At $T$ $K$,an ideal gas $(Z)$ present in $V$ $L$ flask exerted a pressure of $16.4$ $atm$. Its concentration is $1$ $mol$ $L^{-1}$. What is the value of $T$ in $K$?

$A$ bubble is at the bottom of a lake of depth $h$. As the bubble rises to the surface,its radius increases by a factor of $3$. If the atmospheric pressure is equal to the pressure exerted by a water column of height $\ell$,then $h$ is equal to:

$A$ bubble of air is underwater at temperature $15^\circ C$ and the pressure $1.5 \ bar$. If the bubble rises to the surface where the temperature is $25^\circ C$ and the pressure is $1.0 \ bar$,what will happen to the volume of the bubble?

$A$ gas occupies $10 \ L$ at $0 \ ^{\circ}C$ and $2 \ atm$ pressure. At what temperature will the pressure in the container be $2.5 \ atm$,assuming the volume remains constant (in $^{\circ}C$)?

If a gas occupies $1 \, L$ volume at atmospheric pressure,what will be the volume of the same amount of gas at $750 \, mm \, Hg$ pressure at the same temperature?

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