Download BONUS: Which line in the above graph represents G for the reaction

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PAGE 1 of 23
1. When a hypothetical ionic crystal M+X– is heated, it vaporizes to form separate M+(g) and
X–(g) ions. The energy required for this vaporization (the lattice energy) will be greatest when
(A)
the electron affinity of X is small in magnitude and the ionization potential
of M is large in magnitude.
(B)
the heat of vaporization of crystalline M is small.
(C)
the heat of vaporization of crystalline M is large.
(D)
the effective radii of M+ and X– are large.
(E)
the effective radii of M + and X– are small.
2. Which reaction has the largest positive entropy change per mole of product formed?
3.
(A)
S(s) + 3F2(g)  SF6(g)
(B)
SO2(g) + Na2O(s)  Na2SO3(s)
(C)
Fe3+(aq) + SCN–(aq)  FeSCN2+(aq)
(D)
H2O(l)  H2O(g)
The reaction:
You standing on a log,  You falling off a log
is spontaneous at all temperatures because
4.
(A)
H and S are both positive.
(B)
H and S are both negative.
(C)
H is positive and S is negative.
(D)
H is negative and S is positive.
A sample of 25.0 mL of vinegar (acetic acid) is titrated with standard sodium hydroxide
solution, which is 0.500 M. If 30.0 mL of the NaOH solution are required for exact
neutralization (phenolphthalein as indicator), the vinegar is
HAc + OH-  Ac- + H2O
(A)
0.060 M (B)
(E)
6.00 M
PAGE 1 of 23
0.425 M (C)
0.450 M (D)
POINTS:_______
0.600 M
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PAGE 2 of 23
5. Which factor would cause a change in the equilibrium constant, Kc, for this reaction?
2NOCl(g)


2NO(g) + Cl2(g)
(A)
adding NO(g)
(B)
decreasing the volume of the reaction vessel
(C)
cooling the system
(D)
adding an inert gas
6. In which reaction will an increase in total pressure at constant temperature favor formation
of the products?


(A)
CaCO3(s)
CaO(s) + CO2(g)
(B)
H2(g) + Cl2(g)
(C)
2NO(g) + O2(g)
(D)
COCl2(g)


CO(g) + Cl2(g)
BaCO3(s)


BaO(s) + CO2(g) H = + 125 kJ/mol


2HCl(g)


2NO2(g)
7. In the reaction
which change will cause an increase in the pressure of CO2(g) when equilibrium is
re-established?
(A)
increasing the reaction temperature
(B)
decreasing the volume of the container
(C)
adding some more BaCO3(s)
(D)
removing some of the BaO(s)
8. Consider the equilibrium:
energy + 2H2O


H3O+ + OH–
As the temperature of a sample of pure water is increased
(A)
the number of moles of water present will increase.
(B)
the ionization constant for water will decrease.
(C)
both the number of hydrogen ions and hydroxide ions will increase.
(D)
the hydrogen ion concentration will increase and the hydroxide ion
concentration will decrease.
(E)
the ionization constant for water remains unchanged.
PAGE 2 of 23
POINTS:_______
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PAGE 3 of 23
9. In the equilibrium
HS– + H2O


2H3O+ + S2–
the addition of what ion would effectively increase the S2– concentration?
(A)
H3 O+
(E)
Na+
(B)
Br–
Cl–
(C)
(D)
OH–
BONUS: Consider the following reactions:
I
2Ag+ (aq) + SO3= (aq)
II
2H+ (aq) + SO3= (aq)
 Ag2SO3 (s) 
 H2SO3  H2O + SO2 (g)
How will equilibrium I shift on addition of HCl?
(A) There will be no effect
(B) More silver sulfite will ppt out.
(C) Silver sulfite will dissolve.
(D) SO2 gas will be sucked out of the air and into the
reaction vessel
10. Consider the reversible system at equilibrium:
2CO + O2


2CO2 + heat
When CO is removed
(A)
the CO2 concentration will be increased.
(B)
the CO2 concentration will be decreased.
(C)
the amount of each substance will be unchanged.
(D)
the amount of each substance will be increased.
(F)
the result cannot be predicted from the information given.
PAGE 3 of 23
POINTS:_______
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PAGE 4 of 23
11. Which is a proper description of chemical equilibrium?
(A)
The frequencies of reactant and of product collisions are identical.
(B)
The concentrations of products and reactants are identical.
(C)
The velocities of product and reactant molecules are identical.
(D)
Reactant molecules are forming products as fast as product molecules
are reacting to form reactants.
(E)
The numbers of moles of reactants and products are equal.
12.
2X(g) + Y(g)


