7. Gases

Under which conditions do real gases deviate most from ideal gas behavior?

Under which conditions of temperature and pressure does oxygen gas behave least like an ideal gas?

A car tire is initially inflated to a pressure of 2.0 atm at a temperature of 300 K. After driving, the temperature inside the tire increases to 360 K, while the volume and amount of gas remain constant. According to the ideal gas law, what is the new pressure of the tire?

Under which set of conditions do real gases deviate the most from the ideal gas law?

Under which of the following sets of conditions will a real gas most closely approach ideal behavior?

Under which conditions of temperature and pressure does a real gas behave most like an ideal gas?

When the pressure in a beaker containing an ideal gas is lowered at constant temperature, what happens to the volume of the gas according to the ideal gas law?

Which of the following best explains why the pressure of a fixed amount of gas decreases as altitude increases in Earth's atmosphere, assuming temperature remains constant?

At a constant temperature and amount of gas, which of the following relationships between pressure and volume is described by the ideal gas law?

At what temperature (in K) would 2.10 moles of N_2 gas exert a pressure of 1.25 atm in a 25.0 L tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

Using the ideal gas law, what is the volume (in liters) occupied by 2.5 moles of nitrogen gas at a pressure of 1.75 atm and a temperature of 475 K? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

A gas expands from state i to state f in the figure, with the pressure remaining constant. Which equation best describes the relationship between the initial and final volumes and temperatures according to the ideal gas law?

What is the volume of 0.200 mol of an ideal gas at 200. kPa and 400. K? Use the ideal gas law and R = 8.314 L·kPa·mol^{-1}·K^{-1}.

In an ideal gas law experiment, a student collects 0.50 mol of a gas in a 10.0 L container at 300 K. What is the pressure of the gas in atmospheres? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

A sample of nitrogen gas occupies 2.50 L at 300 K and 1.00 atm. If the gas is completely vaporized from liquid nitrogen at its boiling point (77 K), and the pressure remains constant, which of the following equations would you use to determine the heat of vaporization (ΔH_vap) of nitrogen using the Ideal Gas Law and the given data?