Lab Report 3 Moles
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Lab Report 3
Moles
Name
Abel Abad
1.
Note the average atomic mass of the elements on the nano-balance. Add atoms to the
larger balance until it registers the same number (in g) as the reading on the nano-
balance (in u). Use the
Exponent
slider to help get the correct amount. Stop adding
atoms when the readings on both balances match exactly.
Element
Atomic mass (units)
How many atoms did
you need to add?
Cu
63.546 u
6.0221x10
23
C
12.011 u
6.0221x10
23
S
32.065 u
6.0221x10
23
Al
26.982 u
6.0221x10
23
2.
Select
Copper(I) oxide, Cu
2
O
. Note that Cu
2
O is a compound composed of different
types of ions bonded together. Place the formula unit of Cu
2
O on the nano-balance.
A.
What is the
molar mass
of Cu
2
O?
143.091 u
B.
Add molecules to the larger balance until its reading matches that of the nano-
balance exactly. How many molecules did you need to add?
6.0221x10
23
3.
Complete the following statements using
the number of specific particles
:
A.
1 mole of
any atomic element
contains
6.0221x10
23
particles
B.
1 mole of
any molecular compound
contains
6.0221x10
23
particles
4.
For compounds, it is sometimes necessary to consider the number of atoms of each
element within a compound. Select
Iron (II) chloride.
Note the image in the Gizmo.
A.
How many Fe atoms are within FeCl
2
?
1
B.
How many Cl atoms are within FeCl
2
?
2
C.
Use the nano-balance to find the mass of each of the independent atoms:
Mass of Fe atom:
55.845 u
Mass of Cl atom:
35.453 u
D.
Find the sum of their masses (1 Fe atom + 2 Cl atoms):
126.751 u
Additional Questions
1.
Solve each of the following problems using dimensional analysis (or another method).
Show your work
.
A.
9.23 × 10
23
Al atoms =
1.533
moles of Al
9.23
x
10
23
atoms
6.022
x
10
23
atoms
/
moles
= 1.533 moles of Al
B.
75 g of KMnO
4
=
2.858 x 10
23
formula units of KMnO
4
KMnO
4
= 158.034 g/mol
75
g
158.034
g
mol
x
6.022
x
10
23
atoms
moles
= 2.858 x 10
23
formula units
C. 0.75 moles of CO
2
=
total carbon and oxygen atoms
(0.75 moles)(
6.022
x
10
23
atoms
/
moles
)= 4.517 atoms of CO
2
1.22 atoms of C
3.30 atoms of O
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O STOICHIOMETRY
Using the Avogadro Number
An aluminum atom has a mass of 4.48 × 10
-23
g and a small airplane has a mass of 5000. kg.
Use this information to answer the questions below. Be sure your answers have the correct number of significant digits.
What is the mass of 1 mole of aluminum atoms?
Round your answer to 3 significant digits.
How many moles of aluminum atoms have a mass equal to
the mass of a small airplane?
Round your answer to 3 significant digits.
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How can we find out the formula?
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Question 1 options:
A. The Mole
We will use the analogy of an elephant and its body parts to explore the concept of moles of compounds or elements. The elephant and the carbon tetrachloride, CCl4 molecule are the test cases.
One elephant has one trunk and four legs
One carbon tetrachloride molecule, CCl4, contains one carbon atom and four chlorine atoms
1 amu = 1.6606 x 10-24 g
1 dozen = 12 items
1 mole = 6.022 x 1023 items = Avogadro's Number
Critical Thinking Questions: (Give your answers in terms of a number such as 17 or 3.25 x 1015 trunks)
How many carbon atoms are found in one dozen carbon tetrachloride (CCl4) molecules?
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Sucrose has the molecular formula
C12H22O11. If a sucrose sample
contains 5.0 x 1022 atoms of carbon,
how many molecules of sucrose are
present in the sample?
[?]
molecules C12H22O11
Hint: How many atoms of C are in the sucrose
molecule? Enter the coefficient in the green blank
and the exponent in the yellow blank.
Coefficient (green)
Exponent (yellow)
[?] x 10
mational Academy of Science. All Rights Reserved.
h
F6
✡ a
8
Enter
Home
arrow_forward
+Using Molar Mass and AVO
tab
Part B
Caffeine is a bitter stimulant drug and is found in varying quantities in seeds, leaves, and so on. Its formula is CH10N4O₂. Match the number of moles of each element found in the specified number of moles of caffeine.
Match the numbers in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
► View Available Hint(s)
caps lock
esc
Submit
1
alt
1.2
2.0
4.0
7.0
8.0
10
16
control option
28
F1
Q
A
N
5,388
2
**
F2
W
S
1. There are
2. There are
3. There are
4. There are
JUL
27
X
#3
H
command
80
F3
E
D
$
4
с
mol of carbon in 2.0 mol of caffeine.
mol of nitrogen in 0.30 mol of caffeine.
mol of oxygen in 3.5 mol of caffeine.
mol of hydrogen in 2.8 mol of caffeine.
DOO
000
F4
R
F
%
5
V
F5
T
G
MacBook Air
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B
F6
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18⁰
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Reset Help
tv
F7
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U
*
8
J
F
F8
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9
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O
F9
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X
command
F10
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F11
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option
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Measurements show that unknown compound X has the following composition:
element
iron
0
oxygen
Write the empirical chemical formula of X.
