1. Measurements and Calculations
Chapter 2
Measurements and Calculations

2. II. Matter and Its Properties
-Matter: has mass & occ space
1. Occupy space
2. Experience inertia
*Inertia: resist change

3. *weight: (mass)(gravity)
*mass: amount of matter
*Law of Conservation of Mass

4. -NRG
*ability to do work
*ability to create a force over a distance some time in the future
~Chem deals mostly with
1. Thermal
2. Radiant
3. Electric

5. *kinetic nrg= (.5)(m)(v)2
nrg of motion
*potential nrg= (m)(g)(h)
nrg do to position

6. -Law of Conservation of NRG (1st) -States of Matter 1. Solid 2. Liquid
3. Gas
4. Plasma
**See Website Ex’s**

7. -Properties & Changes
*can be used to classify subst
1. Physical: observ or measure
without alter ident
of the material.
ex: color
2. Chemical: change that alters
ident
ex: burn wood, rust iron

8. *Chem Rxn: pg13
*Reactans yields Products
A + B ----> AB
*Exother: acid + HOH -->heat + ???
*Endother: ice + heat ---> HOH

9. Indicators of Chem Rxn’s
1. Produce heat & light
2. Produce gas
3. Produce precipitate
**K Demo**
*precip.: solid formed from
a solution

10. III. Classification of Matter
-Mixture
*Heterogeneous: pg 16
ex: veg. soup, clay + water
*Homogeneous / Solutions: pg16
ex: air, salt HOH

11. *Homogeneous / Solutions: pg16
ex: air, salt HOH
~components of any mixture can
be separated from each other
by physical methods

12. -Pure Substances
1. Same property
2. Same composition
3. Can not be separated without
changing the ident
ex: electrolysis

13. *element: ex: K, Pb
*chem. Cmpnd:ex: HOH, sugar
*Law of Definite Composition:
ex: CH4
C=75% H=25%

14. IV. Chemical Elements
*Groups: vert
*Periods: horz
-Symbols:

15. -Types of Elements (pg21)
1. Metals:
2. Nonmetals:
3. Metalloids:
4. Noble Gas:

16. II. Units of Measurements
Factor/Label: ex’s
Derived Units
Table 2-3 pp 36

17. Density: = (m) / (v) units??
g/ml
***table 2-4 pp 38**
Volume: = (l) (w) (h) units??
cm3

18. A. Heat and Temp
*Temp:
*Heat:
ex’s: pp

19. -Kelvin:
Freeze:
Boil:
K = (C)
0 K is absolute 0

20. Celsius
Freeze = 0 °C
Boil = 100 °C
° C = (5/9) (F )

21. Fahrenheit:
Freeze = 32 °F
Boil = 212 °F
°F = (9/5) (°C) + 32

22. -Units of Heat
*Joule (J)
*Calorie (c): c = 4.184

23. Paper Cup Demo
#2 (boiling water in a paper cup)

24. Heat Cap. and Spec. Heat
*HC:
pp 513 Fig. 17-1

25. = heat lost or gained (J or Cal) mass(g) X ∆ in Temp (°C)
Spec. Heat
= heat lost or gained (J or Cal)
mass(g) X ∆ in Temp (°C)
Cp = ______q______
(m) (∆ T)

26. Examples
Determine the specific heat of a material if a 35g sample absorbed 48 J as it was heated from 293 K to 313 K.
A: .069 J/(g*K)

27. Examples
2. How much heat is needed to raise the temperature of 5 g of gold by 25 C?
A: 16 J

28. Examples
3. If 980 kJ of energy are added to 6.2 L of water at 291 K, what will the final temperature of the water be?
A: 329 K

29. III. Scientific Measurements
*Accuracy:
*Precision:
ex’s: pp 44
*Percent Error = Valueacc - Valueexp
Valueacc

30. -Proportional Relationships Directly: y/x = k or y = kx
Inversely: xy = k or y = k/x
**ex’s and graphs