1 / 19

Chapter 13 and 14 Review

Chapter 13 and 14 Review. Make sure you come prepared with your foldables and a calculator. The change of a solid directly to a vapor. Evaporation Sublimation Condensation Solidification. All matter consists of tiny particles that are in constant motion. Particle theory

gerald
Download Presentation

Chapter 13 and 14 Review

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chapter 13 and 14 Review Make sure you come prepared with your foldables and a calculator.

  2. The change of a solid directly to a vapor. • Evaporation • Sublimation • Condensation • Solidification

  3. All matter consists of tiny particles that are in constant motion. • Particle theory • Constant motion theory • Kinetic theory • Movement theory

  4. The pressure resulting from the collision of atoms and molecules with objects • Atomic pressure • Molecular pressure • Collision pressure • Atmospheric pressure

  5. The energy an object has due to its movement • Active energy • Kinetic energy • Potential energy • Movement energy

  6. A device that measures the atmospheric pressure • Barometer • Atmometer • Pressure reader • Atmospheric recorder

  7. PV = nRT • Boyle’s Law • Charles’s Law • Combined Law • Ideal Gas Law

  8. For a given mass of a gas at constant temperature, the volume of the gas varies inversely with pressure (P1V1=P2V2) • Boyle’s Law • Charles’s Law • Gay-Lussac’s Law • Combined gas Law

  9. The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. • Graham’s Law of effusion • Combined Gas Law • Dalton’s Law of Partial Pressure • Gay-Lussac’s Law

  10. The escape of gas through a small hole in the container. • Diffusion • Escapism • Porision • Effusion

  11. A measure of how much the volume of matter decreases under pressure. • Shrinkibility • Compressibility • Pressurization • Volumization

  12. SI unit of pressure Pascal (Pa)

  13. What unit of temperature is used to calculate the gas laws? Kelvin (K)

  14. What is 35 degrees Celsius in Kelvin? 308 K

  15. The volume of a gas is .25 L at 340.0 kPa pressure. What will the volume be when the pressure is reduced to 50.0 kPa? 1.7 L

  16. A balloon filled with helium has a volume of 30.0 L at a pressure of 100 kPa and a temperature of 15.0 degrees C. What will the volume of the balloon be if the temperature is increased to 80.0 degrees C?(Pressure is constant) 36.8 L

  17. A rigid container of oxygen gas has a pressure of 340 kPa at a temperature of 713 K. What is the pressure at 273 K? 130 kPa

  18. A gas occupies a volume of .14 L at 35.0 degrees C and 97 kPa. What is the volume at 0 degrees C and 101.3 kPa? T1 = 35.0 + 273 = 308 K P1 = 97 kPa T2 = 0 + 273 = 273 K P2 = 101.3 kPa V1 = .14 L Since you have all three variables you use the combined gas law: V2 = (P1 x V1 x T2)/(T1 x P2) = .12 L

  19. The gaseous product of a reaction is collected in a 25 L container at 27 degrees C. The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container? V = 25 L T = 27 + 273 = 300 K P = 300 kPa R = 8.31 n = ? Grams are not a part of the equation so ignore them. They were added as a distraction. PV=nRT n = (PV)/(RT) = (300 x 25)/(8.31 x 300) = 3 mol

More Related