SUMMER INSTITUTE – Module 3 – Intro to Energy
______________________________________________________________________________________________________________________________________ Jump to: Activity 1, Activity 2, Activity 3, Activity 4, Activity 5, Activity 6, Activity 7, Module Test
Module 3 – Intro to Energy –
5 hours – due July 17th!
| 2011 edition reference tables.pdf
|For viewing on screen|
| 2011 edition reference tables printable.pdf
|For Printing as a Hard Copy|
Now that we understand the differences between all types of matter we need to begin our discussion in the energy changes that occur between physical and chemical changes in matter. Remember that all matter will have preferred low energy states. Things in nature tend to move toward more stability (LOW Energy) by releasing their extra energy but can also move to less stable states in energy (High Energy) when energy is available to be consumed (or absorbed).
Activity 1: SKILL : Energy introduction overview: units Joules, calories, stability and energy, chemical changes and physical changes of energy, Exothermic (like exergonic) and Endothermic (like endergonic), ∆H and Table I (in reference table).
1 : Lecture 1.10 – Energy Intro
2 : Energy – Intro – Presentation
1 : Instructions of how to complete graphing assignment:
Activity 3: SKILL: Temperature and its scales.
1 : Conservation Energy Demo – Steam to Electricity!
2 : Conservation of Energy Demo – Hero’s Engine
1: Please watch the lecture 1.12 – Temperature below on the basics of temperature up to 15:40.
1 : Lecture 1.12 – Temperature
2 : Lecture 1.11 – Temperature Scales
1 : Lecture 1.13 – Temperature to Calorimetry math problems
Why doesn’t the the paper cup just burn (combust or react with oxygen)?
1. melting the white solid: KClO3(s) + heat —> KClO3(l)
2. hot liquid reacts: 2KClO3(l) + heat —> 2 KCl(s) + 3 O2(g)
3. Sucrose (table sugar in gummi bear reacts with oxygen:
C12H22O11 + 35/2 O2 —> 12CO2 + 11H2O + heat (5635 kJ) sucrose
Energy + Sr(OH)2 • 8 H2O (s) + 2 NH4SCN (s) —> Sr(SCN)2 (s) + 10 H2O (l) + 2 NH3 (g)
H2O (l) —> H2O (s) + Energy
The energy absorbed endothermically by the first reaction was taken away from the water (who released it exothermically to the first reaction! I hope this does not board you!
The Cool and “up lifting demo!!”:
Activity 5: SKILL Advanced Calorimetry problems –
1 : Lecture 1.13B – Honors Expanded Calorimetry problems
1 : Calorimetry of a Cheeto Lab
Module Test 3 – available below