1 / 14

Ch 5: Thermochemistry

Ch 5: Thermochemistry. The relationship between chemical reactions and energy changes involving heat is called thermochemistry. Types of Energy. Potential energy : energy objects posses as a result to position to other objects

halle
Download Presentation

Ch 5: Thermochemistry

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. Ch 5: Thermochemistry The relationship between chemical reactions and energy changes involving heat is called thermochemistry.

  2. Types of Energy Potential energy: energy objects posses as a result to position to other objects Kinetic energy: energy posses by virtue of motion (E=1/2mv2)

  3. Units of Energy Joule = 1kg-m2/s2 1 calorie = 4.184 J 1 Cal = 1000 cal = 1 kcal

  4. System: the focus of study Surroundings: everything else

  5. Energy used to cause an object to move against a force is called work. W = F x d

  6. Heat is the energy transferred from a hotter object to a colder one.(q) Energy is the capacity to do work or transfer heat.(E)

  7. First law of thermodynamics Energy is conserved. E = Efinal - Einitial

  8. E = q + w Anytime work or heat acts on the system it is a positive value. (Vice-versa)

  9. When a process occurs in which the system absorbs heat, it is called endothermic. A process in which the system evolves heat is called exothermic.

  10. Calculate E The system absorbs 77.5 kJ of heat while doing 63.5 kJ of work on the surroundings.

  11. E = 14 kJ Endothermic

  12. How to solve for q q = mct c = the specific heat of the material. H2O = 4.18 J/gK

  13. If a 3.0 g metal is heated to 95oC and added to a cup of water (50g) at 23oC, and the water raises to 30oC, what is the specific heat of the metal?

  14. If 125 mL of water at 88oC is added to 50 mL of water at 30oC, what is the new temperature of the water?

More Related