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AP Chem 2013-2014 Summer Assignment (2549892)
Question
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Description
Problems from Chapters 1-3 of Zumdahl
Instructions
The following questions represent the baseline knowledge you will need to succeed in
AP Chemistry. The goal of this assignment is twofold. First, it will tell you what you are
up against in the upcoming school year. Second, this assignment covers curriculum
that is basic and will allow us the time to cover more critical material in class during the
school year. We will review this material during the first week of school and you will be
tested on it at the end of the second week of school. Answer the following questions
before the beginning of the 2013-2014 school year. If you have questions, please feel
free to email me at [email protected]. If you would like to pick up a textbook from
school to help you with this, send me an email but you have access to the digital text. I
give you the answers for all questions so you know when you get it correct. You don't
have to show work for the naming questions....just know the answers BUT you do have
to hand in work for the math-based questions.
1.
Question Details
ZumChem8 1.E.097. [1070250]
A column of liquid is found to expand linearly on heating 5.40 cm for a 12.7°F rise in temperature. If the initial temperature
of the liquid is 95.3°F, what will the final temperature be in °C if the liquid has expanded by 20.0 cm?
61.3 °C
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2.
Question Details
ZumChem8 1.E.099. [1068700]
For each of the following, decide which block is more dense: the orange block, the blue block, or it cannot be determined.
(a)
orange
blue
cannot be determined
Explain your answer.
Key: Volume
density = mass; the orange block is more dense. Since mass (orange) > mass (blue) and since
volume (orange) < volume (blue), the density of the orange block must be greater to account for the large
mass of the orange block.
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(b)
orange
blue
cannot be determined
Explain your answer.
Key: Which block is more dense cannot be determined. Since mass (orange) > mass (blue) and since volume
(orange) > volume (blue), the density of the orange block may or may not be greater than the blue block. If the
blue block is more dense, it's density cannot be so large that it's mass is larger than the orange block's mass.
(c)
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orange
blue
cannot be determined
Explain your answer.
Key: Since mass (blue) = mass (orange) and since volume (blue) < volume (orange), the density of the blue
block must be larger in order to equate the masses.
(d)
orange
blue
cannot be determined
Explain your answer.
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Key: Since mass (blue) > mass (orange) and since the volumes are equal, the density of the blue block must be
larger in order to give the blue block the larger mass.
3.
Question Details
ZumChem8 1.E.105. [1864423]
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Many times errors are expressed in terms of percentage. The percentage error is the absolute value of the difference of the
true value and the experimental value, divided by the true value, and multiplied by 100.
Calculate the percent error for the following measurements.
(a) The density of an aluminum block determined in an experiment was 2.61 g/cm3. (True value 2.70 g/cm3.)
3 %
(b) The experimental determination of iron in iron ore was 16.60%. (True value 16.12%.)
3.0 %
(c) A balance measured the mass of a 1.000 g standard as 0.9911 g.
0.9 %
4.
Question Details
ZumChem8 1.E.112. [1070254]
An experiment was performed in which an empty 100 mL graduated cylinder was weighed. It was weighed once again after
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it had been filled to the 10.0 mL mark with dry sand. A 10 mL pipet was used to transfer 10.00 mL of methanol to the
cylinder. The sand-methanol mixture was stirred until bubbles no longer emerged from the mixture and the sand looked
uniformly wet. The cylinder was then weighed again. Use the data obtained from this experiment (and displayed at the end
of this problem) to find the density of each of the following.
Mass of cylinder plus wet sand
45.2613 g
Mass of cylinder plus dry sand
37.3488 g
Mass of empty cylinder
22.8317 g
Volume of dry sand
10.0 mL
Volume of sand + methanol
17.6 mL
Volume of methanol
10.00 mL
dry sand
1.45 g/mL
methanol
0.7913 g/mL
sand particles
1.9 g/mL
Does the bubbling that occurs when the methanol is added to the dry sand indicate that the sand and methanol are
reacting?
