no reaction. If the reaction will occur, predict the products of the reaction and write a balanced chemical
reaction.
b. MgCI2 + Ba-->
c. I Zn +a114-1CI ->
d.DÿH20 + I St -->
%o,c.lÿ-u ux%
I z,£1z + i H
,
s,-(o/%z + I Hÿ
toÿt ,ÿ q" ÿ_47-ÿ--ÿ.z
7, ÿC_%..ÿ, [,>
Use the Solubility charts and Predict if the following compounds are soluble or insoluble. Write soluble (aq)or insoluble solid(s)
a. KCI c'JQÿtx%J\ÿ (ÿ e NH4OH. %0\%%s\ÿ. (m.ÿ}
, In the reaction shown below, what is the name of the precipitate? (Hint: figure out if your products form
solids(s) or aqueous solutions (aq) .... the solid is your precipitate)
BaCI ÿ(,ÿq)+ Na ÿ SO ,ÿ(aq)ÿ 2NaCI (ÿ)+ BaSO ÿLÿ
% Barium Sulfate
b. Sodium Chloride
2
+ Determine if the following pairs of solutions will form a precipitate.
• If they do form a precipitate, write the balanced reaction.
• If they do not form a precipitate, write NVR for no visible reaction.
c. I CuSÿOlÿ(aq)÷ ÿ ÿ)ÿ
9. Balance the following combustion reactions.
a. Ic4H8 ÷LoO2÷ 4co2 +ffH20
i t " ÿl
Gq C / x,4ÿ-'-/
0 ? "ÿ ÿ ++ÿ,ÿ 0 Zÿÿ+ " 12
b oÿCsHm ++ÿ502 ÷ IbCOz + IÿHzO
,-, ÿ V,ÿ_i/" Q |ÿJt..o= @" ÿ f+ÿ- tb2xlÿ=SZ"> ÿ0
10. Based on the oxidation numbers (charge)known for the other element(s), determine the oxidation
number of the underlined element.
a. CÿO ÿ1
c. ÿ_ÿo 41
e. AICIÿ
11. Define oxidation: ÿecLcSÿioÿx tÿ,ÿ O. \6ÿ5 ÿ£ tzÿeCScron5 ÿCÿOvo)(L iS iÿqC'Ceÿ:'({ÿ
13. In an oxidation-reduction reaction, reduction is defined as the -
A. gain of protons.
gain of electrons.
C. loss of electrons.
D. Ioss of protons.
OIL RIGoxidation is loss reductioIÿ is ÿatn
14. Determine the oxidation numbers of each element in the following reaction and then complete the chart todetermine which is being oxidized and which is being reduced. (labeloxidation numbers for allelements)
Fe+ 2HCI -) Hÿ + FeCIz
Element Ox.# Reactanÿ $!der OX,ÿ Pÿoducts side LosetGain e"i
/c5£ÿ
1'ÿ (b'+ÿ,2
Oxidized!Reduced
b ,ÿi 4 ÿ@>o
t),ÿ ct uÿ+.ÿd o,q
15. The chemical equation below represents a redox reaction.
4 HCI + MnO2 -ÿ MnCla + 2 H20 ÷ CI2What occurs during this reaction?
A .The manganese is oxidized, and its oxidation number changeÿ
(ÿThe is and its oxidation number from +4 to +2.manganese reduced, changes
C. The manganese is oxidized, and its oxidation number changes from +4 to +2.
D.The manganese is reduced, and its oxidation number changes from +2 to +4.
Stoichiometry
Mole Math-)
16. Complete the mole road map. You will use this for the Mole Math and Stoichiometry sections.
17. Find the mass of 0.89 tool of CaCI2. CÿI -- ÿ, ÿ ÿ ÿ Z
-!t
18. Determine the number of moles of hydrogen that are in 3662.ÿof this diatomic element.
33. The actual amount of product fKrmed in a reaction during lab was ÿ. You however jcÿhat
would form. Wha.ÿt iÿeld of this product?
gÿc:ÿd aÿ.\c\ ,- " '-' \ ÿ xlOÿ ÿ/S-% ;etcl
34, Dÿÿpeÿerittÿd if 86.0 g of ammonia is produced when 66,0 g hydrogen tea .,
/-
5qa3Which reactant is the limiting reactant?
Gas Laws-->
35. In a sample of gas, what causes pressure? Answer in a complete sentence.
36. How does the behavior of gas particles change as temperature is decreased? How does this affect the
37. When performing gas law calculations, temperature must be in what units? ÿJ'ÿ ÿ'1 ÿ ÿf'ÿ
6
¼38. A gas at conÿ is in a container with a volume of 15 L.
What will theÿe inside the container be if n9 qas has been removed?
f%Vz
The container is contracted to 7.5 L.
Use the following graphs to answer the next 7 problems.
