Download Mole Unit Review Packet

Name: _________________________________
Period: _______
Date: _____________
Mole Unit Review Packet
Dear my wonderful students,
I hope you all had a wonderful Memorial Day weekend. Sadly I am sick today and cannot make
it to school. In my absence, you will practice some of the topics that we have learned recently. This
packet is due in class on WEDNESDAY, May 28 (tomorrow).
Your To Do List:

Work on this packet during class today

Finish the packet for homework

DO YOUR PRELAB! There are extra copies in the Yesterday’s Homework
folder. It is also posted on my website.
Good luck!
Ms. Eggleston
www.mseggleston.com
[email protected]
SHOW YOUR WORK ON A SEPARATE SHEET OF PAPER!
Solve the problems and match the answers with the solutions and letters below to finish the comic.
“_ _ _ _ _ _ _ _ _ _ _ _ _’_ _ _ _ _ _ _ _.”
1
2
3
4
5
6
7
8
9
10
11 12
13 14
15 16 17 18 19 20 21
Convert to Moles
Convert to Atoms
Convert to grams
1) 3.45 g Na
8) 23 g H2O
15) 4.83 x 1022 atoms Fe
2) 4.32 x 1024 atoms Ni
9) 3.00 mol Na
16) 74 mol W
3) 232. g Ca
10) 9.2 x 10-22 mol S
17) 3.4 x 10-2 mol Mg(OH)2
4) 62.3 g H2CO3
11) 456 g Fe(OH)3
18) 1.03 mol Ar
5) 32 atoms F
12) 5.2 x 10-23 g N
19) 8.00 molecules CH4
6) 10.00 g KCl
13) 83 g Br2
20) 952.0 mol PbSO4
7) 3.01 x 1023 molecules NaCl
14) 7.52 mol Si
21) 3.04 x 1025 molecules H2
L. 1.81 x 1024
***Select the correct numerical answer (the correct units are omitted)***
S. 5.3 x 10-23
A. 4.48
D. 1.36 x 104
L. 550
E. 1.341 x 10-1
O. 1.98
P. 41.1
E. 2.89 x 105
D. 102
P. 1.50 x 10-1
E. 7.69 x 1023
M. 4.53 x1024
A. 1.00
T. 0.500
M. 2.57 x 1024
E. 2.24
E. 5.79
I. 3.12 x1023
T. 2.13 x 10-22
L. 7.18
Percent Composition Practice
𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 × 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡
× 100 = ____________%
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
1. N2S2
N: ___________
S: ___________
2. KMnO4
K: ___________
Mn: ___________
O: ___________
Empirical and Molecular Formula Practice
4. Which is an empirical formula?
a. C6H12O6
b. C2H4NO
c. C2H6
d. All of the above
5. Fill in the blanks:
Percent to ______________, Mass to ________________, Divide by
_________________, Multiply till whole.
6. A compound contains 0.0130 mol carbon, 0.0390 mol hydrogen, and 0.0065 mol oxygen.
What is its empirical formula?
7. A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is its empirical
formula?
STEPS:
Element 1: ___________
Element 2: ___________
1. Convert
from
PERCENT to
MASS
2. Convert
from MASS
to MOLES
3. Divide
both
numbers by
the smallest
number of
moles
4. Multiply
both
numbers by
the same
number so
that they’re
whole
5. Write the
empirical
formula
8. A compound’s empirical formula is C3H7 and its formula mass is 86 g/mole. Find its molecular
formula.
Empirical
Molecular
Formula
Molar Mass
𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑀𝑀
=𝑋
𝐸𝑚𝑝𝑖𝑟𝑖𝑐𝑎𝑙 𝑀𝑀
Multiply each element
in empirical formula
by 𝑋.
9. A compound is 58.8 % C, 9.9 % H, and 31.3 % O. If its formula mass is 306 g/mole, what is the
molecular formula? (Hint: find the empirical formula first, THEN calculate the molecular
formula.)