2Z(g)
H = –335 kJ
Which combination of pressure and temperature gives the highest yield of Z at
equilibrium?
(A)
1000 atm and 500 °C
(B)
500 atm and 500 °C
(C)
1000 atm and 100 °C
(D)
500 atm and 100 °C
(F)
catalyst, 500 atm and 100 °C
13. A solution of sodium acetate in water is observed to become more alkaline as the
temperature is raised. Which conclusion can be drawn?
Na+ + C2H3O2– + H2O


HC2H3O2 + Na+ + OH–
(A)
The forward reaction proceeds with an evolution of heat.
(B)
The forward reaction proceeds with a absorption of heat.
(C)
Acetic acid is less volatile than water.
(D)
Sodium acetate is less soluble in hot water than in cold water.
(F)
At higher temperatures the reaction
Na+ + OH–  NaOH will occur.
PAGE 4 of 23
POINTS:_______
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PAGE 5 of 23
14. In which set are the substances arranged in order of decreasing solubility in water?
(A)
Al(OH)3 > Mg(OH)2 > NaOH
(B)
BaSO4 > CaSO4 > MgSO4
(C)
CaCO3 > NaHCO3 > Na2CO3
(D)
AgCl > AgBr > AgI
BONUS: What do these have in common?
20Ne
19F–
24Mg2+
(A)
the same number of protons
(B)
the same number of neutrons
(C)
the same number of electrons
(D)
the same size
15. Calculate K in terms of molar concentration for the reaction
eq
N2(g) + 3H2(g)


2NH3(g)
when the equilibrium concentration moles per liter are:
N2 = 0.02, H2 = 0.01, NH3 = 0.10.
(A)
2  10–6
(B)
5  103 (C)
5  105 (D)
5  107
16. The equilibrium constant K for the conversion
p
butane(g)


isobutane(g)
is 2.54 at 25 °C. If 1.00 mole of butane is allowed to come to equilibrium, the # of
moles of isobutane in the equilibrium mixture will be
(A)
0.390
(C)
1.65
(B)
0.720
(D)
2.54
PAGE 5 of 23
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PAGE 6 of 23
17. For this reaction, AB3(g) 
 A(g) + 3B(g), what is the equilibrium constant expression if
the initial concentration of AB3 is 0.1 M and the concentration of A is represented by x?
(A)
x · 3x
0.1 – x
(C)
x · x3
(0.1 – 3x)3
(B)
x · x3
(0.1 – x)3
(D)
x · (3x)3
0.1 – x
18. A mixture of 2.0 mol of CO(g) and 2.0 mol of H O(g) was allowed to come to equilibrium
2
in a l L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2(g) in the
equilibrium mixture?
CO(g) + H2O(g)
(A)
1.0
(B)
0.67


(C)
CO2(g) + H2(g)
0.75
(D)
1.3
19. The reaction
Arginine + water


Nitric oxide + Ornithine
catalysed by the enzyme nitric oxide synthase (NOS), has been studied at five widely
different temperatures and the equilibrium constants tabulated.
Equilibrium constant, K
(at various temperatures)
K
K
K
K
1  10–2
2.25
1.0
81
4  10–1
at T1
at T2
at T3
at T4
K at T5
At which temperature will there be the maximum conversion of Arginine and water
to nitric oxide and ornithine, when equilibrium is attained?
(A)
T1
(E)
T5
PAGE 6 of 23
(B)
T2
(C)
T3
(D)
POINTS:_______
T4
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PAGE 7 of 23
20. What is the [OH–] of a solution which is 0.18 M in ammonium ion and 0.10 M in
ammonia?
Ionization Constant for Ammonia
Kb = 1.8  10–5
(A)
(B)
1.3  10–3
1.3  10–5
1.0  10–3
1.0  10–5
(C)
(D)
21. Which possesses the greatest concentration of hydroxide ion?
(A)
a solution with a pH of 3.0
(B)
a 1  10–4 M solution of HNO3
(C)
a solution with a pOH of 12.0
(D)
water
22. According to the Brønsted–Lowry definition, bases, when reacting with acids
(A)
give up protons. (D)
form hydronium ions.
(B)
accept protons. (E)
accept electrons.
(C)
lose electrons.
23. In this reaction, which substances are bases according to the Brønsted–Lowry definition?
HC2H3O2 + H2O
(A)
HC2H3O2 and H2O
(B)
HC2H3O2 and C2H3O2
(C)
H2O and C2H3O2–
(D)
PAGE 7 of 23