-oÿ9ÿ\The Relationship betweenVolume and Pressure of a Gas
0 20 40 60 80 100
Volume (mL)
Graph #2: The Relationship betweenVolume and Temperature of a Gas
..... i ....... i ....... i .................] < - ....... ÿ-- i ..............
i ÿ L. '<' . ..... i i.i TLiTLI : 12 :I i : : : ' " "
0 20 40 60
Temperature (K)
39. Which graph represents Boyle°s Law? ÿT-ÿÿh ÿ ÿL
40. Which graph represents Charles°s Law? ÿ VOÿ/h ÿ
41. Which graph has the same shape as Avogadro's Law? 9 f-ÿ0/"ÿ -ÿ
42. In Graph #1, what is the pressure on 40mL of gas? ÿ.ÿ0ÿ ÿ ÿ ÿ ÿ0ÿ
43. In Graph #2, what is the volume when the temperature reaches 30K? 0ÿGÿ
44. Which graph represents an inverse relationship? ÿ ÿÿ ÿ /
45. Which graph represents a direct relationship? ÿ lÿ ÿ ÿ
Show work (with units) for the following nine problems .... ÿ 1.3ÿatnÿ?46. What is the volume of a sample of gas that contains 1.ÿnÿ_ ol at 780 K and
mot,, K.
47. A balloon inflated in a room at 24°C has a volume of 4.0ÿ_ÿ_L
58°C. What is the new volume if the pressure remains constant?
The balloon is then heated to a temperature of
i
52. What volume does 0.742mol of argon gas occupy at STP?
fk=O ,q q).mÿ,l
53. A 6.0 L sample atÿCÿand 2ÿof pressure contains 0.5 moles of a gas. If an additional 0.25 moles ofgas Ot the same pressure and temperature are added, what if-s thÿhe-ÿ?
"J, :: Is,OL Vz= ÿ n, ¢ÿz ÿ Ll
54. If 4.5Q of oxygen gas is placed in aÿcontainer at 450K, ÿlculate the pÿ. ÿÿcontainer.
1k"T-= qÿ-b
55. At high altitudes, pilots ha:e to supplement their supply of oxygen. In thiA mix____ture__ ther_ e_are _0yÿn and
nitrogen gases. If nitrogens artial pressure is 550mmHg,_ ÿcalculaÿe t-he partial pressure of oxygen:ygen/lif the
tot tÿ__pressure is 945mmHg.
Solutions Review-->
100
90
8OI
0o
oo
so
4oz,
30
o
Which chdracteristic of water explains its ability to dissolve a great
10 20 30 40 50 60 70 80 90 100Tempemlure (°O)
56.
variety of things?a. its transparency in lightb. its electrical conductivityc. its physical state of matter
es molecular arrangement and shape
57. Does Ceÿ(SO4)3 resemble a solid or gas
10
58. Explain your answer to #56. -ÿ%# ÿ a ÿOi'll I-ÿ 0-ÿ'- ÿ ÿS
59. What is the solubility of Pb(NOÿ)ÿ at 20°C?
60. If you have 30g of KCIOÿ at 40°C, the solution is:a. unsaturated
b. saturated
supersaturatedd. slightly saturated
61. How many grams of KzCrÿO7 are needed to saturate 200g of HÿO at 50°C? _ÿ___ÿ ÿ-ÿ-ÿ-ÿ'-ÿ
62. Increasing the pressure of 35g solid NaCI at 20°C would the solubility. ÿ
increase decrease
63, You need to make a solution containing 150g of potassium chloride in 3009 of water. Whattemperature is required? (Use solubility graph on the previous pagd)
[t .... ÿ-t
-T-
64. Circle the condition that causes salt to dissolve faster in water.rock salt or in'granulated formj)when allowed to stand or ÿ_.£ÿ?
(ÿahigher-}emperafÿrÿ) or a lower temperature?
65. Where would a data point be on a line graph ira solution is? unsaturated: 0ÿ)-3 ÿ iÿ ÿ] [ÿ ÿ ÿsaturated: 0 I% A'ÿ \ÿ ÿ ,or supersaturated: CLÿ<':,-\'>,ÿ "ÿ /{ ÿl ÿL
66. If two liquids dissolve each other, they are said to be fÿi ÿc-3ÿ') \ate
67/ÿHow does the solubility of solid substances change as the temperature of the solvent increases?Qÿ) The solubility increases for most solids.
b. The solubility decreases for most solids.c. The solubiiity remains constantl
68. How does the solubility of a gas change with the increase in temperature?
69. What types of compounds when dissolved in water will cause the solution to be electrolytic?
70. Label the partial charges and the element symbols on the water molecule below.
71.
light:Which of the following solutions are considered electrolytes and would cause a light bulb to give a bright
. sugar solution
. NOa solution,-ÿ) CaCla solution
d. kg
10
(
72. Match the following terms with their correct definitiona) Hydrogen bondb) Polar moleculec) Nonpolar moleculed) Electrolytee) Nonelectrolyte
Molecule in which there is a partial negative charge on one end and a partial positive charge on theother end
_ ÿ A substance that does not dissolve to form ions in an aqueous solutionIX Bond occur between a hydrogen and the negatively charged end of another molecule
A substance which forms ions in an aqueous solutionMolecule which has no separation of charge, so no positive or negative poles are formed.
