ has the dimensions of

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 $, g/L$)

$A$ 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