Unit 5: Gases

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Across
  1. 3. A measurement of the amount of gas particles
  2. 8. @STP 1 mol of gases equals this volume(in liters).
  3. 11. STP(Temp = 273K, Pressure = 1.0 atm)
  4. 12. these types of gases do not exist naturally, because they require conditions to be constant.
  5. 16. The individual pressure exerted by a gas in a mixture.
  6. 17. P1V1 = P2V2
  7. 18. Amount of energy required for a chemical reaction to take place.
  8. 20. relationship between volume and temperature.
  9. 21. Distance between gas particles
Down
  1. 1. P(total) = P1 + P2 + P3
  2. 2. Collision of gas particles against a surface.
  3. 4. Rounded value for the universal gas constant(R).
  4. 5. "Energy is being absorbed, therefore, the reaction feels cold."
  5. 6. can be found by taking the moles of an individual gas, and dividing it by the total number of moles in the sample.
  6. 7. Substance that speeds up a chemical reaction, by lowering the activation energy.
  7. 9. "Energy is being released. Therefore, the reaction feels hot."
  8. 10. V1/T1 = V2/V2
  9. 13. represents the overall change in thermal energy. If positive, the reaction is endothermic. If negative, the reaction is exothermic.
  10. 14. relationship between pressure and volume.
  11. 15. Movement between atoms (kinetic energy)
  12. 19. PV = nRT