Yes
No
5.
Question Details
ZumChem8 1.E.072. [1070253]
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A copper wire (density = 8.96 g/cm3) has a diameter of 0.10 mm. If a sample of this copper wire has a mass of 25 g, how
long is the wire?
1200 ft
6.
Question Details
ZumChem8 1.E.069. [1068689]
In each of the following pairs, which has the greater volume?
(a) lead or feathers
1.0 kg of lead
1.0 kg of feathers
Both have same volume.
(b) gold or water
100 g of gold
100 g of water
Both have same volume.
(c) mercury or copper
1.0 L of mercury
1.0 L of copper
Both have same volume.
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7.
Question Details
ZumChem8 1.E.065. [1070257]
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A sample containing 33.49 g of metal pellets is poured into a graduated cylinder initially containing 11.8 mL of water,
causing the water level in the cylinder to rise to 19.1 mL. Calculate the density of the metal.
4.6 g/cm3
8.
Question Details
ZumChem8 1.E.056. [1092120]
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Convert the following Kelvin temperatures to Celsius and Fahrenheit degrees.
(a) the temperature that registers the same value on both the Fahrenheit and Celsius scales, 233 K
-40. °C
-40. °F
(b) the boiling point of helium, 4K
-269 °C
-452 °F
(c) the temperature at which many chemical quantities are determined, 298 K
25 °C
77 °F
(d) the melting point of tungsten, 3680 K
3410 °C
6160 °F
9.
Question Details
ZumChem8 1.E.044. [1070243]
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Although the preferred SI unit of area is the square meter, land is often measured in the metric system in hectares (ha).
One hectare is equal to 10,000 m2. In the English system, land is often measured in acres (1 acre = 160 rod2). Use the
exact conversions and those given below to calculate the following.
5 1/2 yards = 1 rod
40 rods = 1 furlong
8 furlongs = 1 mile
0.01 km2
(a) 1 ha =
(b) The area of a 4.5 acre plot of land in hectares, square meters, and square kilometers
1.8 ha
18000 m2
0.018 km2
(c) A lot with dimensions 120 ft by 75 ft is to be sold for $6500. What is the price per acre?
$
31000
What is the price per hectare?
$
10.
Question Details
78000
ZumChem8 2.CW.03. [1110960]
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.
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11.
Question Details
ZumChem8 2.E.061. [1212712]
Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in
each case?
(a) Na
(b) Te
gain
gain
lose
ion formed
lose
ion formed
Na+
Te2-
(c) Rb
(d) Br
gain
lose
ion formed
Rb+
gain
lose
ion formed
Br-
-
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(e) O
(f) Al
gain
gain
lose
lose
ion formed
ion formed
O2-
12.
Al3+
Question Details
ZumChem8 2.E.060. [1212698]
Complete the following table.
Symbol
238 U
Number of
protons in
nucleus
92
Number of
neutrons in
nucleus
146
Number of
electrons
92
Net
charge
0
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92
40
Ca2+
20
20
20
51 3+
V
23
23
28
89
39
Y
79
Br35
31 3P
15
39
18
20
50
35
44
15
16
2+
3+ -or- +3
39
36
0
1- -or- -1 -or- -
18
3-
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13.
Question Details
ZumChem8 2.E.064. [1212707]
Name the compounds in parts (a) through (d) and write the formulas for the compounds in parts (e) through (h). (Enter
your answer using the format copper(II) chloride for CuCl2.)
(a) TiCl4
titanium(IV) chloride
(b) FeBr3
iron(III) bromide
(c) CoS
cobalt(II) sulfide
(d) Hg2O
mercury(I) oxide
(e) tin(II) nitride
Sn3N2
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(f) mercury(II) oxide
HgO
(g) niobium(V) oxide
Nb2O5
(h) iron(III) oxide
Fe2O3
14.
Question Details
ZumChem8 2.E.067. [1068708]
Name each of the following compounds.
