Download 1 CHM130/Practice/Measurement Name

CHM130/Practice/Measurement
1.
Name:___________________________
For each of the following, write the scale reading and identify the number of significant figures.
Reading
1
Number of significant figures
2.
For each of the volume devices below record the scale reading.
scale
reading ________
scale
reading ________
uncertainty
________
scale
reading ________
uncertainty
________
9
10
uncertainty
________
11
2
CHM130/Practice Significant Figures/Scientific Notations/Units/Prefixes
Name:____________________________
1.
Identify the number of significant figures in each of the following.
a)
c)
e)
g)
2.
3.
4.
0.003040 cm
34500 g
100. L
2.050 x 10-12 g
_____
_____
_____
_____
b)
d)
f)
h)
1090 mL
1.200 km
0.302 in
35.05 mL
_____
_____
_____
_____
Round off each of the following measurements to the number of significant figures (digits) given in
the parenthesis.
a)
0.0050895 km (4)
___________________
b)
10566 g (3)
___________________
c)
239688 mm (3)
___________________
d)
175000 mL (2)
___________________
e)
89.995 (3)
___________________
Write each of the following numbers in scientific notation.
a) 0.00000980
_____________________________
b) 45000
_____________________________
c) 120.00
_____________________________
d) 0.00002002
_____________________________
Complete the table.
prefix
symbol
c
Numerical value
deci
1,000,000
µ
kilo
10-9
3
5.
Complete the table using the example given.
Abreviation
m
mL
kg
cc
nm
dL
6.
Full name
meter
Type of measurement
length
Complete the following relationship.
a) 1 m = __________ mm
b) 1 L = __________ dL
c) 1 kg = __________ g
d) 1 g = __________ µg
e) 1 in = __________ cm
f)
1 lb. = _________ g
g) 1 m = __________ cm
h)
1 L = __________ mL
4
CHM130
Practice (Measurements/Significant Figures in Calculations)
Name:
1.
Measure the length of a pencil in cm and mm with correct number of significant figures.
__________ cm
___________ mm
2.
Give the answers for the following calculations with the proper number of significant figures.
a)
10.005 + 0.03238 =
b)
9.345 x 3.02 =
c)
12.024 - 2.7890
=
9.000
d)
1967 - 390 =
e)
28 + 0.000348 =
e)
(2.31 x 103) x (3.0 x 105) =
f)
9.32 x 10 8
=
3.11 x 10 3
g)
7.668 x 1010
1.24 x 10 -5
h)
(4.122 x 10-5) x (1.76 x 1012) =
i)
(6.34 x 1034) x (3.325 x 1014) =
=
5
CHM130/Practice /Unit Equations/Conversion factors/Factor-label Method
Name:__________________________
1.
Complete the unit equation and write two corresponding conversion factors for each of the following
in the table.
Unit equation
1 km = _1000_ m
Conversion factors
1 km
1000 m
or
1000 m
1 km
1 cm = ______ m
1 g = ______ mg
1 L = ______ dL
1 cc = _____ 1 mL
2.
Use the appropriate conversion factor to solve the following problems by factor-label method
(dimensional analysis method). Show your work.
a)
26.5 mg = __________ g
b)
12450 cm = __________ m
c)
1.25 km = ___________ m
d)
25.8 dL = ___________ L
6
CHM130/Practice/Factor-Label Method
Name:___________________________
Perform the following conversions by factor-label methods.
example) Convert 1250 g to lb.
i)
plan: identify the given unit (g) and wanted value (lb) :
ii)
equality:
ii)
two conversion factors from equality:
find the unit relationship(s):
g lb
1 lb = 454 g
1 lb
454 g
or
454 g
1 lb
iii) problem-solving: use the appropriate conversion factor from ii) to
cancel the given unit and to obtain the wanted unit.
1250 g
a)
x
1 lb
= 2.75 lb
454 g
76.3 L to dL
i)
ii)
ii)
plan:
equality:
two conversion factors:
iii) problem-solving:
b)
98650 mm to m
i)
ii)
ii)
plan:
equality:
two conversion factors:
iii)
problem-solving:
7
CHM130/Practice/Factor-Label Method
Name:____________________________
Perform the following conversions by factor-label methods.
a)
b)
c)
175 lbs to kg (1 lb = 454 g)
i)
ii)
plan:
conversion factors:
iii)
problem-solving:
0.500 qt to L (4qts = 1 gal,
i)
ii)
plan:
conversion factors:
iii)
problem-solving:
1 gal = 3.784 L)
754000 µm to cm
i)
ii)
plan:
conversion factors
iii)
problem-solving
8
CHM130/Practice/Temperature Conversions/Density
1.
