The graph of pressure $(P)$ versus density $(d)$ is shown for an ideal gas at two temperatures $T_1$ and $T_2$. Which of the following is correct?

If $P$,$V$,$M$,$T$ and $R$ are pressure,volume,molar mass,temperature and gas constant respectively,then for an ideal gas,the density is given by

$A$ 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:

At $1 \text{ atm}$ pressure and $0 \, ^oC$,a certain mass of a gas occupies $0.4 \, L$. Keeping the pressure constant,if the temperature is increased to $273 \, ^oC$,what will be its final volume (in $, L$)?

What is the relationship between the mass and volume of a gas?

Calculate the final volume of a gas when the pressure of $60 \ mL$ of gas is increased from $1 \ atm$ to $1.5 \ atm$,keeping the temperature constant.