(a) K2Cr2O7
potassium dichromate
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(b) NaClO2
sodium chlorite
(c) Li3PO4
lithium phosphate
(d) BaSO3
barium sulfite
15.
Question Details
ZumChem8 2.E.066. [1214701]
Write the formula for each of the following compounds.
(a) aluminum sulfide
Al2S3
(b) beryllium oxide
BeO
(c) potassium bromide
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KBr
(d) tin(IV) fluoride
SnF4
(e) magnesium chloride
MgCl2
(f) silver iodide
AgI
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16.
Question Details
ZumChem8 2.E.069. [1068688]
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ZumChem8 2.E.072. [1068691]
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Name each of the following compounds.
(a) SO2
sulfur dioxide
(b) N2O4
dinitrogen tetroxide
(c)
dinitrogen tetroxide
(d)
iodine trichloride
17.
Question Details
Name each of the following compounds. Assume the acids are dissolved in water. (Enter your answer using the format
copper(II) chloride for CuCl2.)
(a) HC2H3O2
acetic acid
(b) NH4NO2
ammonium nitrite
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(c) Co2S3
cobalt(III) sulfide
(d) ICl
iodine monochloride
(e) Pb3(PO4)2
lead(II) phosphate
(f) KClO3
potassium chlorate
(g) H2SO4
sulfuric acid
(h) Sr3N2
strontium nitride
(i) Al2(SO3)3
aluminum sulfite
(j) SnO2
tin(IV) oxide -or- stannic oxide
(k) Na2CrO4
sodium chromate
(l) HClO
hypochlorous acid
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18.
Question Details
ZumChem8 2.E.075. [1212693]
Write the formula for each of the following compounds.
(a) sulfur difluoride
SF2
(c) sodium dihydrogen phosphate
NaH2PO4
(e) chromium(III) carbonate
Cr2(CO3)3
(b) sulfur hexafluoride
SF6
(d) lithium nitride
Li3N
(f) tin(II) fluoride
SnF2
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(g) ammonium acetate
NH4C2H3O2
(i) cobalt(III) nitrate
Co(NO3)3
(k) potassium chlorate
KClO3
19.
Question Details
(h) ammonium hydrogen sulfate
NH4HSO4
(j) mercury(I) chloride
Hg2Cl2
(l) sodium hydride
NaH
ZumChem8 2.E.105. [1068719]
Each of the following statements is true, but Dalton might have had trouble explaining some of them with his atomic
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theory. Give explanations for the following statements.
(a) The space-filling models for ethyl alcohol and dimethyl ether are shown below.
These two compounds have the same composition by mass (52% carbon, 13% hydrogen, and 35% oxygen), yet
the two have different melting points, boiling points, and solubilities in water.
Key: Both compounds have C2H6O as the formula. Because they have the same formula, their mass percent
composition will be identical. However, these are different compounds with different properties since the atoms
are bonded together differently. These compounds are called isomers of each other.
(b) Burning wood leaves an ash that is only a small fraction of the mass of the original wood.
Key: When wood burns, most of the solid material in wood is converted to gases, which escape. The gases
produced are most likely CO2 and H2O.
(c) Atoms can be broken down into smaller particles.
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Key: The atom is not an indivisible particle, but is instead composed of other smaller particles, e.g., electrons,
neutrons, and protons.
(d) One sample of lithium hydride is 87.4% lithium by mass, while another sample of lithium hydride is 74.9%
lithium by mass. However, the two samples have the same properties.
Key: The two hydride samples contain different isotopes of either hydrogen and/or lithium. Although the
compounds are composed of different isotopes, their properties are similar because different isotopes of the
same element have similar properties (except, of course, their mass).
20.