2.
Name:__________________________
Perform the following conversions.
a)
78.0 oF to oC
b)
105 oC to oF
c)
34.5 oC to K
d)
290 K to oC
e)
372 K to oF
f)
98.6 oF to K
A metal has a density of 11.2 g/cm3.
a)
What would be the volume (in cm3) of 96.5 g of the metal?
b)
How many grams would the metal with the volume of 46.5 cm3 weigh?
9
CHM130/Practice/Percent as Conversion Factors
Name:____________________________
Show your work for the following problems.
1.
A solution contains 23.5 grams of sugar and 100.0 grams of water.
a)
Calculate the % sugar by weight.
___________% sugar
b)
Write the conversion factors that can be obtained from the answer in a).
c)
How many grams of this solution would contain 12.8 grams of sugar?
Solve this problem by factor-label method.
__________ g solution
2.
A drink contains 4.5 % of real fruit juice by volume. How many mL of real fruit juice is in 155 mL of
a drink?
i) plan:
ii) conversion factors:
iii) solving problem:
__________ mL real fruit juice
10
CHM130/Practice/Factor-label Method
1.
2.
Name:___________________________
A solution of ethanol was prepared by mixing 34.5 g of ethanol with 295 g of water.
a)
What is the percent of ethanol by mass in this solution?
b)
Write the conversion factors you can obtain from a).
c)
How many grams of ethanol are there if you take 35.0 g of this solution? Solve this by factor
label method.
A solid bar that measures 10.0 cm x 12.5 cm x 12.5 cm weighs 3250 g.
a)
Calculate the density of the solid.
b)
Write the density obtained for a) as two conversion factor forms.
c)
What volume in cc will 25.5 g of the solid occupy? Solve this by factor label method.
11
CHM130/Practice/Conversion Factors/Factor-label method
1.
2.
Name:__________________________
Write two conversion factors for each of the following statements.
a)
A car travels 55 miles per hour.
b)
Twenty five candies are in a bag.
c)
A medication is given at 3.50 mg/kg body weight.
Solve the following problems using conversion factors.
a)
A water bottle has a volume of 500. mL. What is the capacity of the water bottle in liters?
b)
The length of a pencil is 20.5 cm. How long is the pencil in meters?
c)
Convert 0.240 g to mg.
12
CHM130/Practice/Matter
Name:_____________________________
1.
Define ‘Matter’. ____________________________________________________________
2.
Identify three states of matter.
i)____________
3.
ii)____________
Identify which of the following represents a compound. ____
i)
4.
iii)____________
ii)
Which of the following indicates chemical change? _______
i)
ii)
+
+
Explain why.
5.
Name each of the following changes of states.
a)
c)
e)
solid to liquid_____________
liquid to gas_______________
solid to gas________________
b)
d)
f)
liquid to solid________________
gas to liquid__________________
gas to solid___________________
13
7.
The following represents the liquid state of water (H2O).
a)
Which of the following diagrams best represents water (H2O) molecules after liquid
water was heated to vaporize? _______
i)
ii)
iii)
Is vaporization physical or chemical change?_________
Explain your reasoning.
__________________________________________________________________
b)
Water (H2O) can be decomposed into hydrogen gas (H2) and oxygen gas (O2) by the
process called electrolysis.
Draw the diagram ii) of hydrogen gas and oxygen gas.
i)
ii)
Electrolysis
Is an electrolysis physical or chemical change? ___________
Explain your reasoning.
____________________________________________________________
14
CHM130/Practice/Physical and Chemical Changes
1.
2.
Name:___________________________
Classify each of the following as physical or chemical change.
a)
breaking glassware
__________
b)
drying clothes
__________
c)
burning wood
__________
d)
digesting a cookie
__________
e)
chopping an onion
__________
f)
inflating a balloon
__________
g)
dissolving an antacid tablet in water
__________
h)
rusting iron metal
__________
Classify each of the following as an element, compound, or mixture.
a)
air
__________
b)
table salt (NaCl)
__________
c)
copper
__________
d)
bronze alloy
__________
e)
ore
__________
15
CHM130/Practice/Element/Atom
Name:______________________
Write the symbols of the following elements.
