Measurement and Communication:
1. Complete the following table of prefixes.
Factor
106
Prefix
to
3
O
kil
101
Abbreviation
cV
co..
deci
C
‘o
i0
micro
icr
1012
4 times and obtained the following masses:
25.5g, 29.6g, 23.6g, 27.3g
The actual value is known to be 10.20045g
2. A student weighed a mass
What can be said about the accuracy and precision of the measurements?
-
3.
c’oç c(ç€ (cc)
c cc€
(ceco&
c’)
Write the following numbers in scientific notation with the same number of significant digits.
5Pr)c tDLL
a) 0.000005187
b) 7,247
;2—’iI- ic
&H XO
c)16,140
d)0.0921
4.
Convert the following numbers from scientific notation into decimal form.
L5Q,7coo
a) 4.562 x 106
b) 8.276
5.
x 108
Complete the following calculations. Include all units and don’t forget about sig figs.
a) l.0068g+2.15g+8.3g=
b)21.O5cm— 12.lcm=
c) l.5OxlO2mol
=
3
QCcr
45
110
A.’)) C)
d)
21.8cm x(7.645cm-3.58cm)
6.
Convert
D
432.8g
12
23- LD(3
milliamperes into megaamperes.
.J_
’
\f
(
1
=
1
2
C
E
0
E
c.
a)
C
C)
‘-0
>
J
-
.—
a)
0
C)
a)
C
C
I:
E
-
C
C CC
s-i
C
C
a) C ooj C
NC
I
od
0
Cl)
0)
0
c-)
ci.)
0
a)
o
-
‘
(3
..
ii-
•—‘
30
00
C
L)
0
C)
•.—‘
%)
_)
—
)
w
44
oo
c1
—?-
x
a)
-O
E
-
_)
c
e1
QØE
0
o
cOGO
—
-
N
.0
.,
?2
—
-
-
a)
0
‘-4
C)
0
a)
-
I
0
C
C
0
q
2
1D 0
a)
C
I
a)
a)
$
CO
Cl)
C
C
a)
If
—‘
C
-
a))(
rS)
S
K
c(
cl
-J
C)
C)
N
I!
\.g
.1
0
N—
tI
x.
0
Z
0
a)
o
C
a)
$
0
a)
Cl)
-4
-4
.8
Percentage Composition, Empirical and Molecular Formulae:
1. Write the empirical formula for each of the following compounds.
c) 3
(C0
2
Pb
4
)
a) P
10
0
4
C.\.,
3
C1
2
Mg
b) 4
d) N
0
2
2. Calculate the percentage composition by mass of each of the following compounds.
0 ‘T
8
H
4
a) CO
b) C
2
2
Ho
(7-
-
L\L\
P
—h
%32_>
1oO°
7ç
\ ‘7 \
%Th0
0
/
3. Calculate the percentage composition of the bold species in each of the following cornpounçls.
oj
2
)
3
a) Cu(N0
( b) NaSCN 51120
%o=
9oc\
3
N0
cc
(
—
4. a) A compound has the following composition: 24.24% C, 4.04% H and 71.72% Cl. What is
the empirical formula of the compound?
29eZL4c
coL 2oa\/Zc
CJ4CI
0ç
\
2/o
\
b) If the molecular mass of this compound is 99.5 g/mol, what is the molecular formula?
cccm
tE
-
Cx3SS
z
1Dc)co\ck.
ito
3
q95
5. The molar mass of a compound is 58g/mol. What is the molecular formula of the compound if
the empirical formula is C
?
5
H
2
=
D
Molarity Calculations:
1. If a 4.50g sample of solid NaOH is dissolved to make O.500L of solution, what is the molarity
of the solution?
O5coL
CO
2
Na
?
2. How many grams of 3
CO would be required to produce 400.OmL of O.600M 3
2
Na
O5
4>ic
0
-
OOxJ XL%
25 kiCo
Ji&
3. If 75.7g of Magnesium chloride are mixed with sufficient water to make a O.885M solution,
what is the volume of the solution?
q
D9 L
S0
2
H
?
S0 are needed to prepare 755mL of O.25M 4
2
H
4. How many mL of 16.4 M 4
iI
12L
Chemical Reactions and Equations:
1. Balance and classify the following chemical reactions.
3
a) KN0
b) LCaC
2
12
H
5
c) C
d)
-*
+
e) 2
KOH
I BaCl
+
+
f) LCa(OH)
2
2
CO
O2
0
4
S
2
)H
+
Z
ce-r
+ ±02
202 -* Ca +
+
0
4
S
2
K
2
ZKNO
NHCl
+
3rcfr e?\acccv
O
2
H
ZKC1
—*
—*
2
Zco
+
0
4
S
2
JK
4
jBaSO
+
H
2—NH
O
4
-÷
j)
-*
LNa + ±Zn1
2
—>
3
BF
+
NaI
2
2
±N
+
tZn
4
p\CCQft-fl
0
H
2
+
2
LCaC1
S +2902 —* jC0
9
H
4
0
2
2 + jH
2 + SO
g) jC
5 02
1
Q
2
h) 2C
30 ±L
H
15
2 + 30H
3DC0
i) .