Question Details
ZumChem8 2.E.095. [1212690]
The designations 1A through 8A used for certain families of the periodic table are helpful for predicting the charges on ions
in binary ionic compounds. In these compounds, the metals generally take on a positive charge equal to the family
number, while the nonmetals take on a negative charge equal to the family number minus eight. Thus the compound
between sodium and chlorine contains Na+ ions and Cl- ions and has the formula NaCl. Predict the formula and the name of
the binary compound formed from the following pairs of elements.
elements
formula
name
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(a) Ca and N
Ca3N2
calcium nitride
(b) K and O
K2 O
potassium oxide
(c) Rb and F
RbF
rubidium fluoride
(d) Mg and S
MgS
magnesium sulfide
(e) Ba and I
BaI2
barium iodide
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21.
(f) Al and Se
Al2Se3
aluminum selenide
(g) Cs and P
Cs3P
cesium phosphide
(h) In and Br
InBr3
indium(III) bromide
Question Details
ZumChem8 2.E.090. [1212695]
For each of the following ions, indicate the total number of protons and electrons in the ion. For the positive ions in the list,
predict the formula of the simplest compound formed between each positive ion and the oxide ion. For the negative ions in
the list, predict the formula of the simplest compound formed between each negative ion and the aluminum ion.
(b) Se2-
(a) F ‾
protons
9
protons
34
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electrons
compound
10
AlF3
electrons
compound
36
Al2Se3
(d) Rb+
(c) Fe2+
protons
26
protons
37
electrons
24
electrons
36
compound
compound
FeO
(e) Mg2+
Rb2O
(f) Fe3+
protons
12
protons
26
electrons
10
electrons
23
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compound
compound
MgO
(g) Cr3+
(h) Br‾
protons
24
protons
35
electrons
21
electrons
36
compound
22.
Fe2O3
Cr2O3
compound
Question Details
AlBr3
ZumChem8 3.E.170. [1865488]
The compound As2I4 is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic (d =
5.72 g/cm3) that is 3.18 cm on edge is allowed to react with 1.01
1024 molecules of arsenic triiodide, how much As2I4
can be prepared?
827 g
If the percent yield of As2I4 was 73.7%, what mass of As2I4 was actually isolated?
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609 g
23.
Question Details
ZumChem8 3.E.151. [1214718]
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A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 g of the compound produced
0.213 g CO2 and 0.0310 g H2O. In another experiment, it is found that 0.103 g of the compound produces 0.0230 g NH3.
What is the empirical formula of the compound? Hint: Combustion involves reacting with excess O2. Assume that all the
carbon ends up in CO2 and all the hydrogen ends up in H2O. Also assume that all the nitrogen ends up in the NH3 in the
second experiment.
C 7H5N 3O 6
24.
Question Details
ZumChem8 3.E.152. [1053089]
-
Nitric acid is produced commercially by the Ostwald process, represented by the following equations.
4 NH3(g) + 5 O2(g)
2 NO(g) + O2(g)
3 NO2(g) + H2O(l)
4 NO(g) + 6 H2O(g)
2 NO2(g)
2 HNO3(aq) + NO(g)
What mass in kg of NH3 must be used to produce 4.5
106 kg HNO3 by the Ostwald process, assuming 100% yield in each
reaction?
1.8e+06 kg
25.
Question Details
ZumChem8 3.E.154. [1092133]
A 9.752-g gaseous mixture contains ethane (C2H6) and propane (C3H8). Complete combustion to form carbon dioxide and
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water requires 1.120 mol of oxygen. Calculate the mass percent of ethane in the original mixture. (Use 1.008, 12.01, and
16.00 amu as the atomic mass for hydrogen, carbon, and oxygen, respectively.)
48.3 %
26.
Question Details
ZumChem8 3.E.135. [1053046]
-
The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. What number of H atoms are present in
a 9.00 g sample of styrene?
4.16e+23 atoms
27.
Question Details
ZumChem8 3.E.136. [1214692]
-
Terephthalic acid is an important chemical used in the manufacture of polyesters and plasticizers. It contains only C, H, and
O. Combustion of 23.77 mg terephthalic acid produces 50.38 mg CO2 and 7.74 mg H2O. If 0.250 mol of terephthalic acid
has a mass of 41.5 g, determine the molecular formula of terephthalic acid.
