General Overview Of Measurement & Problem Solving

Front 1

Mass Units

Back 1

grams

Common Units:
kg, g, dg, mg, mcg, ng

Front 2

Volume Units

Back 2

liters

Common Units:
kL, L, dL, mL, micro-L, nL

Front 3

1mL is the same volume

Back 3

1cm^3 = 1cc

1 cubic centimeter=
1cm x 1cm x 1cm

Front 4

Density of Water at 4 degrees Celsius

Back 4

1g/1mL = 1g/1cc = 1g/1cm^3

Front 5

1L is the same volume

Back 5

10cm x 10cm x 10cm =1000 cc

Front 6

Accuracy (of a measurement)

Back 6

Closeness to accepted value

Front 7

Precision

(of more than 1 measurement)

Back 7

Repeatability of value

(May or may not be *accurate)

Front 8

Temperature units of measure

Back 8

Metric -
degrees Celsius or Centigrade

Kelvin Units

Front 9

Freezing Point of Water (metric)

Back 9

zero degrees C

273 Kelvins

Front 10

(Normal) Boiling Point of Water
(metric)

Back 10

100 degrees C

373 Kelvins

Front 11

How to convert between Kelvin and Celsius Temp Scales

Back 11

Degrees C + 273 = Kelvins

Front 12

How to Convert between Fahrenheit temp scale and Celsius temp scale

Back 12

Degrees F = 9/5 C + 32

100 degrees C = 212 degrees F

Front 13

Density of Water at 4 degrees C

Back 13

1 kg/1L = 1g/1mL

Front 14

1Liter = ? mL

Back 14

1000 mL = ? L

Front 15

0.1 Liter = ? mL

Back 15

100 mL = ? L

Front 16

0.01 Liter = ? mL

Back 16

10 mL = ? L

Front 17

0.001 Liter = ? mL

Back 17

1 mL = 1 cc = 1 cm^3 = ? L

Front 18

0.000,001 L = ? microliters

1 x 10^-6 L

Back 18

1 micro-L = ? L

Front 19

0.000,000,001 L = ? nL

1 x 10^-9 L

Back 19

1 nanoliter = ? L

Front 20

1 kilogram = ? g

Back 20

1000 g = ? kg

1 x 10^3 g

Front 21

1 g = ? mg

Back 21

1000 mg = ? g

Front 22

1 g = ? cg

Back 22

100 cg = ? g

Front 23

1 g = ? dg

Back 23

10 dg = ? g

Front 24

1g = ? mcg

Back 24

1,000,000 mcg = ? g

1 x 10^6 mcg = ?g

Front 25

1 g = ? ng

Back 25

1,000,000,000 ng = ? g

1 x 10^9 ng = ? g

Front 26

Temperature Units (metric)

Back 26

degrees Celsius (Centigrade)

Kelvins

Front 27

Heat Units

Back 27

Calories or Joules

Front 28

1 calorie = ? joules

Back 28

4.18 joules = ? cal

Front 29

1 dietary Calorie = ? calories

Back 29

? dietary Calories=1000 calories

Front 30

1 dozen = 12 things

1 gross = 144 things

1 mole = ? things

Back 30

6.02 x 10^23 things
(usually atoms or molecules)

602000000000000000000000

Front 31

1 mole

Back 31

Avogadro's Number

Front 32

6.02 x 10^23 chemical units

602000000000000000000000

Back 32

Avogadro's Number

Front 33

Gram Atomic Mass (or GAW)

Back 33

Mass in Grams of 1 mole of any element.
(Use the Atomic Weight on the Periodic Table)

Front 34

STP

Back 34

Standard Temperature and Pressure (for gases)

Front 35

STP values for temp & pressure

Back 35

Standard Temp = 0 degrees C

Standard Press = 1 atmosphere

Front 36

Equivalent Pressure Units:

1 atmosphere = ? mm of Hg

Back 36

760 mm of Hg = ? atm

Front 37

Equivalent Pressure Units:

1 atm = ? kilopascals

Back 37

101.3 kPa = ? atm

Front 38

Equivalent Pressure Units:

1 atm = 101.3 kPa =? mm of Hg

Back 38

760 mm of Hg = ? atm = ? kPa

Front 39

760 mm of Hg = ? Torr

Back 39

? mm of Hg = 760 Torr

Front 40

Specific Gravity Units of Measure

Back 40

No units of measure

Front 41

Specific Gravity -

Back 41

Ratio of Density of substance to the density of water

Front 42

DIMENSIONAL ANALYSIS -
powerful method of solving problems involving units of measure

Back 42

LABEL FACTOR METHOD -
powerful method of solving problems involving units of measure

Front 43

Dimensional Analysis A.K.A.
Label Factor uses _______
to solve problems

Back 43

CONVERSION FACTORS

Front 44

CONVERSION FACTOR

Back 44

A ratio of 2 equivalent units.

1 ft/12 in

10^3mL/1L

60s=1 min

Front 45

Each Conversion Factor can be made into 2 ratios

Back 45

12 in/1 ft and 1ft/12 in

1 day/24 hrs & 24 hr/ 1 day

1 mole/ Av# of atoms and

Av # of Atoms/ 1 mole

Front 46

3 Conv Factors For any element:

1 mole /1(Av # of atoms)

1 mole /1(GFM)

1(GFM)/1(Av # of Atoms)

Back 46

3 Reciprocal Conversion Factors:

1(Av # of Atoms)/ 1 mole

1(GFM)/1 mole

1(Av # of Atoms)/1(GFM)

Front 47

Define: Molar Volume

Back 47

volume of 1 mole of any gas at STP conditions

Front 48

Value of Molar Volume for any gas at STP

Back 48

22.4L

Front 49

Conversion Factors for Molar Volume of any GAS:

22.4L / 1 mole of Gas and ?

Back 49

Conversion Factors for Mass of 1 mole of any Gas at STP:

1 mole of Gas / 22.4L = ?

Front 50

2 ft (12 in/1 ft) =24 inches because...

Back 50

Ft cancel out leaving inches

Front 51

2.0 ft (1 ft/12 in) =0.16 ft^2/in)

Back 51

Useless answer because wrong form of conversion factor was used

Front 52

What conversion factor will help you to solve this problem?

5.0 mL = ? L

Back 52

5.0 mL(1L/1000mL) = 0.005L

because mL cancel leaving L.

Front 53

What conversion factor will help you to solve this problem?

2L = ? kL

Back 53

2L (1 kL/1000L) = 0.002 kL

because Liters cancel out

Front 54

How do you solve this problem?

5 mL = ? kL

Back 54

5mL (1L/1000mL)(1kL/1000L)

because 2 conversions factors will convert mL->L & then L->kL

Front 55

5mL(1L/1000mL)(1kL/1000L) =?

Back 55

0.000,005 kL = 5 x 10^-6 kL

Front 56

Why is the following solution wrong?

5mL (1L/1000mL)(1000kL/1L)=?

Back 56

The answer, 5kL, is wrong because the conversion factor

1000 kL = 1 L is not valid.

Front 57

Why is the following solution wrong?
5mL (1000mL/1L)(1kL/1000L)=?

Back 57

The units don't cancel properly. The answer becomes:
5(mL^2)(kL)/L^2

which is mathematical wrong and makes no sense.

Front 58

The reason that both numbers AND UNITS need to be used in problem-solving is:

Back 58

Use of proper numbers AND UNITS will help to insure that the problem will be SET UP CORRECTLY.

Front 59

A critical reason for noticing and using correct units of measure is:

Back 59

"Life and Death"

Remember what happened to Dennis Quaid's twin babies.

Front 60

When using chemicals, read the label ? times.

Back 60

Three (3) times to help avoid errors.

Sodium Chloride (table salt) is
safe to eat. (NaCl)

Sodium Chlorate is inedible. (NaClO3)

Front 61

Milligrams(mg) &
Micrograms(mcg)

are common units of medicine dosages.

How many times bigger is a mg compared to a mcg?

Back 61

1000 times

(Note how easy it is to make a mistake!)

Front 62

Qualitative Vs. Quantitative

means-

Back 62

Qualitative - descriptive using no units of measure.
i.e. tall

Quantitative - uses units of measure

i.e. 6' 4"