Name of Element
symbol
Name of Element
Hydrogen
Helium
Lithium
Sodium
Potassium
Beryllium
Magnesium
Calcium
Strontium
Barium
Radium
Manganese
Cobalt
Palladium
Chromium
Iron
Nickel
Platinum
Copper
Silver
Gold
Zinc
Cadmium
Mercury
Boron
Aluminum
Carbon
Silicon
Tin
Lead
Nitrogen
Phosphorus
Arsenic
Antimony
Bismuth
Oxygen
Sulfur
Selenium
Fluorine
Chlorine
Bromine
Iodine
Neon
Argon
Krypton
Titanium
Xenon
Germanium
Cesium
Radium
16
symbol
CHM130/Practice/Element/Atom
Name:_______________________
Write the names of the following elements.
symbol
Name of Element
Name of Element
symbol
Cu
O
Li
I
Pt
Al
Mg
Mn
Sr
Ba
Kr
Xe
Ca
Fe
Co
Ni
Pd
K
H
Au
Si
Zn
C
Hg
B
Be
Cd
Ag
Sn
Pb
Ti
P
Ge
Sb
Bi
He
S
Se
F
Cl
Br
Na
Ne
Ar
Ra
N
Cr
As
17
CHM130
Practice (Atomic Structure)
Name:
1.
Complete the table by providing the missing information.
Name of element
Atomic
notation
Atomic
number
Sodium
Mass
number
Number of
protons
Number
of
neutrons
Number
of
electrons
23
27
13 Al
12
12
20
Potassium
56
14
8
26
16
16
Lithium
4
58
28 Ni
2.
Describe an atom according to (a) the Dalton model, (b) the Thomson model, and (c) the Rutherford
model.
(a)
The Dalton model
(b)
The Thomson model
(c)
The Rutherford model
18
CHM130
Extra (Electron Configuration)
Name:
1.
Write the electron configuration for each of the following and identify the valence shell and number of
valence electrons.
Element
Electron configuration
Valence shell
# of valence
electrons
sodium
neon
phosphorus
potassium
aluminum
bromine
2.
3.
Classify each of the following element as metal, nonmetal, or metalloid.
a)
silicon
____________
b)
silver
c)
e)
_____________
aluminum
___________
d)
chlorine
___________
cesium
___________
f)
copper
___________
Write the names of seven elements that exist as diatomic molecules.
______________________________________________________________
______________________________________________________________
19
CHM130
practice
Name:____________________
Complete the table by writing formulas and names of the compounds.
Cl-
+
O2-
N3-
S2-
Na2O
Na
Sodium oxide
Cu+
Ca2+
Ni2+
Fe2S3
3+
Fe
Iron(III) sulfide
Al3+
20
CHM130
Practice (Nomenclature)
Name:
1.
2.
Write the names of the following compounds.
a)
Ni2S3 __________________________________
b)
HgO
c)
H3P(aq) __________________________________
d)
CsF
__________________________________
e)
OF2
__________________________________
f)
ZnBr2 __________________________________
g)
Ag2O __________________________________
h)
Cu3N __________________________________
i)
S2F10 __________________________________
j)
H2S(aq) __________________________________
k)
N2O4 __________________________________
__________________________________
Write the formulas of the following compounds.
a)
Diphosphorus pentoxide ____________________
b)
Tin(II) fluoride
____________________
c)
Chromium(III) nitride
____________________
d)
Iodine trichloride
____________________
e)
Hydroselenic acid
____________________
f)
Calcium hydride
____________________
g)
Strontium sulfide
____________________
21
CHM130
Practice (Nomenclature)
Name:
1.
Name each of the following binary compounds.
MgS
______________________________________
K3 N
______________________________________
P4O10
______________________________________
H2S(aq)
______________________________________
NO
______________________________________
Fe2S3
______________________________________
H2Se(aq) ______________________________________
PbBr2
______________________________________
Hg2I2
______________________________________
OCl2
______________________________________
BeH2
______________________________________
Sr3P2
______________________________________
2. Write the formula for each compound.
Silver hydride
________________________
Cesium nitride
________________________
Phosphorus tribromide
________________________
Hydrobromic acid
________________________
Copper(II) sulfide
________________________
Barium fluoride
________________________
Tin(IV) carbide
________________________
22
CHM 130
Practice (Nomenclature)
Name:
1.