C 8H6O 4
28.
Question Details
ZumChem8 3.E.138. [1053092]
A binary compound between an unknown element E and hydrogen contains 91.27% E and 8.73% H by mass. If the
formula of the compound is E3H8, calculate the atomic mass of E.
28.1 amu
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29.
Question Details
ZumChem8 3.E.140. [1053070]
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ABS plastic is a tough, hard plastic used in applications requiring shock resistance. The polymer consists of three monomer
units: acrylonitrile (C3H3N), butadiene (C4H6), and styrene (C8H8).
(a) A sample of ABS plastic contains 8.80% N by mass. It took 0.605 g of Br2 to react completely with a 1.20 g
sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene molecules in the polymer and nothing
else. What is the percent by mass of acrylonitrile and butadiene in this polymer?
C3H3N
33.3 %
C4H6
17.1 %
(b) What are the relative numbers of each of the monomer units in this polymer? (Give the ratio of
acrylonitrile:butadiene:styrene. Use the lowest possible coefficients.)
4 (C3H3N) :
30.
2 (C4H6) :
3 (C8H8)
Question Details
ZumChem8 3.E.142. [1216940]
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide
and hydrogen sulfide as the only products.
(a) Write the balanced chemical equation for the reaction of methane and sulfur. (Use the lowest possible
coefficients. Include states of matter under SATP conditions in your answer.)
CH4(g) + 4 S(s) → CS2(l) + 2 H2S(g) -or- 2 CH4(g) + S8(s) → 2 CS2(l) + 4 H2S(g)
(b) Calculate the theoretical yield of carbon disulfide when 160. g of methane is reacted with an equal mass of
-
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sulfur.
95.0 g
31.
Question Details
ZumChem8 3.E.146. [1053064]
-
Commercial brass, an alloy of Zn and Cu, reacts with hydrochloric acid as follows.
Zn(s) + 2 HCl(aq)
ZnCl2(aq) + H2(g)
(Cu does not react with HCl.) When 0.5133 g of a certain brass alloy is reacted with excess HCl, 0.0985 g ZnCl2 is
eventually isolated.
(a) What is the composition of the brass by mass?
Zn
9.21 %
Cu
90.79 %
(b) How could this result be checked without changing the above procedure?
Key: The Cu remains unreacted. After filtering, washing, and drying, the mass of the unreacted copper could be
measured.
32.
Question Details
ZumChem8 3.E.116. [1053063]
Consider the following unbalanced reaction.
P4(s) + F2(g)
PF3(g)
What mass of F2 is needed to produce 220. g of PF3 if the reaction has a 74.2% yield?
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192 g
33.
Question Details
ZumChem8 3.E.115. [1053080]
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Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following reaction occurs.
2 Cu3FeS3(s) + 7 O2(g)
6 Cu(s) + 2 FeO(s) + 6 SO2(g)
If 3.48 metric tons of bornite is reacted with excess O2 and the process has an 78.0% yield of copper, what mass of copper
is produced?
1.51 metric tons
34.
Question Details
ZumChem8 3.E.104. [1053067]
-
Phosphorus can be prepared from calcium phosphate by the following reaction.
2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s)
→ 6 CaSiO3(s) + P4(s) + 10 CO(g)
Phosphorite is a mineral that contains Ca3(PO4)2 plus other non-phosphorus-containing compounds. What is the maximum
amount of P4 that can be produced from 2.1 kg of phosphorite if the phosphorite sample is 99% Ca3(PO4)2 by mass?
Assume an excess of the other reactants.
420 g
35.
Question Details
ZumChem8 3.E.102. [1216955]
One of relatively few reactions that takes place directly between two solids at room temperature is given in the equation
below. In this equation, the · 8 H2O in Ba(OH)2 · 8 H2O indicates the presence of eight water molecules. This compound is
called barium hydroxide octahydrate.