H3O+ + C2H3O2–
H3O+ and C2H3O2–
POINTS:_______
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PAGE 8 of 23
24. Which solution has a pH less than 7.0?
(A)
1 M Na2CO3
(C)
1 M NH4NO3
(B)
1 M K2SO3
(D)
1 M NaOH
25. HCl is a strong acid. What is the pH of 200 mL of
0.002 M HCl?
(A)
2.0
(B)
2.7
(C)
3.4
(D)
4.0
26. The pH of a 1.0  10–3 M Ba(OH)2 solution at 25 °C is
(A)
2.7
(B)
3.0
(C)
11.0
(D)
11.3
BONUS: Which equation best represents the net reaction that occurs when sodium hydroxide
and hydrochloric acid solutions are mixed?
(A)
Na+ + HCl  NaCl + H+
(B)
OH– + HCl  H2O + Cl–
(C)
OH– + H3O+  2H2O
(D)
NaOH + H3O+  2H2O + Na+
27. What is the pH of a solution which is 0.10 M in a monoprotic acid, HKlaque, with K =
a
–6
1.0  10 ?
HKlaque + H2O
(A)
1.6


Klaque- + H3O+
(B)
3.5
(C)
5.0
(D)
6.0
BONUS: As maple sap boils down into syrup, will its boiling point go up or down?
Up! Boiling point elevation!
PAGE 8 of 23
POINTS:_______
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PAGE 9 of 23
1. 10.0 mL of a solution of acetic acid, HC2H3O2, requires 25.0 mL of 0.400 M sodium
hydroxide to neutralize it. How many millimoles of acetic acid are present in the sample?
(A)
2000
(B)
1000
(C)
100
(D)
10
2. If 20.00 mL of 0.100 M H2SO4 is exactly neutralized by 50.00 mL of NaOH solution, what
is the molar concentration of the original base solution?
(A)
0.080 M
(C)
0.040 M
(B)
0.250 M
(D)
0.020 M
3. What is the pH of a 0.01 M NaOH solution?
(A)
10–12
(E)
–2
(B)
12
(C)
–12
(D)
4. A solution that has pH of 8 is
(A)
very acidic.
(D)
slightly basic.
(B)
very basic.
(E)
exactly neutral.
(C)
slightly acidic.
5.
Which is the strongest acid?
(A)
(D)
PAGE 9 of 23
HClO (B)
HClO4
HClO2 (C)
HClO3
POINTS:_______
2
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PAGE 10 of 23
BONUS: The pH of the water in the bag is 7.2. What is the [H 3O+]? 6.3 x 10-8M
.
6. The weakest of the bases listed is
Acid
Ka (Ionization
Conjugate Base Constant of Acid)
Cl–
SO42–
HS–
S2–
HCl
HSO4–
H2 S
HS–
(A)
Cl–
(D)
SO42–
(B)
1 x 106
1.2  10–2
5.7  10–8
1.2  10–13
CN–
(C)
HS–
(D)
Which pair constitutes a buffer in aqueous solution?
(A)
HCl and NaCl
(B)
NH3 and NH4Cl (D)
PAGE 10 of 23
(C)
HBr and KBr
HNO3 and NH4NO3.
POINTS:_______
S2–
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PAGE 11 of 23
7.
Calculate the pH of 0.100 M acetic acid. (pKa = 4.72)
(A)
1.000
(C)
2.86
(B)
4.72
(D)
11.14
8. The acid HGr has an ionization constant of 1  10–4. A solution is 0.1 M in HGr and 1.0 M
in the salt K+Gr–. What is a close approximation of the hydrogen ion concentration?
(A)
1  10–3 M
(C)
1  10–5 M
(B)
2  10–5 M
(D)
1  10–8 M
Pote ntiome tric titra tion of Bongkre kic Acid
(isola te d from a a rdva rk sa liva ) by 0.1000 M
Na OH
12
11
10
9
pH
8
7
6
5
4
3
0
10
20
30
40
pH
mL 0.1000 M Na OH a dde d
THE NEXT THREE QUESTIONS REFER TO THE TITRATION CURVE ABOVE
BONGKREKIC ACID IS A WEAK ACID.
9. What is the pH at the equivalence point in the figure?
(A)
4
(C)
7
(B)
9.5
(D)
11.5
10. What is the pKa of Bongkrekic Acid?
(A)
4
(C)
7
(B)
9.5
(D)
11.5
11. The pH range where Bongkrekic acid and its weak base Bongkrekate make the best
BUFFER is:
(A)
0-4
(C)
8-10
(B)
PAGE 11 of 23
6-8
(D)
9.5-10
POINTS:_______
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PAGE 12 of 23
12. The pOH of an aqueous solution is 6.0. What is the [H+]?
(A)
1  10–8 M
(C)
1  10–6 M
(B)
1  10–7 M
(D)
8M
(C)
8
BONUS: What is the pH of 10-8 M HCl?
(A)
1  10–8 M
(B)
6.96
13. A 0.10 M C6H5COOH solution has a pH of 2.59. What is the pKa of this acid?
(A)
5.18