2.
Write correct formula for each of the following compounds.
a) sodium bromide
_____________________________
b) magnesium sulfide
_____________________________
c) potassium nitride
_____________________________
d) copper(I) oxide
_____________________________
e) calcium phosphide
_____________________________
f) dichlorine pentaoxide
_____________________________
g) iron(III) iodide
_____________________________
h) lithium hydride
_____________________________
Name the following compounds.
a) SO2
_________________________________________
b) NiCl2
_________________________________________
c) K2O
_________________________________________
d) CBr4
_________________________________________
e) AlN
_________________________________________
f) AgF
_________________________________________
g) Br3O8
_________________________________________
23
CHM130
Nomenclature (Binary Acids)
Name:_________________________
Write the names of the following acids.
1. HI(aq)
_______________________________
2. HCl(aq)
_______________________________
3. H3N(aq)
_______________________________
4. H2S(aq)
_______________________________
5. HF(aq)
_______________________________
6. H2Se(aq)
_______________________________
7. H3P(aq)
_______________________________
Write the formulas of the following acids.
1. hydrobromic acid
___________________________
2. hydrofluoric acid
___________________________
3. hydrocarbonic acid
___________________________
4. hydrosulfuric acid
___________________________
5. hydronitric acid
___________________________
6. hydrophosphoric acid
___________________________
7. hydroarsenic acid
___________________________
24
CHM130
Practice (Nomenclature/Acids)
Write formulas for the following acids.
1.
hydrochloric acid
____________________________
2.
perchloric acid
____________________________
3.
chloric acid
____________________________
4.
chlorous acid
____________________________
5.
hypochlorous acid
____________________________
6.
nitric acid
____________________________
7.
sulfuric acid
____________________________
8.
hydrosulfuric acid
____________________________
9.
nitrous acid
____________________________
10.
phosphoric acid
____________________________
11.
acetic acid
____________________________
12.
hydronitric acid
____________________________
13.
hydrofluoric acid
____________________________
14.
phosphorous acid
____________________________
15.
iodic acid
____________________________
Write names of the following acids.
16.
HBr(aq)
____________________________
17.
HBrO(aq)
____________________________
18.
HBrO2(aq)
____________________________
19.
HBrO3(aq)
____________________________
20.
HBrO4(aq)
____________________________
21.
H3P(aq)
____________________________
22.
H2SO3(aq)
____________________________
23.
H2CrO4(aq)
____________________________
24.
H2CO3(aq)
____________________________
25.
HI(aq)
____________________________
26.
H2Se(aq)
____________________________
27.
H3PO3(aq)
____________________________
25
CHM130
Practice (Nomenclature/Acids)
Write the names of the following acids.
1.
HCl(aq)
___________________________________
2.
HClO4(aq)
___________________________________
3.
HClO3(aq)
___________________________________
4.
HClO2(aq)
___________________________________
5.
HClO(aq)
___________________________________
6.
HNO3(aq)
___________________________________
7.
H2SO4(aq)
___________________________________
8.
H2S(aq)
___________________________________
9.
HNO2(aq)
___________________________________
10.
H3PO4(aq)
___________________________________
11.
HC2H3O2(aq)
___________________________________
12.
H3N(aq)
___________________________________
13.
HF(aq)
___________________________________
14.
H3PO3(aq)
___________________________________
15.
HIO3(aq)
___________________________________
Write the formulas of the following acids.
16.
hydrobromic acid
___________________________________
17.
hypobromous acid
___________________________________
18.
bromous acid
___________________________________
19.
bromic acid
___________________________________
20.
perbromic acid
___________________________________
21.
hydrophosphoric acid
___________________________________
22.
sulfurous acid
___________________________________
23.
chromic acid
___________________________________
24.
carbonic acid
___________________________________
25.
hydroiodic acid
___________________________________
26.
hydroselenic acid
___________________________________
27.
phosphorous acid
___________________________________
26
CHM130
Practice (Nomenclature)
Name:
1.
Complete the table by writing formulas and names of the compounds.
