CHEM Cheat Sheet (2)
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CHEM 113 Cheat Sheet
Temperature Conversions:
SI/Metric Prefix Chart
Key Points
Any two things that are equal can be used as a conversion factor
“x”
is used to denote any base unit. Replace “
x”
with the base unit utilized in your problem.
Prefix
Symbol
Relationship to Base Unit (
x
)
x = grams (g), liters(L), meters (m)
Scientific Notation Standard Notation
Tera-
T
1
T
x = 10
12 x
1
T
x
= 1,000,000,000,000x
Giga
G
1
G
x = 10
9 x
1
G
x
= 1,000,000,000x
Mega-
M
1
M
x = 10
6 x
1
M
x
= 1,000,000x
Kilo-
k
1
k
g = 10
3 x
1
k
g
= 1,000x
Hecto-
h
1
h
x = 10
2 x
1
H
x
= 100x
Deca-
da
1
da
x = 10
1 x
1
da
x
= 10x
Base
Units
x = Base Units
x = grams (g), liters(L), meters (m)
Deci-
d
1
d
x = 10
-1 x
1
d
x
= 0.1x
Centi-
c
1
c
x = 10
-2 x
1
c
x
= 0.01x
Milli-
m
1
m
x = 10
-3 x
1
m
x
= 0.001x
Micro-
μ
1
μ
x = 10
-6 x
1
μ
x
= 0.000001x
Nano-
n
1
n
x = 10
-9 x
1
n
x
= 0.000000001x
Pico-
p
1
p
x = 10
-12 x
1
p
x
= 0.000000000001x
CHEM 113 Cheat Sheet
SI/Metric Prefix Chart Usage Help (
values below are in standard notation, but the same applies to scientific notation
)
Length (meters – m)
“
x
” would be replaced with m
Example for kilo (k): 1
k
x = 1,000x would be become 1
k
m = 1,000m
1km = 1,000m can be turned into two conversion factors, 1
km
1000
m
∨
1000
m
1
km
Mass (grams – g)
“
x
” would be replaced with g
Example for milli (m): 1
m
g
= 0.001g would be become 1
m
g
= 0.001g
1
m
g
= 0.001g can be turned into two conversion factors, 1
mg
0.001
g
∨
0.001
g
1
m g
Volume (liter – L)
“
x
” would be replaced with L
Example for micro (μ): 1
μ
L
= 0.000001L would be become 1
μ
L
= 0.000001L
1
μ
L
= 0.000001L can be turned into two conversion factors, 1
µ L
0.000001
L
∨
0.000001
L
1
µL
Inter-system Conversion Factors
Length
1 kilometer (km)
=
0.6214 mile (mi)
1 meter (m)
=
39.37 inches (in.)
1 meter (m)
=
1.094 yards (yd)
1 foot (ft)
=
30.48 centimeters (cm)
1 inch (in.)
=
2.54 centimeters (cm)
Mass
1 kilogram (kg)
=
2.205 pounds (lbs)
1 pound (lb)
=
453.59 grams (g)
1 ounce (oz)
=
28.35 (g)
Volume
1 milliliter (mL)
=
1 cubic centimeter (cm3)
1 liter (L)
=
1.057 quarts (qts)
1 U.S. gallon (gal)
=
3.785 liters (L)
CHEM 113 Cheat Sheet
Electron Filling (
Aufbau Principle
) Chart
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CHEM 113 Cheat Sheet
Electronegativity
Polyatomic Ions
CHEM 113 Cheat Sheet
VESPR Chart
Electron Density
(bonds or lone pairs)
0 Lone Pair
1 Lone Pair
2 Lone Pairs
3 Lone Pairs
2
Geometry
Electron
Linear
Linear
Molecular
Linear
Linear
3
Geometry
Electron
Trigonal Planar
Trigonal Planar
Trigonal Planar
Molecular
Trigonal Planar
Bent
Linear
4
Geometry
Electron
Tetrahedral
Tetrahedral
Tetrahedral
Tetrahedral
Molecular
Tetrahedral
Trigonal pyramidal
Bent
Linear
5
Geometry
Electron
Trigonal Bipyramidal
Trigonal Bipyramidal
Trigonal Bipyramidal
Trigonal Bipyramidal
Molecular
Trigonal Bipyramidal
See Saw
T Shape
Linear
6
Geometry
Electron
Octahedral
Octahedral
Octahedral
Molecular
Octahedral
Square Pyramidal
Square Planar
Stoichiometry: The Molar Key Method
CHEM 113 Cheat Sheet
This Stoichiometry Method
has been developed to aid students in their ability to conduct basic stoichiometric calculations in a single step conversion. This method relies on developing a stoichiometric “Key”
Steps of Method:
1.
