1. Matter and Energy 1

2. Universe Classified
Matter is the part of the universe that has mass and volume
Energy is the part of the universe that has the ability to do work
Chemistry studies
The properties of different types of matter
The way matter behaves when influenced by other matter and/or energy 3

3. Changes in Matter
Physical Changes are changes to matter that do not result in a change in the fundamental components that make that substance
State Changes – boiling, melting, condensing
A specific substance will be defined by it’s Physical Properties.
Physical changes are accompanied by energy changes! 8

4. Changes in Matter
Chemical Changes involve a change in the fundamental components of the substance
Produce a new substance
Chemical changes are accompanied by energy changes! 8

5. Energy
The capacity to do work

6. Energy can be described in two forms:
Kinetic - The energy of motion
KE = ½ mv2
Temperature is a measure of the average KE.
Potential - Stored energy
Electrical
Chemical
Mechanical

7. Temperature vs. Heat
Heat is that portion of energy in a substance that can be transferred to another substance.
Temperature is the measure of the effects of heat on the volume of the liquid.
Absorbed heat increases random motion. This expands the liquid inside the thermometer.

8. Food Calories Food is stored chemical energy.
Energy is produced by reacting the food we eat with oxygen.
Some of the energy can be used to do work!
We are all familiar with food and food energy. Read the nutritional information on any food product. Calories are everywhere. The study of thermodynamics has lead to our understanding of calorie content in foods.

9. Units of Energy
One calorie is the amount of energy needed to raise the temperature of one gram of water by 1°C
kcal = energy needed to raise the temperature of 1000 g of water 1°C
joule
4.184 J = 1 cal
In nutrition, calories are capitalized
1 Cal = 1 kcal 18

10. Converting Calories to Joules
Convert 60.1 cal to joules 19

11. Quantity Matters with Heat
Mass
50 grams of water will take less heat to boil than 500 grams!
Temperature Change
A 1 K temperature change will take less energy than a 10 K temperature change!

12. Specific Heat The heat needed to raise 1 gram of a pure substance 1 K.
calorie
1 gram of pure water needs 1 calorie of heat to increase 1 K
SHWater = 1 Cal/g K.
joule
1 gram of pure water needs Joules of heat to increase 1 K
SHWater = J/g K.
Not everything reacts to heat with the same temperature change.

13. Exercise Calorimetry Fun
Link to exercise

14. How much heat energy (in joules) is needed to raise the temperature of 7.40 g of water from 29.0°C to 46.0°C
Specific Heat of Water = 4.184
Mass = 7.40 g
Temperature Change = 46.0°C – 29.0°C = 17.0°C
Q = s x m x DT 22

15. A 1. 6 g sample of metal that appears to be gold requires 5
A 1.6 g sample of metal that appears to be gold requires 5.8 J to raise the temperature from 23°C to 41°C. Is the metal pure gold? (SH = 0.13 J/g oC) 23