Cl-
SO4-2
OH-
PO4-3
Na+
Ca+2
Fe+3
NH4+
2.
Write the formula for each of the following compounds.
a)
Barium hydroxide
__________________________________________
b)
Sulfuric acid
__________________________________________
c)
Copper(I) phosphate
__________________________________________
d)
Magnesium hydroxide
__________________________________________
e)
Acetic acid
__________________________________________
27
CHM130
Practice (Nomenclature)
Name:
Write the formulas for the following compounds.
1.
lead (II) hydroxide
____________________________
2.
aluminum perchlorate
____________________________
3.
magnesium cyanide
____________________________
4.
lithium iodate
____________________________
5.
cobalt (III) nitrate
____________________________
6.
ammonium phosphate
____________________________
7.
dinitrogen pentoxide
____________________________
8.
sulfur hexabromide
____________________________
9.
barium sulfate
____________________________
10.
nickel (II) acetate
____________________________
11.
mercury (I) carbonate
____________________________
12.
antimony (III) chloride
____________________________
13.
cadmium phosphite
____________________________
14.
manganese (II) bicarbonate
____________________________
15.
nickel (II) fluoride
____________________________
16.
potassium dichromate
____________________________
17.
phosphorus pentabromide
____________________________
18.
copper (II) sulfite
____________________________
19.
calcium carbonate
____________________________
20.
copper(I) oxide
____________________________
21.
tin (IV) nitrate
____________________________
22.
iron (III) hydrogen sulfate
____________________________
23.
bismuth (III) nitrite
____________________________
24.
sulfur dioxide
____________________________
25.
dinitrogen trisulfide
____________________________
28
26.
tetraphosphorus decoxide
____________________________
27.
iodine monochloride
____________________________
28.
zinc acetate
____________________________
29.
iron (II) hydrogen sulfite
____________________________
30.
mercury (II) bromide
____________________________
31.
nickel (II) permanganate
____________________________
32.
barium oxide
____________________________
33.
tin (IV) cyanide
____________________________
34.
cobalt (II) chlorite
____________________________
35.
copper (I) sulfate
____________________________
36.
chromium (III) chloride
____________________________
37.
dichlorine heptoxide
____________________________
38.
silver dichromate
____________________________
39.
tin (II) chromate
____________________________
40.
strontium sulfite
____________________________
41.
potassium permanganate
____________________________
42.
iron (III) sulfate
____________________________
43.
mercury (I) sulfide
____________________________
44.
nickel (II) cyanide
____________________________
45.
dibromine momoxide
____________________________
46.
nitrogen trichloride
____________________________
47.
lithium phosphide
____________________________
48.
iodine monofluoride
____________________________
49.
carbon tetrabromide
____________________________
50.
iron (III) sulfite
____________________________
29
CHM130
Practice (Nomenclature)
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
lead (II) hydroxide
aluminum perchlorate
magnesium cyanide
lithium iodate
cobalt (III) nitrate
ammonium phosphate
dinitrogen pentoxide
sulfur hexabromide
barium sulfate
nickel (II) acetate
mercury (I) carbonate
antimony (III) chloride
cadmium phosphite
manganese (II) bicarbonate
nickel (II) fluoride
potassium dichromate
phosphorus pentabromide
copper (II) sulfite
calcium carbonate
copper(I) oxide
tin (IV) nitrate
iron (III) hydrogen sulfate
bismuth (III) nitrite
sulfur dioxide
dinitrogen trisulfide
tetraphosphorus decoxide
iodine monochloride
zinc acetate
iron (II) hydrogen sulfite
mercury (II) bromide
nickel (II) permanganate
barium oxide
tin (IV) cyanide
cobalt (II) chlorite
copper (I) sulfate
chromium (III) chloride
dichlorine heptoxide
silver dichromate
tin (II) chromate
strontium sulfite
potassium permanganate
iron (III) sulfate
mercury (I) sulfide
nickel (II) cyanide
dibromine monoxide
nitrogen trichloride
lithium phosphide
iodine monofluoride
carbon tetrabromide
iron (III) sulfite
Pb(OH)2
Al(ClO4)3
Mg(CN)2
LiIO3
Co(NO3)3
(NH4) 3PO4
N 2O 5
SBr6
BaSO4
Ni(C2H3O2) 2
Hg2CO3
SbCl3
Cd3 (PO3) 2
Mn(HCO3) 2
NiF2
K2Cr2O7
PBr5
CuSO3
CaCO3
Cu2O
Sn(NO3) 4
Fe(HSO4) 3
Bi(NO2) 3
SO2
N2S3
P4O10
ICl
Zn(C2H3O2) 2
Fe(HSO3)2
HgBr2
Ni(MnO4) 2
BaO
Sn(CN) 4
Co(ClO2) 2
Cu2SO4
CrCl3
Cl2O7
Ag2Cr2O7
SnCrO4
SrSO3
KMnO4
Fe2(SO4) 3
Hg2S
Ni(CN) 2
Br2O
NCl3
Li3P
IF
CBr4
Fe2(SO3) 3
30
CHM130
Practice (Nomenclature II)
Name:
Write the names of the following compounds.
