Download final review cp2 1213 by chapter

Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, + solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 1: Predict the products, write a balanced chemical equation (including states of matter),
and indicate what type of reaction we are talking about (you may need your solubility chart)!!!
aqueous potassium iodide and aqueous lead II nitrate react to produce a solid precipitate
and aqueous solution.
Balanced chemical equation =
Reaction type =
Chapter # 1 Chem I Review:
Naming and Formulas
Reaction Types
1. What type of reaction is:
3Al(s) + 3AgNO3(aq)  3Ag(s) + Al(NO3)3(aq)
a. synthesisb. decomposition
c. single replacementd. double replacement
2. What type of reaction is:
sodium bicarbonate → sodium carbonate + carbon dioxide + water
a. synthesisb. decomposition
c. single replacementd. double replacement
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3. Predict the products, write a balanced chemical equation (including states of matter), and
indicate what type of reaction we are talking about (you may need to use your solubility chart)!!!
aqueous lithium hydroxide and aqueous cupric nitrate react to produce a precipitate and
an aqueous solution.
Balanced chemical formula =
Reaction type =
4. Predict the products, write a balanced chemical equation, and indicate what type of reaction
we are talking about!!!
the electrolysis (decomposition) of aqueous cupric chloride →
balanced chemical equation =
reaction type =
5. In lab you combine solid copper and aqueous silver nitrate. You observe that the copper is
turning a silver color and the liquid is turning blue. Write a balanced chemical reaction
including states of matter.
Reaction type =
6. Choose the observations that you might expect to correspond with the following reaction:
2H2(g) + O2(g)  2H2O(g)
a.
b.
c.
d.
e.
nothing they’re all colorless gases
emission of light and heat (energy)
formation of a precipitate
aqueous products
aqueous reactants
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 2: Calculate the molar mass of barium phosphate.
Chapter # 2 The Mole:
Molar mass conversions, Avogadro’s number, Avogadro’s Law
Particles
_________
_________
Mass
(grams)
Molar
mass
_______
Avogadro’s
law – 22.4
L/mol
Avogadro’s #
= __________
_______ in
_______
1. Which of the following statements are true:
I. A mole is a counter because it’s always 6.022e23.
II. Avogadro’s number is 22.4.
III. Avogadro’s law is the same thing as his number.
a. I only
b. II only
c. III only
d. I and II
e. II and III
f. I and III
g. I, II, and III
h. none
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2. How many grams of nitrogen (N) do you have, if you have 3.5 moles? SHOW WORK!
3. 2.5 mols of S = _____ atoms of S. SHOW WORK!
4. Molar mass of aluminum oxide? SHOW WORK!
5. 1.2 * 1024 molecules of O2 = ______ grams of O2? SHOW WORK!
6. A chemical reaction produced 112 L of carbon monoxide gas at STP. What was the mass (in
grams) of the carbon monoxide produced?
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 3: Calculate the number of moles of water produced when 3.3 moles of Cu(NO3)2 are
produced in the reaction below:
3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l)
Chapter # 3 Stoichiometry:
Mole ratios, limiting and excess reactants
_______ 1. Which of these expressions is an incorrect interpretation of the balanced equation?
2S(s) + 3O2(g) → 2SO3(g)
a. 2 atoms S + 3 molecules O2 → 2 molecules SO3
b. 2 g S + 3 g O2 → 2 g SO3
c. 2 mol S + 3 mol O2 → 2 mol SO3
d. none of the above
2. How many molecules of NO2 are produced when 2.0 × 1020 molecules of N2O4 are
decomposed according to the following equation?
N2O4(g) → 2NO2(g)
c. 2.0 × 1020
d. 4.0 × 1020
a. 4
b. 1.0 × 1020
3. How many liters of CO(g) at STP are produced when 68.0 g of CaCO3(s) is heated
according to the following equation?
CaCO3(s)
a. 0.679 L
b. 15.2 L
CP Chem II Final Review
CaO(s) + CO2(g)
c. 68.0 L
d. 30.4 L
5
4. The equation for the complete combustion of methane is
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
To calculate the number of grams of CO2 produced by the reaction of 29.5 g of CH4
with O2, the first conversion factor to use is
a.
1 mol CH 4
16.0 g CH 4
2 mol O2
b. 1 mol CO2
c.