(a) Balance the equation. (Use the lowest possible coefficients. Include states-of-matter under the given conditions
in your answer.)
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Ba(OH)2 · 8 H2O(s) + NH4SCN(s)
→ Ba(SCN)2(s) + H2O(l) + NH3(g)
Ba(OH)2 . 8 H2O(s) + 2 NH4SCN(s) → Ba(SCN)2(s) + 10 H2O(l) + 2 NH3(g)
(b) What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 4.8 g barium
hydroxide octahydrate?
2.3 g
36.
Question Details
ZumChem8 3.E.089. [1214726]
Give the balanced equation for each of the following chemical reactions. (Use the lowest possible coefficients. Include
states-of-matter under the given conditions in your answer.)
(a) Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor.
C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(g)
(b) Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen
sulfide gas.
Fe2S3(s) + 6 HCl(g) → 2 FeCl3(s) + 3 H2S(g)
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(c) Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium
thiocyanate (NH4SCN).
CS2(l) + 2 NH3(g) → H2S(g) + NH4SCN(s)
37.
Question Details
ZumChem8 3.E.095. [1216947]
Balance the following equations representing combustion reactions. (Use the lowest possible coefficients. Include statesof-matter under the given conditions in your answer where appropriate.)
(a)
2
(b)
2
(c) C12H22O11(s) + O2(g)
+
15
+
→
13
→ CO2(g) + H2O(g)
C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(g)
12
→
+
8
6
+
10
-
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(d) Fe(s) + O2(g)
→ Fe2O3(s)
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
(e) FeO(s) + O2(g)
→ Fe2O3(s)
4 FeO(s) + O2(g) → 2 Fe2O3(s)
38.
Question Details
ZumChem8 3.E.088. [1214710]
A compound contains only carbon, hydrogen, and oxygen. Combustion of 9.612 mg of the compound yields 14.41 mg CO2
and 3.93 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the
compound?
empirical formula
molecular formula
C 3H4O 3
C 6H8O 6
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39.
Question Details
ZumChem8 3.E.069. [1053082]
-
There are several important compounds that contain only nitrogen and oxygen. Calculate the mass percent of nitrogen in
each of the following.
(a) NO, a gas formed by the reaction of N2 with O2 in internal combustion engines.
46.7 %
(b) NO2, a brown gas mainly responsible for the brownish color of photochemical smog.
30.4 %
(c) N2O4, a colorless liquid used as a fuel in space shuttles.
30.4 %
(d) N2O, a colorless gas sometimes used as an anesthetic by dentists (known as laughing gas).
63.7 %
40.
Question Details
ZumChem8 3.E.070. [1053090]
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Arrange the following substances in order of increasing mass percent of carbon.
caffeine, C8H10N4O2
sucrose, C12H22O11
ethanol, C2H5OH
---Select---
41.
sucrose <
---Select---
caffeine <
---Select---
Question Details
ethanol
ZumChem8 3.E.071. [1061771]
-
Fungal laccase, a blue protein found in wood-rotting fungi, is 0.390% Cu by mass. If a fungal laccase molecule contains 4
copper atoms, what is the molar mass of fungal laccase?
65200 g/mol
42.
Question Details
ZumChem8 3.E.065. [1053083]
Chloral hydrate (C2H3Cl3O2) is a drug formerly used as a sedative and hypnotic. It is the compound used to make "Mickey
Finns" in detective stories.
(a) Calculate the molar mass of chloral hydrate.
165 g/mol
(b) What amount (moles) of C2H3Cl3O2 molecules are in 501.0 g chloral hydrate?
3.029 mol
(c) What is the mass in grams of 2.0
10-2 mol chloral hydrate?
3.3 g
(d) What number of chlorine atoms are in 4.4 g chloral hydrate?
4.8e+22
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(e) What mass of chloral hydrate would contain 2.4 g Cl?