1.
PbI2
____________________________
2.
Na2CO3
____________________________
3.
Zn(HCO3) 2
____________________________
4.
SnF2
____________________________
5.
Al(ClO3) 3
____________________________
6.
CF4
____________________________
7.
PI5
____________________________
8.
Al2O3
____________________________
9.
Ag2CrO4
____________________________
10.
Pb(SO3) 2
____________________________
11.
(NH4)2CO3
____________________________
12.
Fe(C2H3O2) 3
____________________________
13.
H2SO4(aq)
____________________________
14.
Mg(MnO4) 2
____________________________
15.
Sr(ClO4) 2
____________________________
16.
Cl2S7
____________________________
17.
OF2
____________________________
18.
Cu(OH) 2
____________________________
19.
Al(CN) 3
____________________________
20.
CS2
____________________________
21.
HgS
____________________________
22.
P4S5
____________________________
23.
Ca(ClO3) 2
____________________________
24.
Cd(CN) 2
____________________________
25.
KBrO2
____________________________
26.
Cr(HSO4) 3
____________________________
27.
Li3PO4
____________________________
28.
SnBr4
____________________________
29.
Hg2 (NO2) 2
____________________________
30.
Ni3 (PO4) 2
____________________________
31
31.
K 2O
____________________________
32.
Fe(ClO2) 2
____________________________
33.
Ca(HCO3)2
____________________________
34.
CI4
____________________________
35.
PF5
____________________________
36.
Mn(ClO) 2
____________________________
37.
BrCl3
____________________________
38.
Cr(NO3) 3
____________________________
39.
CoCO3
____________________________
40.
NCl3
____________________________
41.
BaSO3
____________________________
42.
CuClO
____________________________
43.
P4O10
____________________________
44.
Ni(C2H3O2) 2
____________________________
32
CHM130
Practice (Nomenclature II)
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
PbI2
Na2CO3
Zn(HCO3) 2
SnF2
Al(ClO3) 3
CF4
PI5
Al2O3
Ag2CrO4
Pb(SO3) 2
(NH4)2CO3
Fe(C2H3O2) 3
H2SO4(aq)
Mg(MnO4) 2
Sr(ClO4) 2
Cl2S7
OF2
Cu(OH) 2
Al(CN) 3
CS2
HgS
P4S5
Ca(ClO3) 2
Cd(CN) 2
KBrO2
Cr(HSO4) 3
Li3PO4
SnBr4
Hg2 (NO2) 2
Ni3 (PO4) 2
K 2O
Fe(ClO2) 2
Ca(HCO3)2
CI4
PF5
Mn(ClO) 2
BrCl3
Cr(NO3) 3
CoCO3
NCl3
BaSO3
CuClO
P4O10
Ni(C2H3O2) 2
lead (II) iodide
sodium carbonate
zinc bicarbonate
tin (II) fluoride
aluminum chlorate
carbon tetrafluoride
phosphorus pentaiodide
aluminum oxide
silver chromate
lead (IV) sulfite
ammonium carbonate
iron (III) acetate
sulfuric acid
magnesium permanganate
strontium perchlorate
dichlorine heptasulfide
oxygen difluoride
copper (II) hydroxide
aluminum cyanide
carbon disulfide
mercury (II) sulfide
tetraphosphorus pentasulfide
calcium chlorate
cadmium cyanide
potassium bromite
chromium (III) bisulfate
lithium phosphate
tin (IV) bromide
mercury (I) nitrite
nickel (II) phosphate
potassium oxide
iron (II) chlorite
calcium bicarbonate (or calcium hydrogen carbonate)
carbon tetraiodide
phosphorus pentafluoride
manganese (II) hypochlorite
bromine trichloride
chromium (III) nitrate
cobalt (II) carbonate
nitrogen trichloride
barium sulfite
copper (I) hypochlorite
tetraphosphorus decoxide
nickel (II) acetate
33
CHM130
Practice (Single Replacement Reaction)
Name:
1.
i)
ii)
iii)
Write balanced formula equation for each of the following reactions.
