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7. Nonmetals rarely lose electrons in chemical reactions because
(A) their electron affinities are too high
. (B) their ionic radii become too small.
(C) their ionization energies are too small.
(D) their size is to small.
(E) their ionization energies are too high.
8. How many lone pairs of electrons are found in the Lewis structure of the
interhalogen compound BrCl?
(A) 6
(B) 2
(C) 7
(Dl
3
(El 4
9. Which of the following species are radicals?
(A) NO2
(B) HN02
10. What is the shape of ~
(A) T-shaped
(B) trigonal pyramidal
(C) seesaw
(C) N20
(D)
(3320
(E) HCN
0 3 ?
~ -
(D) tetrahedral
(E) trigonal plane
11. Which of the following has bond angles slightly less than 120°?
(A)
NO^-
(B) H02-
(c)
NO^-
(D) cs3'-
(E) I ~ +
12. Which of the following is paramagnetic?
(A) B2
B) N2
C) 0;-
D)
c;-
E)
B;-
13. The hybrid orbitals used by the underlined atoms in CH3CHCHcN, from left to
right, respectively, are
(A) sp3 and sp
(D) sp2 and sp2
(B) sp2 and sp
(E) sp and sp3
(C) sp2 and sp3
14. A badly tuned automobile engine can release about 50 moles of carbon dioxide per hour.
At 35"C, what volume of carbon dioxide is released in a six-hour period if the
atmospheric pressure is 740 Torr?
(A) 7.9 x lo5 L
(B) 7.8 x lo3 L (C) 1.3 x lo3 L . (D) 10 L (E) 1.3 x lo5 L
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20. What is the total motional contribution to the molar internal energy of gaseous H20 at
25"C?
(A) 6.19 kJ1mol
. (B) 7.43 kJ/mol
(C) 3.72 kJ/mol
(D) 12.4
(E) 2.48
kJ/mol
kJ/mol
21. A battery does 35 kJ of work driving an electric motor and 7 kJ of heat are released.
What is the change in internal energy of the system?
(A)-35 kJ
(B) +42 kJ
(C) -42 kJ
(D) -28 kJ
(E) +28 kJ
22. Calculate the change in entropy of a large pail of water after 200 J of energy is
reversibly transferred to the water at 20°C
(A) -0.733 JIK
(B) +0.733 J/K
(C) -0.683 JIK
(D) +0.683 J/K
(E) -200 J/K
23. Consider the following processes. (Treat all gases as ideal.)
1. The pressure of one mole of oxygen gas is allowed to double isothermally.
2. Carbon dioxide is allowed to expand isothermally to 10 times its original volume.
3. The temperature of one mole of helium is increased 25°C at constant pressure.
4. Nitrogen gas is compressed isothermally to one half its original volume.
5. A glass of water loses 100 J of energy reversibly at 30°C.
Which of these processes leads to an increase in entropy?
(A)
1 and 4
(B)
5
(C) 3 and 5
(D)
2 and 3
(E)
1 and 2
24. Which of the following is true for a spontaneous process at constant temperature?
(A) AS = q/T B) AS > q,,,/T
C) AS < q/T
D)AS > q/T
E) none of these
25. Which of the following statements is true?
(A)The molar entropy does not depend on the structure of the compound.
(B) The molar entropy of H20(1) is about the same as the molar entropy of ice.
(C) All processes that give positive changes in energy are spontaneous.
(D) If AGp 0, then the reaction is spontaneous.
(E) An isothermal process that leads to a decrease in free energy is spontaneous.
26. The phase diagram for sulfur is given below.
104 -
102 -
-s
r-
-z
.'rU
e
m
V1
w
fr
Liquid
U
'
t5
Li
-5
.-
1 -
3
10-2 -
50
2
100
1.50
Temperr~ture("C)
200
What is the critical temperature of the sulfur?
"C
(A) 96°C
(D) 200
(0) 120°C
(E) Not enough information given
(C) 151°C
to calculate.
27. Which of the following compound has the lowest freezing point?
(A) 2.0 m sodium perchlorate
(B) 1.0 m potassium phosphate
(D) 1.0 m aluminum sulfate
(E) 1.5 m magnesium phosphate
(C) 1.5 m aluminum nitrate
28. For CaC12, the absolute value of the enthalpy of hydration is larger than the lattice
enthalpy. This means that for CaC12
(A) he lattice enthalpy is negative
(B) the enthalpy of solution is exothermic.
(C) the enthalpy of solution is endothermic.
(D) the solubility increases when the temperature increases.
(E) the lattice enthalpy is positive
-
.
,
29. The osmotic pressure of 1.OO g of a polymer dissolved in benzene to give 200 mL
of solution is 1.50 kPa at 25°C. Estimate the average molar mass of the polymer.
.
(A)693 glmol
(B)1650g/mol
(C) 8260 g/mol
(D) 41 300 glmol
(E) 62000 g/mol
+
30. One new reaction is A(,)
2B(,). The equilibrium constant K of this reaction is
a function of temperature T (Kelvin) listed below:
This equation should be used between 300K and 600K.
correct description of this reaction?
(A)The free energy of the reaction is positive.
(B) High temperature will decrease the product of B.
(C) High pressure will increase the product of B.
(D)The enthalpy of the reaction is exothermic.
(E) The above are all correct.
