Gaseous State — MCQ Practice

A gas occupies a volume of $2.5\,L$ at $27^{\circ}C$ and $1\,atm$ pressure. If the pressure is increased to $2\,atm$ and the temperature is raised to $127^{\circ}C$, what will be the new volume of the gas?

Which of the following conditions is most favorable for a real gas to behave like an ideal gas?

A mixture of $H_2$ and $O_2$ gases has a total pressure of $1.5\,atm$. If the partial pressure of $H_2$ is $0.9\,atm$, what is the mole fraction of $O_2$ in the mixture?

Which of the following gases will have the highest rate of diffusion at the same temperature and pressure?

At what temperature will the average kinetic energy of $N_2$ molecules be the same as that of $O_2$ molecules at $27^{\circ}C$?

A $10\,L$ container holds $0.5\,mol$ of an ideal gas at $27^{\circ}C$. What is the pressure exerted by the gas? (Given $R = 0.0821\,L\cdot atm\cdot mol^{-1}\cdot K^{-1}$)