Gas Law Theory
According to the Kinetic Molecular Theory, what happens to the average kinetic energy of gas molecules as the temperature of the gas increases.
It increases
A balloon is filled with 2.0 L of air at 300 K. If the balloon is placed in a freezer at 150 K, what will be the new volume of the balloon (assume constant pressure)?
1.0 L
Describe the relationship between pressure and volume in Boyles law. Is it a direct or inverse relationship?
Inverse
A 5.0 L tank contains a gas at a pressure of 2.0 atm. If the gas is compressed into a 1.0 L tank at constant temperature, what is the new pressure?
10.0 atm
Why do real gases deviate from "Ideal" behavior at very high pressure and very low temperature?
At high pressure the volume of the gas particles themselves becomes significant; at low temperature, attractive forced between particles become significant.
300: What is the pressure (in atm) exerted by 0.50 moles of Nitrogen gas in a 10.0 L container at 27°C?
1.23 atm
According to the Graham's law, if you have a mixture of helium and argon at the same temperature, which gas will effuse through a pinhole faster and why?
Helium; lighter gasses move at higher average speeds and effuse faster than heavier gases at the same temperature
A mixture of gases contains O2, N2, and Ar. The total pressure is 800 mmHg. If the partial pressure of O2 is 150 mmHg and N2 is 550 mmHg, what is the partial pressure of Argon?
100 mmHg
Under the KMT, what two assumptions are made about "Ideal" gas particles regarding their volume and their interactions with one another?
2. There are no attractive or repulsive forces between the particles.
A 2.00 g sample of an unknown noble gas occupies 1.12 L at STP (0°C and 1.00 atm). Identify the gas by calculating its molar mass.
Argon (Ar).