7. Gases

In an ideal gas law experiment, how is the temperature of the hydrogen gas typically determined?

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

Which of the following is closest to the vapor pressure of propanone (acetone) at 45 °C?

A sample of oxygen gas has a volume of 640 mL at a temperature of 23°C. At what temperature (in °C) will the volume of the oxygen be 820 mL, assuming pressure and amount of gas are constant?

A sample of oxygen is collected over water and has a volume of 7.18 mL. The pressure of the collected 'wet' gas is 68.68 kPa and the temperature is 20°C. What will the volume of the 'dry' oxygen be in mL if the pressure is changed to 93.57 kPa, assuming the temperature remains constant?

What is the mass in grams of 185 mL of Freon gas (CCl2F2) at 0.944 atm and 17°C, using the Ideal Gas Law?

Which of the following graphs best represents the relationship between pressure (P) and temperature (T) for a fixed volume of an ideal gas?

Under which of the following conditions does a sample of gas behave most ideally according to the ideal gas law?

When liquid water is converted to water vapor at constant mass, what happens to its volume and mass?

1.636 g of an unknown sulfur oxide gas, SO_x, is in a 0.5 L flask at 1 atm and 25.0 °C. Which is the most likely chemical formula of the compound?

In the context of the Ideal Gas Law, why is it important to remove oil from a low-pressure system operating at 130 °F?

A sample of argon gas has a volume of 0.240 L, a pressure of 0.900 atm, and a temperature of 27.0°C. At what temperature (°C) will the argon have a volume of 80.0 mL and a pressure of 3.20 atm, assuming the amount of gas remains constant?

At what temperature in °C does 250.0 mL of argon gas at 25°C and 1.50 atm occupy a volume of 450.0 mL at a pressure of 1.90 atm, according to the Ideal Gas Law?

An ideal gas expands through an adiabatic process. Which of the following statements is true?

A balloon is inflated to 7.0 L of volume. How many moles of gas does it contain at standard temperature and pressure (STP)?