(C)
2.58
(B)
4.18
(D)
1.58
14. What is the pH of a 0.1 M NaF solution?
Ionization Constant for HF
pKa = 3.15
(A)
2.1
(B)
5.9
(C)
8.1
(D)
9.1
15. What is the pH of a buffer solution containing 0.10 M Sodium Klaquate (NaKl) and 0.20
M Klaquic acid (HKl)?
Ionization Constant for Klaquic Acid
pKa = 3.35
(A)
3.00
(C)
3.04
(B)
3.35
(D)
2.02
PAGE 12 of 23
POINTS:_______
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PAGE 13 of 23
16. The hydrogen (hydronium) ion concentration in a 0.1 M solution of HC2H3O2 will be more
than in
Acid
Ka (Ionization
Conjugate Base Constant of Acid)
HSO4–
HF
HNO2
HC2H3O2
H2 S
HS–
1.2  10–2
7.2  10–4
4.0  10–4
1.8  10–5
5.7  10–8
1.2  10–13
SO42–
F–
NO2–
C2H3O–
HS–
S2–
(A)
0.1 M HF
(D)
0.1 M NaHS
(B)
0.1 M HNO2
(E)
0.2 M HC2H3O2
(C)
0.1 M NaHSO4
(F)
A bottle of concentrated sullfuric acid
17. What is the pH of a 0.0100 M solution of NH 3(aq)?
Ionization Constant, pKa
NH4+
9.26
(A)
2.00
(C)
3.37
(B)
10.63
(D)
5.63
18. What is the correct equation for the ion product constant of water?
(A)
[H3O+] + [OH–] = 10–14
(B)
[H3O+]  [OH–] = 10–7
(C)
[H3O+]
= 10–14
[OH–]
(D)
(D)
PAGE 13 of 23
[H 3O + ]  [OH] = 10–14
[H 2 O]2
[H3O+]  [OH–] = 10–14
POINTS:_______
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PAGE 14 of 23
19. A buffer of pH 4.1 is to be prepared from a weak acid and its salt. The best acid from
which to prepare the buffer is
(A)
hydrogen phthalate, Ka = 3.910–5
(B)
benzoic acid, Ka = 6.310–5
(C )
hydrocyanic acid, Ka = 410-10
20. The solubility of BaCO3 is 7.9  10–3 g·L–1. Calculate the solubility product, Ksp .
Molar Mass
197 g·mol–1
BaCO3
(A)
1.6  10–2
(C)
4.0  10–5
(B)
1.6  10–9
(D)
6.2  10–5
21. Typical “hard” water contains about 2.0  10–3 mol of Ca2+ per liter. Calculate the
maximum concentration of fluoride ion which could be present in hard water.
Solubility Product Constant, Ksp
4.0  10–11
CaF2
(A)
1.4  10–4 M
(C)
4.0  10–3 M
(B)
2.0  10–3 M
(D)
2.0  10–8 M
22. What is [OH–] in a saturated solution of Mg(OH) where [Mg2+] = 1.510–5 M?
2
Solubility Product Constant, Mg(OH)2
Ksp = 1.5  10–11
(A)
2.210–10 M
(C)
5.010–4 M
(B)
3.010–5 M
(D)
1.010–3 M
PAGE 14 of 23
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PAGE 15 of 23
24. What is the value of G for this reaction?
3H2(g) + O3(g)  3H2O(l)
H2(g) + 1/2O2(g)  H2O(l)
G = –286 kJ
3O2(g)  2O3(g)
G = +271 kJ
(A)
–15 kJ
(D)
–995 kJ
(B)
–558 kJ
(E)
–1130 kJ
(A) –722 kJ
BONUS A particular chemical reaction has a negative H and negative S. Which statement is
correct?
(A)
The reaction is spontaneous at all temperatures.
(B)
The reaction is nonspontaneous at all temperatures.
(C)
The reaction becomes spontaneous as temperature increases.
(D)
The reaction becomes spontaneous as temperature
decreases.
PAGE 15 of 23
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PAGE 16 of 23
28. Write the equation relating G and Keq
1.
In every electrolytic and galvanic (voltaic) cell the anode is that electrode
(A)
at which oxidation occurs.
(B)
which attracts cations.
(C)
at which electrons are supplied to the solution.
(E)
at which reduction occurs
2. BALANCE THE FOLLOWING REDOX REACTION IN ACIDIC SOLUTION:
Hg22+ + H2  Hg
Hg22+ +2e-  2Hg
H2  2H+ + 2eHg22+ + H2  Hg + 2H+
3.
Five metals are represented by the symbols S, M, C, V, and T. When a solution
containing all five ions at 1 M concentration is electrolyzed with a small applied voltage,
which metal is most likely to be deposited first on the cathode?
Unknown Metals
Standard Reduction Potentials
E0
S2+ + 2e– 
+0.76 V
 S
M2+ + 2e– 
M
+0.44 V