BN +
2
Type of Reaction
Ccx bor
5
RQQ\ccQ
0
2. Classify, complete AND balance the following chemical equations.
)+
8
INi(
a)
I
± Ni ?(JO 5Tc coccc c-r\
i_ C
(aq)
2
)
3
Cu(N0
Type of Reaction
b) LFe(S) + 3
02(g)
c) 2NaCl() -*L\
H2SO4(aq) +
d)
10
-
Oc\X
ZJo
2NaOH(aq)
O2(g)
e) ZC
O(l) + 3
1
H
4
f)
g)
L
Ag(s) +
(g)
2
\C1
‘
(g) +
2
Cl
ZKI(s)
‘
O
1
LQ\-k
5fl2t
c_._2
KC\
)+AgCl(aq)-* J15
5
h)\Fe(
JL
i) ZAgNO3(aq) + 3BaC12(aq)
j)
+
(aq)
2
(aq) + ISr(OH)
3
JBaCO
g)
HsoH(l)+o
2
k)iC
(
1)
\
‘
ç
3
Co
-
KOH(aq)
HNO3(aq) +
COj
‘
Energy of Reactions:
1. Define
ENDOTHERMIC
and EXOTHERMIC reactions.
Endothermic:’\Q S ck
Oec
cc-cN
44 c
cccN
Exothermic:
ih
ceod?on
+c
ccc)
2. Classify the following reactions as either endotherrnic or exothermic.
a) 2C
+02
—
2
2C0
b) N
4 + energy
0
2
+ energy
—*
2
N
+ 202
c)AB+C—*CB+A+56.9kJ
d) AB
+
CD
—*
AD
+
BC
z\H
=
-256.4kJ
CQc
4hQ
Stoichiometry:
1. Ammonia combines with oxygen gas in the following reaction:
+
3
4NH
—
0
2
+4NO
50
*6H
3 are needed to combine with 3.57 moles of 02 gas?
a) How many moles of Nil
2(x
3 were reacted?
b) If 1.5 grams of NO is produced in the above reaction, how many grams of N}1
5J
1me
2.
CO
2
3Na
3
+
3
2FeCI
—*
6NaC1
+
(CO)
2
Fe
3
CO with
2
Na
a) How many grams of NaC1 will be produced from the reaction of O.O8Omoles of 3
‘‘
excess FeC!
?
3
LkcL
.
\Q
3tft(cO3
9
zi
3 would be needed to react with 4.2g of 3
CO
2
Na
?
b) How many grams of FeC1
l2&3S
c
2
I.
O(Oc3 S!UaEj \\-i3
3.
3Mg
+
3
2A1C1
—÷
2
3MgC1
+
io(_o
13 pj
2A1
2 would be formed if 50.OmL of O.200M A1C1
3 is reacted with
a) How many grams of MgC1
excess Mg?
O2Oe
‘-c
,‘34C(Ct,
i3 fr(
1
t
Ci
3
b) How many mL of O.150M A1C1
3 would be needed to react completely with 2.OOg of Mg?
35ij
LP
Excess and Limiting Reagents/Percent Yield:
3
S
2
2Fe
1.
+ 902
—*
3
0
2
2Fe
+
6 SO
2
3 is combined with 4.54g of oxygen gas.
S
2
In a chemical reaction 6.92g of Fe
a) Which reactant is the LIMITING reagent?
3
cO
(D9 ça’L
J
L5
2Fo
o)3i3k
b) How many grams of the EXCESS reactant will be left
y OOZ
9
c
3
over
F 0
after the reaction is complete?
az3 =
32O%
95)
O3-Z3
3 can be formed in this reaction?
0
2
c) How many grams of Fe
\crIo €
, and 7.80g of C are
2
(P0 26.3g of Si0
3
Ca
,
2
)
4 will be produced when 41.5g of 4
2. What mass of P
reacted according to the following balanced equation?
4 + 6CaSiO
3 + 1OCO
2 + 1OC —* P
24
(P0 + 6 Si0
3
Ca
2
)
H
ceo
cc
\( ‘\
(co
3
cQ
cç
L)(
ç)
o
\O
m
3
0
2
2A1
4A1 + 302
A1 would be expected to form in the reaction of
,
3
0
a) How many grams of aluminum oxide, 2
15.Og Al with 18.43g of oxygen gas?
3.
cç
0
\
3
fD
L\
3
c\\
3
—
—
3\
\—
, what would the
3
0
2
3 produced in the reaction was only 22.4g Al
0
2
b) If the actual yield of Al
PERCENT YIELD of the reaction be?