Explanation
JAN
mass %
69.9%
30.0%
Check
#
X
200
S
888
F4
0/
F5
MacBook Air
A
F6
F7
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center
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FB
F9
A
F10
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Match the left column correctly with the right column.
Hg2CL2
molecular element
Silicon dioxide
atomic element
Hydrosulfuric acid
molar mass
HIO4
si O2
NO
mole
Avogadro's Number
H2S
Isotopers
NO2
Germanium
Nitorgen monoxide
O2 gas
periodic acid
metalloid
mercury(I) chloride
Silicon oxide
percent natural abundance
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A molecule contains 16.623% hydrogen, 2.078% oxygen, and no other element
except carbon. What is the empirical formula?
C = 12.01 g/mol
H = 1.01 g/mol
O 16.00 g/mol
Make sure that you use the letter O not the number O for oxygen please! The
computer system will not recognize zero as 'O!
Make sure that your formula has a C first, then a H in the middle, then the oxygen.
You will not be able to do subscripts so If the formula was CH₂O, you will need to
type CH2O
A/
arrow_forward
b
Learning Goal:
To learn how to convert grams to moles and to use the mole to
find the number of atoms in a sample.
The mole (abbreviated mol) is a counting unit used to simplify
calculations that would otherwise involve very large numbers. The
mole is equivalent to the number of carbon atoms in exactly 12 g
of isotopically pure 12C, or 6.02 x 1023. This number is known
as Avogadro's number in honor of Amedeo Avogadro.
"ock
Avogadro's number can be used as a conversion factor between
moles and atoms as shown here:
The molar mass of a substance is the mass of one mole of a
substance and is written in units of grams per mole. The molar
mass of an atom is equivalent to its atomic mass whereas the
molar mass of a substance is equivalent to its formula weight.
esc
!
6.02x10 atoms
1 mole of atoms
1
Q
A
N
@
2
W
S
3
X
2
Control option command
H
80
E
D
$
4
C
Part A
How many moles of atoms are in 5.00 g of 13 C?
Express your answer numerically in moles.
▸ View Available Hint(s)
a
Part B…
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An analytical chemist measures the amount of Elements E, and E₂ in four samples of an unknown Substance X:
mass mass
sample of E₁ of E₂
1
2
3
4
12.2 g 13.8 g
12.5 g
14.4 g
6.1 g
6.9 g
Continue
It's known that X contains no elements other than E, and E.
11.7 g
13.3 g
Using this information, answer the questions in the table below.
Is X a pure substance or a mixture?
If you don't have enough information to decide, choose can't decide.
If you said X is a pure substance, calculate the mass of Element E, the
analytical chemist would find in a new 10.0 g sample of X.
Round your answer to 2 significant digits.
Opure substance
O mixture
O (can't decide)
U
MacBook Air
0
X
Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms
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Pls help, sorry for the trouble, ignore my handwriting
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Show ALL your work. Remember to follow significant digit rules and show proper format in all answers.
NOTE: Record all molar mass values to 2 decimal places.
Question:
Calculate the number of ions in 7.15 g of RbNO3.
arrow_forward
Please and the question below
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F7
1/2 | - 100% + »
c. 132.07 g/mol
d. 29.02 g/mol
e. 89.07 g/mol
(2) How many molecules are in 30.1 g of sulfur dioxide?
a.
1.81 x 10²5
b.
2.83 x 1023
c. 6.02 x 1023
d.
1.02 x 1024
e.
5.00 x 10-23
(3) How many moles of hydrogen are there in 6.50g of ammonia (NH³)?
a. 0.382 mol
b. 1.39 mol
F8
c.
0.215 mol
d. 1.14 mol
e. 2.66 mol
(4) What are the stoichiometric coefficients in the following equation when it is balanced?
SiCl4(s) + H₂O(1)→ H₂SiO3(s) + HCl (g)
a. 1,3,1,3
b. 1,1,3,4
c. 1,4,1,4
d. 1,3,1,4
e. 3,9,1,4
(5) Ammonia is produced by the reaction of nitrogen and hydrogen:
N2(g) + H2(g) → NH3(g)
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*
F10
F11
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LO @
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A sample of 7.55 g of Mg(OH)2 is added to 25.0 mL of 0.195
M HNO3.
Part C
How many moles of Mg(OH)2 are present after the reaction is complete?
Express your answer in moles to three significant figures.
moles Mg(OH)2 =
mol
%3!
Submit
Request Answer
Part D
How many moles of HNO3 are present after the reaction is complete?
Express your answer in moles to three significant figures.
ΑΣΦΦ
mol
moles HNO3 :
Submit
Request Answer
Part E
How many moles of Mg(NO3)2 are present after the reaction is complete?
Express your answer in moles to three significant figures.
ΑΣφ
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Information for Parts B, C, and D
A compound is 80.0% carbon and 20.0%
hydrogen by mass. Assume a 100.-g sample of
this compound.
Part B
How many grams of each element are in this
sample?
Enter the number of grams of carbon
followed by the number of grams of
hydrogen, separated by a comma (e.g.,
30.0,70.0).
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