1. Kinetic Molecular Theory-KMT Unit 5 Gases Chemistry Students will be able to solve for gases under other conditions besides STP.

2. Kinetic-Molecular Theory KMT explains the assumptions that all gas laws follow. What is an “ideal gas”?

3. Main Tenets of Kinetic-Molecular Theory 1.Gas molecules are dimensionless points with no volume.

4. 2. Gas molecules move in straight line motion.

5. 3. Collisions are perfectly elastic.

6. 4. Gas molecules do not attract or repel each other.

7. Why are all gas laws based upon the ideal gas that does not exist? Real gases behave like Ideal gases under moderate conditions. What is moderate? High temperature, enough to be a gas Low pressure, still able to behave like gas molecules.

8. Ideal-Gas Equation PV = nRT Pressure in atmospheres Volume in Liters moles Universal gas constant 0.08206 L ·atm K·mole Temp in Kelvin

9. Calculate the volume occupied by 7.40 g of NH 3 at STP.

10. Calculate the pressure of 1.82 moles of a gas in a 5143 mL container at 69.5˚C.

11. What is random molecular motion?

12. How do smells spread out?

13. What’s the difference? EffusionDiffusion The escape of gas molecules through a tiny hole into an evacuated space. The spread of one substance throughout a space or throughout a second substance.

14. Gas Molecules effuse through the holes in a balloon: Faster at ______temperature T = average kinetic energy _____ molecules travel faster than _______molecules

15. When someone standing at one end of a large room opens a bottle of vinegar, it may take several minutes for a person at the other end to smell it. Gas molecules at room temperature move at very high velocities, so what is responsible for the delay in detection? a.The increase in the airspace occupied by vinegar molecules b.The chemical reaction with nerves, which is slower than other sensory processes c.Attractive forces between the air and vinegar molecules d.Random collisions between the air and vinegar molecules Under same conditions of temperature and pressure, which noble gas diffuses most rapidly? Ne Kr Ar Xe Ammonia (NH3) diffuses through the air because the molecules are a.Moving rapidly b.Dissolving quickly c.Traveling slowly d.Expanding steadily