3.7 g
(f) What is the mass of exactly 483 molecules of chloral hydrate?
1.33e-19 g
43.
Question Details
ZumChem8 3.E.064. [1053088]
-
Complete the following table.
Sample
Mass of sample (g)
C6H6
4.28
H2O
CO2
CH3OH
44.
4.32
1.85
0.297
Moles of sample (mol)
Molecules in sample
Total atoms in sample
0.0548
3.30e+22
3.96e+23
1.45e+23
4.34e+23
0.240
0.0420
0.00927
2.53
5.58e+21
Question Details
For each chemical term, select the appropriate examples. (Select all that apply.)
(a) homogeneous mixture
1022
7.59e+22
3.35
1022
ZumChem8 1.E.028. [1068721]
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oil and water mixture
brass (Cu + Zn)
coffee
saltwater
glucose
pure carbon
(b) heterogeneous mixture
hydrogen gas
book
desk
liquid mercury
argon gas
tree
(c) compound
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copper (Cu)
glucose (C6H12O6)
carbon dioxide (CO2)
water (H2O)
sodium chloride (NaCl)
oxygen (O2)
(d) element
zinc
fluorine
chloroform
ethanol
copper
diethyl ether
(e) physical change
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boiling water
combustion of gasoline
dry ice subliming
freezing water
melting a popsicle
photosynthesis
(f) chemical change
boiling water
combustion of gasoline
dry ice subliming
freezing water
melting a popsicle
photosynthesis
45.
Question Details
ZumChem8 1.E.030. [1068695]
Indicate the number of significant figures in each of the following statements. (If the number is an exact number, as in 100
cm in a meter, then type "infinite" for the number of significant figures.)
(a) One inch is approximately 2.5 cm.
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2 -or- two
(b) This book is almost 1200 pages.
2 -or- two
(c) One gallon is about 3.8 L.
2 -or- two
(d) This boat is approximately 900.00 tons.
5 -or- five
(e) A gram is exactly 1000 mg.
infinite -or- infinite
(f)A liter is approximately 1.059 qt.
4 -or- four
46.
Question Details
ZumChem8 1.E.033. [1070594]
Round off each of the following numbers to the indicated number of significant digits and write the answer in standard
scientific notation.
(a) 0.00034177 to four digits
3.418e-04
(b) 107.645
102 to two digits
1.1e+04
(c) 17.0425 to three digits
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1.70e+01
(d) 3.322
105 to two digits
3.3e+05
47.
Question Details
ZumChem8 1.E.062. [1070251]
A rectangular block has dimensions 2.9 cm
2.0 cm
-
10.0 cm. The mass of the block is 645.0 g.
(a) What is the volume of the block?
58 cm3
(b) What is the density of the block?
11 g/cm3
48.
Question Details
ZumChem8 2.E.054. [1212694]
Write the atomic symbol (AZX) for each of the isotopes described below.
(a) number of protons = 20, number of neutrons = 20
40
Ca
20
(b) the isotope of boron with mass number 10
-
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10
B
5
(c) Z = 53, A = 132
132
I
53
(d) atomic number 29, number of neutrons = 36
65
Cu
29
(e) Z = 11, number of neutrons = 12
23
Na
11
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(f) number of protons = 12, mass number 23
23
Mg
12
49.
Question Details
ZumChem8 2.E.056. [1068730]
How many protons, neutrons, and electrons are in each of the following atoms or ions?
Protons
62
28
Ni
34
28
Au
79
118
79
Co2+
27
33
25
O2-
8
10
10
Tc3+
43
54
40
1
2
0
79
27
18
8
97
43
3
1
Electrons
28
197
60
Neutrons
H+
-
46 of 52
50.
Question Details
ZumChem8 2.E.091. [1068703]
-
The formulas and common names for several substances are given below. Give the systematic names for these substances.
(Enter your answer using the format copper(II) chloride for CuCl2.)