At 500K, what is the
3 1. Consider the reaction
CUSO~(S) C U ~ ( S+)so3(g)
If Go = -14.6 kJ at 950°C for this reaction, what is G for an S03(g) pressure
of 50 bar at this temperature?
(D)2.68 kJ
(A) 25.2 kJ
(B) 54.4 kJ
(E) -54.4 kJ
(C) 16.3 kJ
32. Which of the following statements is true?
(A) When the value of Q is large, the equilibrium lies on the product side of the
equilibrium reaction.
(B) When the value of Q is small, the reaction moves towards the product side of
the equilibrium reaction.
(C) A small value of K means that the equilibrium concentrations of the reactants
are small compared to the equilibrium concentrations of the products.
(D) A large value of K means that the equilibrium concentrations of products are
large compared to the equilibrium concentrations of the reactants.
(E) The above are all correct.
33. Given: PH3(g) P ~ s ) in
, a basic solution
balanced half-reaction?
-+
-
(A) 3
(B)6
How many electrons appear in the
(Dl 9
(El 12
34. In a basic solution, Fe(OH)2 and Fe(OH)3 are solids. The former may be
oxidized by H202.
Balance this equation to get a, b ,c and d. Please calculate a+2b+3c+4d
(A) 5
(Dl 12
(B) 6
(C) 10
(El 14
35. Write the cell diagram for the reaction :
2AgCl(s) + H2(g)-+ 2Ag(s) + 2 ~ + ( a+~2Cl-(aq)
)
(A)AgCl(s) I Ag(s) I Cl-(aq)Y H+(aq) I :H2(g) I Pt(s)
(B) Pt(s) I H2(g> I ~ + ( a q )Cl'(aq)
,
I AgCl(s) I Ag(s)
(C) Pt(s) I Cl-(aq)Y H+(aq) I H2(g> I AgCl(s) I Ag(s)
(D)Ag(s) I AgCl(s) I Cl-(aq), ~ + ( a qI)
I Pt(s)
(El Pt(s) I H2(g) I ~ + ( a q )Cl-(aq)
,
I Ag(s) I AgCl(s)
36. Consider the following cell
Zn(s)
zn2+(aq,0.200 M)
1
~ + ( a q?),
H2(g, 1.OO atm)
Pt
If E = +0.66 V and EO= +0.76 V at 25OC, calculate the concentration of H+ in the
cathode cell compartment.
(D) 4 . 0 1~o - ~M
( ~ ) 9 . 2 ~ 1M
0-~
(B) 4 . 0 lo-'
~ M
(C) 8.4 x10-~WI
(E) 2.1 x
M
37. Given: A -;tP rate = k[A]. If 20% of A reacts in 5.12 min, calculate the time
required for 90% of A to react.
(A) 1.05 min
(D) 52.8 min
(E) Not enough information given
(B) 2.42 min
(C) 22.9 min
to calculate.
38. A reaction that has a very low activation energy
(A) has a rate that is very sensitive to temperature.
(B) has a rate that does not change much with temperature.
. (C) must be second order.
(D) gives a curved Arrhenius plot.
(E) must be first order.
39. Consider the reaction below
2 A + B 2 2AB
Rate = ~ [ A ] ~ [ B ]
Which of the following mechanisms is likely and consistent with the experimental
rate law?
1.
2.
3.
A + A + B 2 2AB
B2 2B
A+B
AB
B2 2B
B2 + A 2
(A) 2 and 3
2AB
K, fast
k, slow
kl, slow
k2, fast
k, slow
(B) 2
(C) 3
40. A second-order reaction has a rate constant of 1.25 M-' s-'. If the initial reactant
concentration is 1.0 M, calculate the time required for 90% reaction.
(A) 1.3 sec
(D) 17 sec
(B) 0.13 sec
(E) 0.89 sec
(C) 7.2 sec
41. The atomic radii of the Period 6 d-metals are about the same as the Period 5
d-metals. Which one provides the best explanation?
(A) the shielding effect of the d-electrons is less than that of the f-electrons.
(B) the shielding effect of the d-electrons is greater than that of the f-electrons
(C) of the poor shielding effect of the f-electrons and the higher nuclear charge.
(D) the d-electrons shield the f-electrons from the nucleus.
(E) f-electrons interact more strongly with each other than d-electrons.
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47. Which of the following undergo nitration faster than benzene?
(A) 4 and 5
(B)2,3, and 5
(C) 1 and 2
(D) 3 and 4
(E) l , 4 , a n d 5
48. The product of the reaction of 2-butene with HBr is
(A) 1-bromobutane.
(D) 2-bromo- 1-butene.
(B) 2-bromo-2-butene.
(E) . butane.
(C) 2-bromobutane
49. Consider the reaction
CH3(CH2)4CH2CH(Br)CH3 + NaOH
CH3(CH2)4CH2CH(OH)CH3
(optically pure enantiomer)
If 2-bromooctane rotates the plane of polarized light to the right while the product
rotates the plane of polarized light to the left, which of the following statements is true?
(A) This is an example of an elimination reaction.
(B) The reaction occurs by an SN2 mechanism.
(C) The reaction occurs by an SN1 mechanism.
(D) This is an example of an addition reaction.
(E) This is an example of an electrophilic substitution.
50. Which of the following polymers are condensation polymers?
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