The compressibility factor $(Z)$ for an ideal gas is ...... .

At $27\,^oC$ temperature in a $2\, L$ closed vessel,$10\, g$ of $H_2$ and $22\, g$ of $CO_2$ gases are filled. Find the partial pressure of each gas and the total pressure of the mixture. (Use $R = 0.08314\, L \cdot bar \cdot K^{-1} \cdot mol^{-1}$ and formula $pV = nRT$)

At a temperature of $27\,^oC$ and a pressure of $1\,atm$,the density of a gas is $d$. At constant pressure,at what temperature will its density become $0.75\,d$?

Density of a gas is found to be $5.46 \, g / dm^3$ at $27^{\circ} C$ at $2 \, bar$ pressure. What will be density at $STP$?

Choose the correct option for the graphical representation of Boyle's law,which shows a graph of pressure vs. volume of a gas at different temperatures:

At $25 \, ^\circ C$,a $3.7 \, g$ gas occupies the same volume as $0.184 \, g$ of $H_2$ gas at $17 \, ^\circ C$ under the same pressure. What is the molar mass of the gas?