Metric Conversion I Chemistry

Front 1

deka

Back 1

10

Hint 1

Deka (gram,liter,meter)

Front 2

Kilo

Back 2

10^3

1000grams

Hint 2

1000

Front 3

deci

Back 3

10^-1

/10grams

Hint 3

0.1

Front 4

Centi

Back 4

10^-2

Hint 4

1g=100centi grams

Front 5

Milli

Back 5

10^-3

Hint 5

0.001

Front 6

Micro

Back 6

10^-6

Front 7

Nano

Back 7

10^-9

Front 8

Pico

Back 8

10^-12

Front 9

femto

Back 9

10^-15

Front 10

hecto

Back 10

100

Front 11

Kilo

Back 11

1000

Front 12

mega

Back 12

10^6

Front 13

giga

Back 13

10^9

Front 14

tera

Back 14

10^12

Front 15

peta

Back 15

10^15

Front 16

Meter-inch

Back 16

39 inches

Front 17

Kilogram (kg) to lb

Back 17

2.2 lbs

Front 18

1kilogram

Back 18

1000 grams

Front 19

Density

Back 19

D=m/v

Hint 19

Density is equal to the mass divided by volume

Front 20

Mg to mcg

Back 20

1mg =1000mcg

Front 21

Percent error

Back 21

Percent error= measured value- Accepted value,Divided by accepted value, multiplied by 100.

Answer %

Hint 21

Percent error= mv - Av / Av * 100. Answer given in percent.

Front 22

C-kelvin

Back 22

C=0

F=32

K=273

Hint 22

C-k

C- 273= K

Front 23

1pt = 473ml

Back 23

1pt/473ml

Front 24

Pure substance

Back 24

Matter that has a fixed or definite composition

There are two types of pure substance: elements and compounds

Front 25

Element

Back 25

The simplest type of a pure substance.

Composed only of one type atom (silver, iron)

Front 26

1ml= 1cm^3

Back 26

1ml = 1cm^3

Front 27

Peta P

Back 27

P=10^15

Front 28

Tera

Back 28

10^12

Front 29

Giga

Back 29

G = 10^9

Front 30

Mega

Back 30

M= 10^6

Front 31

Kilo

Back 31

K= 10^3

Front 32

1 m = mm

Back 32

1m= 1000mm

Front 33

1km= m

Back 33

1km=1000m

Front 34

Deciliter to Milliliter

Back 34

dL to L then L to ml

Hint 34

10dl = 1L

1L= 1000ml

Front 35

1cc= 1.0 ml

Back 35

1000cm^3 = 1000ml = 1 L

Front 36

1gal = 3.784 L

Back 36

3.784 L = 1 gal

Front 37

Specific gravity

Back 37

specific gravity = grams \ mL

Hint 37

D=g/ml. D=mass/volume

Front 38

Mixtures

Back 38

Can’t be physically separated

Front 39

Distillation

Back 39

Separation of mixture is using heat

Hint 39

Alcohol And water

Front 40

ChromaGraph

Back 40

Used to separate color compounds

Front 41

Chemical separation

Back 41

Pure substances can be chemically separated

Front 42

Mole

Back 42

6.02x10^23

Hint 42

1mole of anything is 6.02x10^23

Front 43

The law of conservation of matter

Back 43

Which states that matter cannot be created or destroyed, only change form.

Hint 43

Balance equations

Front 44

Methane gas

Back 44

CH4

Front 45

Mass calculations for reactions

Back 45

Step 1write the equation.

step 2 write a plan to convert the given to the Needed quality

Step 3 . Use the coefficients to write multiple factors, write molar mass factors if needed

Step four. Set up the problem to give the Needed quantity (grams)

Front 46

Law of conservation of matter

Back 46

Matter cannot be created or destroyed, it can only change form

Front 47

NH3

Ammonia

Back 47

Nitrogen tri hydride (ammonia)

Front 48

N2 O5

Back 48

Di nitrogen Pent Oxide

Front 49

SO2

Back 49

Sulfur di Oxide

Front 50

N2 O3

Back 50

Di Nitrogen tri oxide

Front 51

P CL3

Back 51

Phosphorus trichloride

Front 52

S Cl 6

Back 52

Sulfur hexa chloride

Front 53

Stoichiometry

Back 53

Mole ratio theory