C2+ + 2e– 
C
+0.13 V

V3+ + 3e– 
V
-0.34 V


T+ + e–
T
-3.05 V

(A)
S
(B)
M
(D)
V
(E)
T
(C)
C
BONUS: Which one of these metals is MOST LIKELY to be a GROUP I metal?
T
PAGE 16 of 23
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PAGE 17 of 23
What is the charge of a mole of electrons?
6.
Standard Reduction Potentials
+ 2e–  Zn
Ag+ + e–  Ag
Zn2+
E0 = –0.76 V
E0 = +0.80 V
What is the potential of the cell involving this reaction?
Zn + 2Ag+  Zn2++ 2Ag
(Assume all substances in their standard states.)
(A)
0.04 V
(B)
0.84 V
(C)
1.56 V
(D)
2.36 V
PAGE 17 of 23
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PAGE 18 of 23
9.
Standard Reduction Potential
Br2(l) + 2e–  2Br–(aq)
E0 = +1.06
Ce4+(aq) + e–  Ce3+(aq) E0 = +1.61
V
V
Calculate the standard potential for the reaction
Br2(l) + 2Ce3+(aq)  2Br–(aq) + 2Ce4+(aq)
(A)
–2.67 V (B)
(D)
+2.67 V
–2.16 V (C)
–0.55 V
-
11. From the data given, which reaction is MOST LIKELY to proceed
spontaneously as written?
Standard Reduction Potentials
H4XeO6 + 2H+ + 2e-  XeO3 + 3H2O
E0 =
4+
–
3+
Ce (aq) + e  Ce (aq)
E0 =
–
Br2(l) + 2e–  2Br (aq)
E0 =
2+
Ra + 2e  Ra
E0 =
+
Li + e  Li
E0 =
(A)
2 Ce3+ + XeO3 + 3 H2O  2Ce4+ + H4XeO6 + 2H+
(B) 2Li + Ra  2Li+ + Ra 2+
(C) 2Li+
+ H4XeO6
+ 2H+  2Li + XeO3 + 3 H2O
(D) Ra + Br2  2Br- + Ra2+
(E) The Red Sox win 9 consecutive World Series in this decade.
PAGE 18 of 23
POINTS:_______
+3.0 V
+1.61 V
+1.06 V
-2.92 V
-3.05 V
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12. CIRCLE ALL TRUE RESPONSES:
The Arrhenius equation, k = Ae-E/RT expresses the relationship between the reaction rate constant, k, and
the energy of activation, E. The probability that colliding molecules will react
(A)
increases with increasing energy of activation.
(B)
decreases with increasing energy of activation
(C)
depends only on the empirical constant, A.
(D)
has nothing whatsoever to do with A, it’s only a fudge factor.
(E)
Increases with increasing temperature.
(F)
Is independent of temperature
(G)
decreases with increasing temperature
(H)
Increases as the molecules get closer to Stowe
(I)
is influenced solely by the spirit of Svendt Arrhenius, who is really Maxwell’s Demon.
BONUS: Calculate the pH of 0.1 M acetic acid (pKa = 4.72)
PAGE 19 of 23
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PAGE 20 of 23
13. (This question is canonically asked of every General Chemistry student in the known Universe). Which line in the
diagram represents the activation energy for a forward reaction?
-
G
E
A
D
C
B
reaction coordinate 
(A)
A
(B)
B
(C)
C
(D) D
BONUS: Which line in the above graph represents G for the reaction? C
14.
Given that
CH4 (g) + 2O2(g)
1