Explain why this reaction occurs.
Write word equation.
i)
Al
+ HCl →
ii)
iii)
2.
i)
AgNO3
+
Mg
→
ii)
iii)
3.
i)
H3PO4 +
Li →
ii)
iii)
4.
i)
Mn
+ PbBr2
→
ii)
iii)
5.
i)
Fe2(CO3)3 + Ca
→
ii)
iii)
34
CHM130
Practice (Single Replacement reaction)
Name:
Write balanced formula equations for the following single replacement reactions. If no reaction occurs,
write NR.
i)
Na + AgNO3 →
ii)
H2SO4 + Mg →
iii)
Fe + NiCl2 →
iv)
K2CO3 + Ba →
v)
K + H2 O →
vi)
Al + Fe(NO3)2 →
vii) NaCl + Br2 →
viii) LiBr + Cl2 →
CHM130
35
Practice (Double Replacement Reaction)
Name:
Write balanced formula equations for the following double replacement reactions. If no reaction occurs,
write NR.
a)
NaOH + H2SO4 →
b)
AgNO3 + HCl →
c)
K2CO3 + ZnBr2 →
d)
NH4I + LiOH →
e)
HC2H3O2 + Na2SO3 →
f)
KCl + Mg(NO3)2 →
36
CHM130
Practice (Reactions)
Name:
Write balanced formula equations for the following and classify each of these reactions as combination,
decomposition, single replacement, or double replacement reaction. If no reaction occurs, write NR.
a)
sodium + iron(II) nitrate →
b)
copper(II) chloride + potassium hydroxide →
c)
ammonium chloride + sodium iodide →
d)
Mg(C2H3O2)2 + H2CO3 →
e)
K + HgCl2 →
f)
H2 + O2 → H2 O
g)
H2SO4 + Na2CO3 →
h)
KClO3 → KCl + O2
i)
MgO + H2O → Mg(OH)2
j)
silver nitrate + sodium chloride →
k)
iron(II) bromide + sodium →
CHM130
37
Practice (Reactions)
Name:
Complete the following i)word equations and write ii)balanced formula equations. iii)Classify each of these
reactions as combination, decomposition, single replacement, or double replacement reaction. If no
reaction occurs, write NR.
a)
i) lead(II) nitrate + potassium chloride →
ii)
iii)
b)
i) silver hydroxide → silver oxide + water
ii)
iii)
c)
i) barium + chromium(III) chloride →
ii)
iii)
d)
i) iron(III) nitrate + potassium hydroxide →
ii)
iii)
e)
i) sodium carbonate + sulfuric acid →
ii)
iii)
f)
i) sodium sulfite + sulfuric acid →
i)
ii)
iii)
38
h)
i) phosphoric acid + potassium hydroxide →
ii)
iii)
i)
i) hydrochloric acid + potassium hydroxide →
ii)
iii)
j)
i) copper + silver nitrate →
ii)
iii)
k)
i) ammonium acetate + sodium hydroxide →
ii)
iii)
l)
i) hydrosulfuric acid + aluminum →
ii)
iii)
m)
i) iron(III) bromide + phosphoric acid →
ii)
iii)
n)
i) cadmium(II) acetate + barium bromide →
ii)
iii)
39
CHM130
Practice (Chemical quantities)
Name:____________________
1.
Find the mass (in grams) of 2.45 moles of gold atoms.
2.
How many copper atoms are in 2.35 x 104 grams of copper metal?
3.
What is the mass (in grams) of 6.44 x 1021 molecules of P4O10?
4.
a)
Give the mass of each of the following. Make sure to include unit.