Determine what amount you are given
.
2.
Determine what unknown
amount you are trying to find.
3.
Determine the stoichiometric key
s for the given amount
and the unknown amount
. (
The stoichiometric key is simply a visualization of the basic stoichiometric equivalences for any molecule as represented by its molar mass.)
Example: The stoichiometric “Key” for H
2
O
would be,
D ŽůĂƌ
<ĞLJ
ĨŽƌ
H
2
O
D ĂƐƐ;ŐͿ
Atomic Weight (element)
Molecular Weight (molecules)
с
ŵŽů
с
ƚŽŵƐ;ĞůĞŵĞŶƚƐͿ
ŽƌD ŽůĞĐƵůĞƐ
ϭϴϬϭϱ
͘°
Ő
H
2
O
с
ϭŵŽů
H
2
O
с
ϬϮϮdžϭϬ
ϲ͘
Ϯϯ
ƚŽŵƐ
ͬ"D ŽůĞĐƵůĞƐ
H
2
O
4.
Create a coefficient conversion template
using coefficients from the chemical equation
. Place the given on the bottom and the unknown on the top.
Conversion Template: Givenamount x
unknowncoefficient
(
Key
)
givencoefficient
(
Key
)
= unknown amount
5.
Find the given key
that matches the given units
and the unknown key
that matches the unknown units
and enter them into their key positions. Perform the calculations.
Example 1
: (
Moles to Moles
): How many mols of O
2
are needed to react with 5.21 mols of CH
4
CH
4
(
g
) +
2
O
2
(
g
)
CO
2
(
g
) + 2H
2
O (
l
)
1.
Given
amount (Value you are given) – 5.21 moles CH
4
2.
Unknown
amount - moles of O
2
3.
Stoichiometric Keys
4.
Coefficient conversion template
. (Coefficients from chemical equation are shown in red.)
5.21 mole CH
4
x 2
(
Unknown Key
)
O
2
1
(
GivenKey
)
CH
4
= ? moles O
2
5.
Find the given key
that matches the given units
and the unknown key
that matches the unknown units
and enter them into their key positions. Perform the calculations.
5.21 mole CH
4
x 2
(
mole
)
O
2
1
(
mole
)
CH
4
= ? moles O
2
5.21 mole CH
4
x 2
(
mole
)
O
2
1
(
mole
)
CH
4
= 10.42 moles O
2 *The coefficient in front of CH
4
is an implied “
1
”
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CHEM 113 Cheat Sheet
Example 2
: (
grams to grams
): What mass (g) of NaOH
, would be required to produce 14.2 g of magnesia [Mg(OH)
2
] by the following reaction? MgCl
2
(
aq
) + 2
NaOH
(
aq
) ⟶
Mg(OH)
2
(
s
) + 2NaCl(
aq
)
1.
Given
amount (Value you are given) – 14.2 g Mg(OH)
2
2.
Unknown
amount - ? g NaOH
3.
Stoichiometric Keys
4.
Coefficient conversion template
. (Coefficients from chemical equation are shown in red.)
14.2 g
Mg(OH)
2
x 2
(
Unknown Key
)
NaOH
1
(
Given Key
)
Mg
(
OH
)
2
= ? g
NaOH
5.
Find the given key
that matches the given units
and the unknown key
that matches the unknown units
and enter them into their key positions. Perform the calculations.
14.2 g
Mg(OH)
2 x 2
(
40.0
g
)
NaOH
1
(
53.3
g
)
Mg
(
OH
)
2
= ? g NaOH
; 14.2 g
Mg(OH)
2 x 2
(
40.0
g
)
NaOH
1
(
53.3
g
)
Mg
(
OH
)
2
= 21.3 g NaOH
Example 3
: (
moles to grams
): What mass of oxygen gas, O
2
, from the air is consumed in the combustion of 0.532 moles of octane, C
8
H
18
,
one of the principal components of gasoline? 2
C
8
H
18
+ 25
O
2
16CO
2
+ 18H
2
O
1.