(a) sugar of lead, Pb(C2H3O2)2
lead(II) acetate
(b) blue vitrol, CuSO4
copper(II) sulfate
(c) quicklime, CaO
calcium oxide
(d) Epsom salts, MgSO4
magnesium sulfate
(e) milk of magnesia, Mg(OH)2
magnesium hydroxide
(f) gypsum, CaSO4
calcium sulfate
(g) laughing gas, N2O
dinitrogen monoxide -or- nitrous oxide
51.
Question Details
ZumChem8 3.E.007. [1053052]
A new grill has a mass of 30.0 kg. You put 1.0 kg of charcoal in the grill. You burn all the charcoal and the grill has a mass
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of 30.0 kg. What is the mass of the gases given off? (Assume that the charcoal is pure carbon solid and that it burns
completely in oxygen.)
3.7 kg
52.
Question Details
ZumChem8 3.E.009. [1053073]
-
You may have noticed that water sometimes drips from the exhaust of a car as it is running. Is this evidence that there is
at least a small amount of water originally present in the gasoline?
Yes
No
Explain.
Key: Water, along with carbon dioxide, are products of the combustion of hydrocarbons (such as octane in gasoline).
53.
Question Details
ZumChem8 3.E.016. [1070595]
Consider the equation below.
2A+B
→ A2B
If you mix 2.2 mol of A with 2.2 mol of B, what amount (moles) of A2B can be produced?
1.1 moles
-
48 of 52
54.
Question Details
ZumChem8 3.E.033. [1053069]
-
An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu,
22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu.
Calculate the average atomic mass.
207.2 amu
Identify the element (Give the symbol).
Pb
55.
Question Details
ZumChem8 3.E.061. [1053057]
-
ZumChem8 3.E.063. [1070587]
-
What amount (moles) are represented by each of these samples?
(a) 170.0 g Fe2O3
1.064 mol
(b) 20.0 mg NO2
0.000435 mol
(c) 1.8
1016 molecules of BF3
3.0e-08 mol
56.
Question Details
What number of atoms of nitrogen are present in 8.50 g of each of the following?
(a) magnesium nitride
1.01e+23 atoms
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(b) lead(II) nitrate
3.09e+22 atoms
(c) glycine, C2H5O2N
6.82e+22 atoms
(d) calcium nitrate
6.24e+22 atoms
50 of 52
57.
Question Details
ZumChem8 3.E.004. [1053085]
-
Nitrogen (N2) and hydrogen (H2) react to form ammonia (NH3). Consider a mixture of six nitrogen molecules and six
hydrogen molecules in a closed container. Assuming the reaction goes to completion, what will the final product mixture
be?
number of NH3 molecules
4
number of N2 molecules
4
number of H2 molecules
0
Which of the following equations best represents this reaction?
N2 + 3 H2
6 N2 + 6 H2
N2 + H2
4 NH3 + 4 N2
NH3
N + 3 H2
2 N2 + 6 H2
58.
2 NH3
NH3
4 NH3
Question Details
ZumChem8 3.E.034. [1070582]
An element "X" has five major isotopes, which are listed below along with their abundances.
Percent
Natural Abundance
Mass (amu)
46
8.00%
45.952690
47
7.30%
46.951764
48
73.80%
47.947947
Isotope
X
X
X
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49
5.50%
48.947841
50
5.40%
49.944792
X
X
Calculate the average atomic mass.
47.9 amu
What is the element?
Titanium -or- titanium -or- Ti
59.
Question Details
ZumChem8 3.E.099. [1053072]
Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel
rocket motors. The reaction is given below.
Fe2O3(s) + 2 Al(s)
2 Fe(l) + Al2O3(s)
What masses of iron(III) oxide and aluminum must be used to produce 20.0 g iron?
iron (III) oxide
28.6 g
aluminum
9.66 g
What is the maximum mass of aluminum oxide that could be produced?
18.3 g
Assignment Details
Name (AID): AP Chem 2013-2014 Summer Assignment (2549892)
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