Chemistry

Reading Assignment CH 10 & CH 11 Gases

CH 10 Pg 329-332

  1. State the Kinetic Molecular Theory:
  2. Apply the KMT to the three states of matter (explain the particle movement in solids, liquids and gases, how do they compare and how do they differ)
  3. What is an ideal gas and why was it developed?
  4. List the five assumptions of the KMT of gases:
  5. What are elastic collisions?
  6. What happens to ideal gases when they get next to each other and what is meant by attractive forces and do ideal gases have attractive forces, do real gases?
  7. What is the formula of KE and explain what each component stands for:
  8. How does temperature and KE compare
  9. What can you tell me about the average KE of all gases under the same conditions, how do heavier gas molecules, in speed, compare to lighter gas molecules?
  10. What is expansion and what properties about gas molecules allow them to expand?
  11. What is fluidity and what properties about gas molecules allow them to flow?
  12. What about gases allows them to have low density?
  13. What is compressibility and what properties about gas molecules allow them to be compressed?
  14. What is diffusion and effusion and what properties about gas molecules allow them to do this?
  15. Explain the main differences between a real gas and an ideal gas.

CH 11 Pg 361-367

  1. Define pressure and state 3 ways in which you can increase the pressure of a gas.
  2. What is the SI meaning of a newton?
  3. What is atmospheric pressure and what can cause that pressure to change?
  4. Why do your ears pop when you drive from low altitude of high altitude?
  5. Is the air pressure higher or lower at higher altitudes and WHY?
  6. What is a barometer and what is the normal air pressure (in mmHg) at sea level on at 0C and what is that pressure called?
  7. What is standard pressure measured in mmHg ______in torr ______in atm ______in kPa ______. (KNOW THESE!!)
  8. What is standard temperature in C ______in K ______. (KNOW THESE!!)
  9. Know how to convert from one pressure to another.
  10. Covert 103.78 kPa to atm.
  11. State Daltons Law of Partial Pressure Ptotal = P1 + P2 + P3 + ……
  12. What is meant by collecting a gas by water displacement or “over water”?
  13. When collecting a gas “over water” and getting a total pressure inside the bottle, why is it VERY important to subtract out the waters vapor pressure from the total pressure to get the pressure of the “dry gas”?
  14. Why is knowing the temperature of the water so important in determining the waters vapor pressure?
  15. If a young chemist collected a gas “over water” with the water temperature of 25.0C and with a total gas pressure of 758.5 mmHg, find the pressure of the “dry gas” using Daltons Law of Partial Pressure.
  16. State and define Boyles Law?
  17. How does pressure and volume relate?
  18. State and define Charles Law?
  19. When plugging in temperature into ANY laws, temperature must be in _____?
  20. Convert 24.4C to K and 332.4K to C
  21. How does volume and temperature relate?
  22. What happens at absolute zero and what is absolute zero in K ______and in C ______.
  23. State and define Gay-Lussac’s Law?
  24. How does pressure and temperature relate?
  25. What is the Combined Gas Law?
  26. State Avogadro’s Law:
  27. What is STP and give those values in mmHg and C.
  28. What is standard molar volume or “molar volume” and one mole of any gas under STP conditions will occupy what volume of gas?
  29. Calculate the moles of 50.0mL of O2 gas at STP.
  30. Calculate the mass of 250.0mL of CO2 gas at STP.
  31. Calculate the total number of oxygen atoms in 2.0L of SO2 gas at STP.
  32. Calculate the volume (mL) of 500.0g of steam at STP.
  33. From the following equation C3H8 + O2 = CO2 + H2O, calculate the volume of carbon dioxide gas produced if 50.0g of C3H8 reacts with excess oxygen at STP.
  34. State the Ideal Gas Law and what does each symbol represent in the equation?
  35. What unit does volume HAVE TO BE IN when using the ideal gas law?
  36. Complete the following table:

Pressure / R
In Atmospheres
In kPa
In mmHg or torr
  1. Using the ideal gas law equation, calculate the moles of 250.0 mL of CO2 gas at 0.75 atm and 25.0C.
  2. Using the ideal gas law equation, calculate the mass of 550.0 mL of CO2 gas at 800.0 mmHg and 75.0C.
  3. Using the ideal gas law equation, calculate the temperature of 25.0g of CO2 gas at 98.3 kPa and occupies 5.0L.
  4. HC only: From the following equation C3H8 + O2 = CO2 + H2O, calculate the mass of water produced when 500.0mL of C3H8 react with excess oxygen. (not at STP)
  5. HC: From the following equation C4H10 + O2 = CO2 + H2O, calculate the volume of CO2 produced when you are given 25.0 g of C4H10 reacting with 5.0L of oxygen. Which reactant is in excess and by how many moles in excess .