Given
amount (Value you are given) – 0.532 moles C
8
H
18
2.
Unknown
amount - ? g O
2
3.
Stoichiometric Keys
4.
Coefficient conversion template
. (Coefficients from chemical equation are shown in red.)
0.532 moles
C
8
H
18 x 25
(
Unknown Key
)
O
2
2
(
Given Key
)
C
8
H
18
= ? g
O
2
5.
Find the given key
that matches the given units
and the unknown key
that matches the unknown units
and enter them into their key positions. Perform the calculations.
CHEM 113 Cheat Sheet
0.532 moles
C
8
H
18 x 25
(
32.00
g
)
O
2
2
(
mole
)
C
8
H
18
= ? g O
2
;
0.532 moles
C
8
H
18
x 25
(
32.00
g
)
O
2
2
(
mole
)
C
8
H
18
= 213 g O
2
Example 4
: (
grams to molecules
): How many molecules of AgNO
3
would be needed to react with 8.50 g of copper metal, Cu,
in the following reaction?
Cu(
s
)
+ 2
AgNO
3
(
aq
)
2Ag(
s
) + Cu(NO
3
)
2
(
aq
)
1.
Given
amount (Value you are given) – 8.50 g Cu
2.
Unknown
amount - ? molecules AgNO
3
3.
Stoichiometric Keys
4.
Coefficient conversion template
. (Coefficients from chemical equation are shown in red.)
8.50 g
Cu
= 2
(
Unknown Key
)
AgNO
3
1
(
Given Key
)
Cu
= ? molecules
AgNO
3
5.
Find the given key
that matches the given units
and the unknown key
that matches the unknown units
and enter them into their key positions. Perform the calculations.
8.50 g
Cu
x 2
(
6.022
x
10
23
molecules
)
AgNO
3
1
(
63.55
g
)
Cu
= ? molecules
AgNO
3
8.50 g
Cu
x 2
(
6.022
x
10
23
molecules
)
AgNO
3
1
(
63.55
g
)
Cu
= 1.02 x 10
25
molecules AgNO
3
CHEM 113 Cheat Sheet
Units of Pressure
Unit Name and Abbreviation
Definition or Relation to Other Unit
pascal (Pa)
1 Pa = 1 N/m2 recommended IUPAC unit
kilopascal (kPa)
1 kPa = 1000 Pa
pounds per square inch (psi)
14.7 psi = 1atm
atmosphere (atm)
1 atm = 101,325 Pa = 760 torr
bar (bar, or b)
1.01 bar = 1 atm = 101 kPa
torr
760 torr = 1 atm
millimeters of mercury (mm Hg)
1 mm Hg ~1 torr
Gas Laws
V
1
T
1
=
V
2
T
2
P
1
V
1
=P
2
V
2
P
1
V
1
T
1
=
P
2
V
2
T
2
P
Total
= P
A
+ P
B
+ P
C
+ …
PV = nRT
Universal Gas Constants (Common):
R = 0.08206 L atm mol
-1
K
-1
R = 8.314 kPa L mol
-1
K
-1
pH
pH = −log [H
+
]
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Related Questions
Aqueous hydrobromic acid (HBr) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O).
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7.25
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8.91
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olo
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|||
=
O STOICHIOMETRY
Solving for a reactant using a chemical equation
A major component of gasoline is octane (CgH₁8). When octane is burned in air, it chemically reacts with oxygen gas (0₂) to produce carbon dioxide (CO₂)
and water (H₂O).
What mass of oxygen gas is consumed by the reaction of 8.24 g of octane?
Be sure your answer has the correct number of significant digits.
Explanation
Check
X
5
MA
JUL
19
~
tv
0/3
♫
Kir
I
2022 McGraw Hill LLC All Dichte Docenied Torme of Lleo Privacy Center |
A
8 ..ll
d
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(The ? stands for a number the student is going to calculate.)
Fill in the missing part of this equation.
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-7.3 x 10
kg
mol
= ?
Ox10
olo
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the density of aluminum.
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Substance Density (g/mL)
Water
Aluminum 2.72
Chromium
Nickel
Copper
Silver
Lead
Mercury
Gold
Tungsten
Platinum
1.00
16.2 g X
7.25
8.91
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10.50
11.34
13.60
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21.46
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PART 3
A Volumetric Flask
+ A
С —
ALI50
SOA
A 50-mL volumetric flask measures a volume of 50.00 mL. In this experiment, we want to show that
this is true. 50.00 mL is the actual volume measured by this volumetric flask.