16.0 g CH 4
1 mol CH 4
29.5 g CH 4
d. 2 mol CO
2
5. In any chemical reaction, the quantities that are conserved are
a. the number of moles and the volumes.
b. the number of molecules and the volumes.
c. mass and number of atoms.
d. mass and moles.
Questions 6 and 7 refer to the following equation:
3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l)
6. Calculate the number of moles of nitrogen monoxide produced when 3.3 mol of
Cu(NO3)2 are formed in the reaction.
7. How many grams of Cu would be needed to react with 2.0 mol HNO3?
8. (2 points) Solid sodium and chlorine gas react in a synthesis reaction to produce sodium
chloride. If the reaction started with 4 moles of Na and 3 moles of Cl2, what was the limiting
reactant – SHOW WORK!?
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 4: Which noble gas would you expect to effuse the fastest? WHY?
Chapter # 4 Gas Laws:
You will be provided with the information below:
1 atm. = 760 mm Hg = 101,300 Pa = 14.7 psi
R = 0.0821 atm.*L / mol*K
OR
8.314 kPa*L / mol*K
1. Does the graph below correctly represent the general relationship between pressure and
volume? Explain what you decide (Why or why not).
Volume (L)
Boyle’s Law
0
1
2
3
4
Pressure (atms.)
2. Does the graph below correctly represent the general relationship between pressure and
temperature? Explain what you decide (Why or why not).
Gay Lussac's Law ???
Pressure (atms.)
1.8
1.6
1.4
1.2
1
0.8
18
23
28
33
38
Tem perature (C)
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3. Which gas would you expect to effuse the fastest: fluorine, chlorine, or bromine? Why?
4. Which of the following statements explains one way a real gas differs from an ideal gas?
a.They are the same!
b.The particles of a real gas do not attract or repel one another.
c.The particles of a real gas have volume.
d.The particles of a real gas are in constant random motion.
e.The kinetic energy of a real gas depends on temperature.
5. Circle any and all of the choices below that apply: Gases can…
A. expand B. flow
C. compressD. diffuse
6. The average kinetic energy of water molecules is greatest in
a. steam @ 200C
c. liquid H2O @ 373 K
b. liquid H2O @ 90C
d. ice @ 0C
7. When you increase the temperature of a gas, what causes the corresponding increase in
pressure (BE VERY SPECIFIC!)?
8. Water could be made to boil at 105C by
a. applying a great deal of energy.
b. increasing the air pressure above the water.
c. heating the water more gradually.
d. decreasing the air pressure above the water.
9. Is the boiling point of water at the top of Mount McKinley (the highest point in North
America) higher or lower than it is in Death Valley (the lowest point in North America)?
EXPLAIN!
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 5: What intermolecular forces exist for NH3? Put them in increasing order of strength.
Chapter # 5 Inter and Intramolecular Forces:
1.Which of the following explains why methane (CH4) has a boiling point of – 161 °C and
octane (C8H18) has a boiling point of 125.6 °C.
A.the London dispersion forces are stronger in methane
B.the hydrogen bonds are stronger in octane
C.octane can hydrogen bond and methane cannot
D.the hydrogen bonds are stronger in methane
E.the London dispersion forces are stronger in octane
2.Which of the following molecules has a dipole moment? WHY?
A.CH4
B.CO2
C.PCl3
D.Cl2
E.N2
3.H2S is a gas at room temperature while H2O is a liquid. What can explain this difference?
A.H2S has London dispersion forces only
B.The greater electronegativity of O allows hydrogen bonding in H2O.
C.H2O molecules have smaller dipole moments than H2S.
D.H2S is a heavier molecule.
E.H2S is a smaller molecule.
4. List the three states of matter in order of increasing intermolecular attraction.
CP Chem II Final Review
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5. What intermolecular forces exist for HBr? Put them in increasing order of strength.
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
10
Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 6: What volume of 6 M HCl must be diluted to prepare 500 mL of 1.5 M HCl?
Chapter # 6 Water and Solutions:
1. Define electrolyte. What makes something a strong electrolyte?
2. True OR False? All substances with high solubilities are also strong electrolytes.
_____
3.Which of the following salts is insoluble in water?
A. Na2S
_____
B. MgSO4
C. Pb(NO3)2
D. AlF3
4.In which of the following mixtures will a precipitate form?