2
CO2 (g) + 2 H2O(l)
The forward reaction (1) is proceeding at a certain rate at some temperature and pressure;
when the pressure is increased, we may expect for the forward reaction (1)
(A)
a greater rate of reaction and a greater yield of CO2 at equilibrium.
(B)
a greater rate of reaction and the same yield of CO2 at equilibrium.
(C)
a lesser rate of reaction and a lesser yield of CO2 at equilibrium.
(D)
a lesser rate of reaction and a greater yield of CO2 at equilibrium.
(E)
no change in rate or yield, because this is an ignis fatuus.
PAGE 20 of 23
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PAGE 21 of 23
15.
Which procedure will lower the activation energy for a particular reaction?
(A)
subdividing the reactants
(B)
increasing the reactant concentrations
(C)
increasing the temperature
(C)
adding a catalyst
18.
no catalyst present
catalyst present
A+ B
C+ D
reaction coordinate 
Which statement concerning the reaction coordinate diagram is true?
(A)
The catalyst decreases the activation energy.
(B)
The reaction is endothermic.
(C)
The addition of a catalyst slows this reaction.
(D)
A and B have lower potential energy than C and D.
PAGE 21 of 23
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PAGE 22 of 23
18.
The table presents data for the reaction:
2ATP + glucose
1
 k


2ADP + fructose 1,6 diphosphate
The temperature of the reaction is constant. The initial rate is in units of
nanomoles/uL/sec.
Experiment
1
2
2
4
5
[ATP]
0.15 nM
0.30 nM
0. 60 nM
0.15 nM
0.15 nM
[Glucose]
10 uM
10 uM
10 uM
20 uM
40 uM
rate
25.0
50.0
100.0
100.0
400.0
What is the rate law for this reaction?
(A)
rate = k1 [ATP] [glucose]
(C)
rate = k1 [ATP]2 [glucose]
(B)
rate = k1 [ATP]2 [glucose]2 (D)
rate = k1 [ATP] [glucose]2
19. The rate expression for a second order reaction is
rate = k [A]2 [B]
(A)
rate = k [A]2
(C)
(B)
rate = k [A]0 [B] (D)
rate == k [A]2 [B]2
PAGE 22 of 23
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PAGE 23 of 23
Complex II
(purple)
Co2+ + NH3 + Cl- + O2
Start here
Complex I
(orange)
THE FOLLOWING QUESTIONS REFER TO THE FREE ENERGY DIAGRAM ABOVE
23. Suppose you have starting reagents Co2+ + NH3 + Cl- + O2.
Depending on conditions, either complex I or complex II can be made.
Based on the reaction diagram above, what do you predict would be made FASTEST at low
temperature?
(A) Complex I
(B) Complex II (C) it’s too complex for human minds.
24. Which complex is more STABLE (ie G is -)?
(A) Complex I
scientists.
(B) Complex II
(C) There are no unstable complexes, only unstable
25. Which reaction tends to proceed as written?
(A) Co2+ + NH3 + Cl- + O2  Complex I.
(C) Life is complex & poorly understood.
26.
(A)
(B)
(C)
(B) Co2+ + NH3 + Cl- + O2  Complex II.
At high enough temperatures
Complex I would eventually all convert to Complex II
Complex II would eventually all convert to Complex I
The whole lab turns purple.
BONUS: Which reaction is under KINETIC control? Co2+ + NH3 + Cl- + O2 
Complex I. (B) Co2+ + NH3 + Cl- + O2  Complex II.
PAGE 23 of 23
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