EXPERIMENT:
The mass of an empty volumetric flask is measured.
Then water is added to the volumetric flask and the meniscus is adjusted to be at the correct
level.
Then the mass of the volumetric flask and the water is measured.
Finally, the temperature of the water in the volumetric flask is measured.
RESULTS:
Mass of empty volumetric flask = 37.04 g
Mass of volumetric flask and water = 86.83 g
Temperature of the water in the volumetric flask = 23°C
4
Densities of water at different temperatures:
Density of Water at Different Temperatures
(g/cm)
Temp, °C
Density
Temp, °C
Density
Temp, °C
Density
18
0.99862
21
0.99802
24
0.99733
19
0.99844
22
0.99780
25
0.99708
20
0.99823
23
0.99757
26
0.99681
(a) Using the mass of the water measured and the density of the water,…
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- Aqueous hydrobromic acid (HBr) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H2O). Suppose 58. g of hydrobromic acid is mixed with 19.3 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits. gearrow_forwardGaseous ethane (CH₂CH3) will react with gaseous oxygen (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Suppose 0.601 g of ethane is mixed with 2.8 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 3 significant digits. g x10 X 3arrow_forwardYou can calculate cost effectiveness using the following formula: volume of HCI neutralized per dose /cost per dose (formula) If you calculated that your volume of HCl neutralized per dose was 10.22 mL, calculate the cost effectiveness for Brand X. You can directly use the cost per dose you calculated in the previous problem. Do not include a unit in your answer. Report your answer to two decimal places. Brand X antacid: 2 tablets / 500 mg dose 40 tablets / container Cost: $3.75 / containerarrow_forward
- ||| = O STOICHIOMETRY Solving for a reactant using a chemical equation A major component of gasoline is octane (CgH₁8). When octane is burned in air, it chemically reacts with oxygen gas (0₂) to produce carbon dioxide (CO₂) and water (H₂O). What mass of oxygen gas is consumed by the reaction of 8.24 g of octane? Be sure your answer has the correct number of significant digits. Explanation Check X 5 MA JUL 19 ~ tv 0/3 ♫ Kir I 2022 McGraw Hill LLC All Dichte Docenied Torme of Lleo Privacy Center | A 8 ..ll darrow_forwardA student sets up the following equation to convert a measurement. (The ? stands for a number the student is going to calculate.) Fill in the missing part of this equation. 5 mol -7.3 x 10 kg mol = ? Ox10 oloarrow_forwardUse unit analysis to show how to calculate the volume occupied by 16.2 grams of aluminum. See the table below for the density of aluminum. Densities of Some Common Substances Substance Density (g/mL) Water Aluminum 2.72 Chromium Nickel Copper Silver Lead Mercury Gold Tungsten Platinum 1.00 16.2 g X 7.25 8.91 8.94 10.50 11.34 13.60 19.28 19.38 21.46 (number)(unit) mLarrow_forward
- Please answer question 13arrow_forwardPART 3 A Volumetric Flask + A С — ALI50 SOA A 50-mL volumetric flask measures a volume of 50.00 mL. In this experiment, we want to show that this is true. 50.00 mL is the actual volume measured by this volumetric flask. EXPERIMENT: The mass of an empty volumetric flask is measured. Then water is added to the volumetric flask and the meniscus is adjusted to be at the correct level. Then the mass of the volumetric flask and the water is measured. Finally, the temperature of the water in the volumetric flask is measured. RESULTS: Mass of empty volumetric flask = 37.04 g Mass of volumetric flask and water = 86.83 g Temperature of the water in the volumetric flask = 23°C 4 Densities of water at different temperatures: Density of Water at Different Temperatures (g/cm) Temp, °C Density Temp, °C Density Temp, °C Density 18 0.99862 21 0.99802 24 0.99733 19 0.99844 22 0.99780 25 0.99708 20 0.99823 23 0.99757 26 0.99681 (a) Using the mass of the water measured and the density of the water,…arrow_forwardAqueous hydrobromic acid (HBr) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H₂O). Suppose 7.28 g of hydrobromic acid is mixed with 6.6 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 3 significant digits. g x10 X Śarrow_forward
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