7. Gases

What is the pressure (in torr) of 2.10 mol of gas in a 7.00 L container at 65.0 °C, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K, 1 atm = 760 torr)

You have a gas sample of carbon dioxide at 298 K in a 2.00 L container containing 0.500 mol of CO_2. Using the ideal gas law, what is the pressure of your gas sample in atm?

Under which of the following conditions do real gases behave most like ideal gases according to the kinetic molecular theory?

According to the ideal gas law, what is the relationship between pressure and temperature when the volume and amount of gas are held constant?

When water in a syringe boils at 43°C, which factor is primarily responsible for this phenomenon according to the Ideal Gas Law?

Which of the following correctly defines the molar volume of an ideal gas at standard temperature and pressure (STP)?

What is the density in g/L of laughing gas, dinitrogen monoxide (N₂O), at a temperature of 321 K and a pressure of 131 kPa, using the Ideal Gas Law?

A container with a movable piston contains 2.0 moles of argon gas. When the volume of the container is 1.5 L, the pressure is 2.4 atm. Calculate the pressure of the container when the piston is raised to give a volume of 2.5 L. Assume the temperature remains constant.

The system volume is 10 L at STP. If the temperature decreases to 30 K, what is the new volume, assuming pressure remains constant?

What is the pressure in a 13.0 L cylinder filled with 45.8 g of oxygen gas (O2) at a temperature of 318 K, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K)

A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112 °C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.80 atm and the temperature to 25 °C, assuming the amount of gas remains constant?

Would the volume be different if the gas was argon (under the same conditions)?

Using the Ideal Gas Law, calculate the number of moles of air in a car tire with an internal volume of 30.0 L, a temperature of 20°C, and a pressure of 3.50 atm.