A. KCl and NH4NO3
B. Ba(OH)2 and H2SO4
C. Na2SO4 and Al(NO3)3
D. CsI and MgCl2
5. Which of the following would DEcrease the solubility of a gas in a liquid?
a. decreasing the temperature of the solvent
b. decreasing the temperature of the solute
c. decreasing the partial pressure of the gas above the solution
6. Calculate the concentration of a solution (in molarity) that is prepared by dissolving 58.5 g
NaCl in 100 mL water.
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7. What volume of 4 M HCl must be diluted to prepare 250 mL of 1.5 M HCl?
8. Sugar dissolves in water, but is not a strong electrolyte. Explain what must be happening on
the molecular level (feel free to use vocab.).
9. Write the molecular, complete ionic, and net ionic equations for the reaction between aqueous
potassium hydroxide and aqueous calcium nitrate.
( This question was actually covered in Chapter 9 this year) 10. dissociation and hydrolysis of
sodium sulfate (sulfate hydrolyzes water)
Dissociation:
Hydrolysis:
The ending solution will be acidic OR basic?
10. What happens to strong bases when they are placed in water?
Regardless of what strong base we’re talking about this results in an increase in ______ ions.
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 7: From the following enthalpies of reaction,
H2(g) + F2(g)  2HF(g) H = -537 kJ
C(s) + 2F2(g)  CF4(g) H = - 680 kJ
2C(s) + 2H2(g)  C2H4(g) H = +52.3 kJ
calculate H for the reaction of ethylene with F2:
C2H4(g) + 6F2(g)  2CF4(g) + 4HF(g)
Chapter # 7 Thermodynamics:
1. Fill in and study the chart below:
Recall: ΔG = ΔH – TΔS
ΔH (- / +)
ΔS (- / +)
ΔG (- / +)
Spontaneity
Spontaneous at all temperatures
Non-spontaneous at all temperatures
Spontaneous at high temperatures
Spontaneous at low temperatures
2. Determine whether the following describe endothermic or exothermic processes.
ENDO / EXO
a.The enthalpy of the system decreases.
ENDO / EXO
b.The products have more stored energy than the reactants
ENDO / EXO
c.∆H for a system has a negative value.
3. Determine if the following have positive or negative entropy changes.
+ –
a. The entropy change suggests a spontaneous reaction.
+ –
b. 2 NH3(g) + CaCl2(s)  CaO(s) + 2 NH4Cl(s)
+ –
c. 2H2(g) + O2(g)  2H2O(g)
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4. Determine if the following have positive or negative changes in Gibbs Free energy.
+ –
a. A reaction that is spontaneous at all temperatures.
+ –
b. A reaction with a negative ΔH and a positive ΔS.
5. Using the reaction below, Calculate the enthalpy change for the formation of 30.0 g KCl(s).
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
6.
∆H = − 89.4 kJ
Calculate the standard heat of formation for acetic acid from the following reactions.
GOAL: 2 C(s) + O2(g) + 2 H2(g) → HC2H3O2(l)
C(s) + O2(g) → CO2(g)∆H° = – 394 kJ
HC2H3O2(l) + 2 O2(g) → 2 CO2(g) + 2 H2O(l) ∆H° = – 871 kJ
H2(g) + ½ O2(g) → H2O(l)∆H° = – 286 kJ
7. Use the information shown in the table to determine the standard entropy change for the
formation of nitrogen dioxide shown in the reaction below.THEN explain whether your
calculation makes sense using what you know about predicting changes in entropy!
2 NO(g) + O2(g) → 2 NO2(g)
Formula
NO(g)
O2(g)
NO2(g)
∆H˚f
(kJ/mol)
90.37
0
33.84
∆G˚f
(kJ/mol)
86.71
0
51.84
S˚
(J/mol-K)
210.62
205.0
240.45
Explanation = ______________________________________________________
__________________________________________________________________
__________________________________________________________________
8. Calculate ∆G° for a rxn at 127°C w/ ∆H° = – 1127.4 kJ and ∆S° = – 255.4 J/K. UNITS!
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 8: Equilibrium system: I2(g) ⇄ 2 I(g) H = + 151 kJ at 1000°C. How will the following changes
affect the system?
a.
b.
c.
Iodine atoms are added ______________________________________
The system is compressed ______________________________________
Temperature is increased ______________________________________
Chapter 8 Reaction Rates and Equilibrium:
1. How does a catalyst change the reaction rate (be specific)?
2. _______ What is the expression for Keq for this reaction?
2H2O(g)
a.
