Ideal Gas Equation — MCQ Practice

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

What is the density of $\text{N}_2$ gas at $227^\circ\text{C}$ and $5.0\,\text{atm}$ pressure? (Given: Molar mass of $\text{N}_2 = 28\,\text{g/mol}$, $R = 0.0821\,\text{L atm mol}^{-1}\text{K}^{-1}$)

A $10\,\text{L}$ container holds $0.5\,\text{mol}$ of an ideal gas at $25^\circ\text{C}$. What is the pressure inside the container? (Given: $R = 0.0821\,\text{L atm mol}^{-1}\text{K}^{-1}$)

Which of the following conditions would cause a real gas to deviate MOST from ideal behavior?

How many moles of an ideal gas are present in a $5.0\,\text{L}$ container at $27^\circ\text{C}$ and $760\,\text{mmHg}$ pressure? (Given: $R = 0.0821\,\text{L atm mol}^{-1}\text{K}^{-1}$)

At STP, $11.2\,\text{L}$ of an ideal gas has a mass of $14\,\text{g}$. What is the molar mass of the gas?