1 mole of N atoms __________
1 mole of S atoms __________
b)
1 mole of H atoms ___________
1 mole of O atoms ___________
Determine the molar mass of ammonium sulfate.
__________________g/mol
c)
Calculate the mass percent composition of ammonium sulfate.
% N:
% H:
% S:
% O:
40
5.
Calculate moles of hydrogen atoms that are contained in 34.5 g of ammonia (NH3).
________________moles of H atoms
8.
How many CO2 molecules are contained in 1.25 x 103 g of CO2?
________________ CO2 molecules
9.
Calculate the mass (in grams) of nitrogen atoms in 4.50 moles of Mg(NO3)2.
________________g of N atoms
10.
Calculate the mass (in grams) of nitrogen atoms in 45.8 grams of dinitrogen monoxide (N2O).
_________________g N
41
CHM130
Practice (Determination of chemical formulas)
Name:__________________
1.
Acetylene used in gas welding contains 92.25 g C and 7.75 g H and has a molar mass of 26.02 g/mole.
a)
Obtain the Empirical formula for acetylene.
Empirical formula________
b)
Find the molecular formula for acetylene.
Molecular formula________
2.
Percent composition of a compound containing carbon, hydrogen, and oxygen is available as follows.
54.53% C, 9.15% H
The molar mass of the compound is 88.106 g/mole. What are the empirical and molecular formulas
for this compound?
Empirical formula________
Molecular formula________
42
3.
Th elemental mass percents of a compound are 40.00% carbon, 6.72% hydrogen, and 53.28% oxygen.
The molar mass of the compound is 180.16 g. What are the empirical and molecular formulas for this
compound?
Empirical formula_________
Molecular formula________
4.
Percent composition of a compound by mass is 24.27 % carbon, 4.07 % hydrogen, 71.65% chlorine.
i)
Determine the empirical formula.
Empirical formula_________
ii)
Molar mass of the compound is 98.96 g/mole. What is the molecular formula of this compound?
Molecular formula________
43
CHM130
Practice (Stoichiometry)
1.
Aluminum oxide was prepared by reacting 2.50 g of aluminum and 2.50 g of oxygen.
4Al + 3O2 2Al2O3
a) Calculate the theoretical yield of aluminum oxide in this reaction and
identify the limiting reactant.
b) Determine the percent yield if 4.25 g of aluminum oxide was obtained.
2.
20.0 grams of NaCl and 41.0 grams of AgNO3 were allowed to react according to the following
equation:
NaCl + AgNO3 AgCl + NaNO3
a)
What is the theoretical yield of NaNO3?
b)
Identify the limiting reactant.
44
3.
For the following reaction;
NH3 + F2 → N2F4 + HF
4.
i)
Balance the equation:
ii)
How many moles of NH3 are needed to produce 20.0 g of N2F4?
iii)
How many grams of F2 are required to react with 12.0 g of N2?
For the combustion of octane;
C8H18 + O2
5.
6.
→
i)
Write a balanced formula equation.
ii)
Suppose 105.0 g of octane is combined with 60.0 g of oxygen. What is the theoretical yield of
H2O?
iii)
Which one is a limiting reactant?
For the following reaction,
CH4 (methane) + 2O2 → 2H2O + CO2
i)
How many grams of oxygen will be required to react with 4.55 moles of methane?
ii)
How many grams of H2O will be produced if 33.2 grams of methane is reacted?
A reaction mixture contains 10.0 grams of Na and 2.35 grams of hydrogen for the following reaction:
2Na + H2 → 2NaH
45
i)
What is the theoretical yield of sodium hydride for the reaction?
ii)
Which one is the limiting reactant? ___
iii)
When the reaction was performed, 8.50 grams of NaH was recovered. What is the percent yield
of the reaction?
46
CHM130
Practice (Solution)
Name:
1.
Identify each of the following as an electrolyte or a nonelectrolyte.
a) solid KBr
b) sugar(C12H22O11) solution
c) NaNO3 (aq)
d) KOH (aq)
2.
A solution has a pH of 8.0.
a) Is this solution an acidic solution or a basic solution?
b) Which ion does this solution have more, H+ or OH-?
c) If this is not a buffer solution, what happens in pH of this solution when
small amount of base is added to the solution?
3.
Draw Lewis structures of the following molecules.
a)
NCl3
b)
H2 S
c)
OF2
d)
CHCl3
47