1 / 18

Chemistry 2009-2010

Chemistry 2009-2010. Final Exam Study Guide. Ideal Gases. Ideal gases are defined according to the KMT. Ideal vs. Real Gases. most gases behave close to the ideal when high temperature – so they have enough KE to overcome attractive forces low pressure – so they are very spread out.

tymon
Télécharger la présentation

Chemistry 2009-2010

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. Chemistry 2009-2010 Final Exam Study Guide

  2. Ideal Gases • Ideal gases are defined according to the KMT

  3. Ideal vs. Real Gases • most gases behave close to the ideal when • high temperature – so they have enough KE to overcome attractive forces • low pressure – so they are very spread out

  4. Conversion • 1 atm = 760 mmHg = 760 torr = 101.325 kPa

  5. Practice Conversions • Convert 0.927 atm to • mmHg • torr • kPa

  6. STP • STP- (standard temperature and pressure) • STP = 273 K or 0 C and 760 Torr or 1 atm

  7. Molar Volume • Standard Molar Volume of Gas • volume of one mole of gas at STP is 22.4L • 22.4 L of any gas has one mole of particles but has different masses • STP is 1 atm and 0°C • If pressure and Temperature are constant the ideal gas law reduces to Avogadro’s Law.

  8. Temperature • Because the temperature of a material acts as “molecular speedometer”. We measure the average kinetic energy (energy of motion) of particles with thermometers. • The measurement of the average kinetic enegry.

  9. Density • Most substances are: • more dense in the liquid state than the gaseous state. • less dense in the liquid state than the solid state. • Most dense in the solid state

  10. Types of Solids • Crystalline solid- consist of crystals, particles arranged in orderly, geometric pattern. • Amorphous solid- one in which the particles are arranged randomly

  11. Solubility Rules • Like dissolves like • Polar solvents will ONLY dissolve polar solutes • Nonpolar solvents will ONLY dissolve nonpolar solutes

  12. Gas in a Liquid • Lack of heat, lack of motion and increase in pressure – help gas dissolve in a liquid (think soda pop)

  13. Acid and Base Properties • Acids- Change indicators (blue litmus to red). • Bases- Change indicators (red litmus turns blue).

  14. Neutralization Reaction • Acid + Base = Water + Salt • Neutralization Reaction - a reaction in which an acid and a base react in an aqueous solution to produce a salt and water.

  15. Strong Acid and Bases • STRONG ACIDS AND BASES IONIZE COMPLETELY IN WATER • WEAK ACIDS AND BASES DO NOT IONIZE COMPLETELY IN WATER

  16. pH

  17. Indicators • Substances that are one color in an acid and another in a basic or alkaline solution • Litmus: acids = red, bases = blue • phenolphthalein (PHTH): acids = colorless, bases = pink

  18. Titration Titration is the process of adding a known amount of solution of known concentration to determine the concentration of another solution

More Related