What is the density of $SO_2$ gas at $27\,^oC$ temperature and $2\, atm$ pressure in $g/L$? (Atomic weights: $S = 32, O = 16, R = 0.082\, L\, atm\, K^{-1}\, mol^{-1}$)

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

Explain the relationship between pressure,volume,and density of gases.

At $300 \ K$,a sample of $3.0 \ g$ of gas $A$ occupies the same volume as $0.2 \ g$ of hydrogen $(H_2)$ at $200 \ K$ at the same pressure. The molar mass of gas $A$ is $...... \ g \ mol^{-1}$ (nearest integer). Assume that the gases behave as ideal gases.

At $400\, K$ temperature,the volume and pressure of a gas are $200\, mL$ and $1.5\, bar$ respectively. Calculate the volume,weight (assuming the gas is $N_2$),and the number of molecules at $STP$. $[R = 8.31 \times 10^{-2}\, L\, bar\, K^{-1}\, mol^{-1}]$.

At $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be