K eq 
 2H O
H   O 
2H2(g) + O2(g)
2
2
2
b.
K eq 
 2H    O 
 2H O
2
2
2
H   O 

 H O
2
c. K eq
2
2
2
 H O

H   O 
2
d. K eq
2
2
3. For which of the following will the equilibrium mixture be comprised of mostly products
(Choose the best answer)?
A. Kc = 6.5 x 10 – 13
B. KC = Q (any reaction)
C. Kc = 2.2
D. Kc = 6.1 x 10 9
4. Which of the following equilibria will shift, in either direction, when the system is
compressed (Circle all that will)?
I2(s) ⇄ I2(g)
N2(g) + O2(g) ⇄ 2 NO(g)
2 HI(g) ⇄ H2(g) + I2(g)
2 HI(g)
⇄
H2(g) + I2(s)
5. The following system has ∆Hforward = + 603 kJ. Ni(CO4)(g) ⇄ Ni(s) + 4 CO(g) To get a better yield of
product, one should …
A.
B.
C.
D.
increase temperature and increase container volume.
increase temperature and decrease container volume.
decrease temperature and increase container volume.
decrease temperature and decrease container volume.
CP Chem II Final Review
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2
15
2
6. For a reaction involving a single reactant, the following data were obtained.
rate (M/min)
0.20
0.20
0.19
conc.
(mol/L)
0.100
0.200
0.300
0.20
0.400
Determine the order of the reaction. Either show work or explain!
7. If a reaction is second order in A, tripling the concentration of A, does what to the rate?
8. Below is a 2-step mechanism for the rxn of NO2 with CO (all gases):
NO2 + NO2  NO3 + NO
slow
NO3 + CO  NO2 + CO2
fast
a. What is the net reaction?
b. NO3 is an example of _________________________________________________.
9. For the system N2(g) + 3 H2(g) ⇄ 2 NH3(g), KC is 0.10 at a certain temperature. Calculate [N2] if
[NH3] = [H2] = 2.0 M.
10. At 100 °C, KC = 0.56 for PCl5(g) ⇄ PCl3(g) + Cl2(g). In a 2-L flask, a gaseous mixture contains 0.210 mol
Cl2(g), 0.350 mol PCl3(g) and 0.750 mol PCl5(g).
A.Determine the value of Q.
B.Is this system at equilibrium?
C. In which direction will the system react?
SHOW YOUR WORK!!!
A.Q = __________
B. YES NO
C. right
left
no shift
Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
16
Name _______________________________________________
Period _______
CP Chem II Final Review Packet
You will be provided a periodic table, polyatomic ions sheet, and solubility
chart. The final Exam covers chapters 1-9 w/ an emphasis on the 2nd half of the year.
ATB 9: For each of the following, fill in the concentration of the requested ion, the pH, and the
type of solution (acid, base, or neutral).
Concentration
[H+] = 1  103
[OH] =
[OH] = 1  104
[H+] =
pH
Solution Type
Chapter # 9 Acids, Bases, and Salts:
1. Fill in the chart below with simple brief definitions:
Type
Arrhenius
Brønsted-Lowry
Lewis
Acid-Base Definitions
Acid
Base
2. Use the reaction below to fill in the blanks:
HC2H3O2 + NH3  NH4+ + C2H3O2Acid = __________________
Base = __________________
Conjugate acid = __________________
Conjugate base = __________________
3. Among the following, which solution is the most acidic?
a. [H+] = 1 × 10–5 mol/L
c. [OH] = 1 × 10–7 mol/L
b. pH = 3
d. pH = 10
CP Chem II Final Review
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4. The monoprotic acid from among the following is
a. H2CO3.
c. H3PO4.
b. H2SO4.
d. HCl.
5. Among the following Ka values, which represents the strongest acid?
a. Ka = 1.2  103
c. Ka = 8.7  108
b. Ka = 3.4  105
d. Ka = 5.8  1010
6. How many moles of Mg(OH)2(aq) would be required to neutralize 3.0 mol HCl(aq)?
a. 6.0 mol
c. 1.5 mol
b. 2.0 mol
d. 3.0 mol
7. Essay: Compare and contrast acids and bases.
Include all of the following:
Ka and Kb
pH values
H+ and OH- ion concentrations
Extent of dissociation (ionization) in solution
Explanation of pH indicators
Anything else you feel important and relevant
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Review Labs, ATBS, and your notes!!!
CP Chem II Final Review
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