73. Describe the settling of particles for each of the following:
86. As hydrogen ion concentration of an aqueous solution increases, the hydroxide ion concentration of thissolution
a. increases
ecreases
c. remains constant
87. Which is not a property of an acid?a. conducts electricityb. reacts with metalsc. corrosive
(ÿtaste bitter
12
88. Which represents the most acidic substance?Apple Juice (pH = 3.0)Black Coffee (pH = 5.0)
c. Hand Soap (pH = 10.0)d. Household Ammonia (pH = 12.0)
89. Which substance will produce the highest pH?a. HCl(aq)b. H20(I)c. NaCl(aq)
aOH(aq)
90. Which pH indicates a solution that has the highest concentration of OH- ions?a. 2
b. 4
91.
c. 6
WhicÿHindicates a solution that has the highest concentration of H+ ions?
kÿjÿ-5.4
c. 6
92.
d. 8
Using the Kw constant and equation, solve for the following:a. Calculate the [OH-] of a solution with an [H+] of 1.6X106'
I b X / o --,/ÿ/o@_
\, Oÿ,lÿlb. Calculate the pH of a solutign with an [OH].concentration of 1.85 X 10-1°. (Hint: 2 ste
...,,. _'7 ..,'--14-t93. ÿof 3.50 L of solution that contains 60._.0ÿoÿoÿ
• LO °,ÿ'ÿ____ÿ ÿ_ I,
94. Write a complete and balanced equation for the following acid-base reaction:
b.ÿHC, , Mg(OH)ÿ ÷ ÿ3Cb + ;ÿ)b
13
95. Calculate the concentration of sulfuric acid if 65.OraL of this acid is neutralized by 23.0mL of .15Mpotassium hydroxide? __k HzSO4 + ÿ KOH ÷ __L KzSO4 + ÿHzO.
Use:
MoV.___ÿ = MbV____bb
Na rib
COVALENT BONDING ->
96. Define ionic and covalent bonding.
97.
98. How many electrons are inÿ single bond
[
Define the octet rule. What are the exceptions? ÿ)ÿ ÿ;ÿ\ÿr'ÿ ÿxÿ e={ ÿ ¢ÿaÿ
double bOnd l ff triple bond /O ?
99. Draw the Lewis structure (dot diagram) for the element nitrogen. How many valence electrons?
5"
100. Determine if the following bonds are ionic, polar, or nonpolar using the electronegativity values in
the table below.Element
HBrCN0FCII
NaP
o,o-o,
23,0
Electronegativity2.1
2.8
2.5
3.0
3.5
4.0
3.0
2.5
0.9
2.1
po m e
• For the polar bonds, circle which bond was the most polar? ÿ ÿ"
• Also, assign the positive pole(c;+) and negative pole(g -) for the bond.
14
101.Draw the Lewis structure for the following molecules.a. Label the type of bonds (polar or nonpolar covalent).b. What is the shape?c. Is the molecule polar or nonpolar? ÿ O ÿ ÿF7 ÿ ÿ
106. Make enthalpy diagrams for the two chemical reactions from above, showing clearly the amount ofenergy released or gained. Label the reactants (R), products (P), activation energy (Ea), and AHrxn foreach diagram.
Exothermic Change
b
Endothermic Change
Time
107. Classify eachÿf the following as an exothermic or endother,ÿic pÿ'ocess.Melting ice cubes ÿ GO Baking Bread i ÿtÿ_-ÿBurning a candle Q ÿ:.ÿ Splitting a gas molecule apart e,ÿ 0Evaporation of water ÿrÿ CÿO Formation of snow in clouds Qÿ
108. Using the enthalpy of formation chart, (a) find the AH for the following reactions (b) classify as
endothermic or exothermic, and (c) rewrite the equation with heat included on the correct side of the
Compound
NO (g)(g)
NaOH (s)HCI (g)NaCI (s)HzO (I)H20 (g)
a.AH =
Co
b.
AHfa (k J/tool)+90.4
+33.9
-426.7
-92.3
-411.0
-285.8
-241.8
r) 2 NO(g) + Oz(g) --- 2 NOz(g)( ,,
-- ;g-o
endotherhÿieÿorÿ×otherrn?cÿ'-'ÿ
Rewrite the Thermochemical equation:
16
a. AH=
b,
C,
II) NaOH(s) + HCl(g) .... > NaCl(s) + H20(g)
s-i q,
Rewrite the Thermochemical equation:
109. Calculate the number of joules needed to warm 100 grams of water from 25.0°C to 80.0°C.
110.1 sample of zinc, specific heat of 0.386 Jÿ, released 1,964 joules of heat when it cooled from 92.5°C to65.0°ÿ. What wasÿ mass of the zinc sample? ÿ
q = t,.. ¢_ÿ. ,ÿ
< = - ....
111. Students conduct an experiment where a reaction occurs in a calorimÿÿhe heat
released/absorbed in Joules to the nearest whole number. The specific heat capacity of water is 4.184
