1) Calculate the freezing point of a 0.05500 m aqueous solution of NaNO3. The molal
freezing-point-depression constant of water is 1.86 oC/m.
A) 0.0286
B) -0.106
C) 0.106
D) -0.0562
E) -0.205
2) How many chiral centers are there in CH3CHClCH2CH2CHBrCH3?
A) 0
B) 1
C) 2
D) 3
E) 4
3) Ka for H X is 7.5 x 10-12. What is the pH of a 0.15 M aqueous solution of Na X?
A) 7.97
B) 1.96
C) 6.00
D) 8.04
E) 12.10
4) Which one of the following is true?
A) Some spontaneous nuclear reactions are e x othermic.
B) Some spontaneous nuclear reactions are endothermic.
C) All spontaneous nuclear reactions are e x othermic.
D) There is no relationship between e x othermicity and spontaneity in nuclear
reactions.
E) All spontaneous nuclear reactions are endothermic.
5) What are the donor atoms in a porphine molecule?
A) N
B) O
C) S
D) Br
E) F
6) The mode of decay of 32P is ________.
A) alpha emission
B) beta emission
C) positron emission
D) electron capture
E) neutron capture
7) Which one of the following is not a valid expression for the rate of the reaction
below?
4NH3 + 7O2–> 4NO2 + 6H2O
A) –
B)
C)
D) –
E) All of the above are valid expressions of the reaction rate.
8) The pH of a 0.55 M aqueous solution ammonia, NH3, at 25.0 oC is 11.50. What is the
value of Kb for NH3?
A) 2.0 x 10-9
B) 1.1 x 10-9
C) 6.0 x 10-5
D) 1.8 x 10-5
E) none of the above
9) A 50.0-g sample of liquid water at 25.0 °C is mixed with 23.0 g of water at 79.0 °C.
The final temperature of the water is ________ °C.
A) 123
B) 27.3
C) 52.0
D) 231
E) 42.0
10) Which one of the following will occur as diatomic molecules in elemental form?
A) helium
B) argon
C) chlorine
D) phosphorous
E) sodium
11) A 4.369 g sample of metal is placed in a flask. Water is added to the flask and the
total volume in the flask is read to be 126.4 ml. The mass of the water, flask, and metal
is 268.5 g. If the mass of the flask is 139.3 g and the density of water is 1.000 g/mL, the
density of the solid is ________ g/cm3.
A) 0.366
B) 1.56
C) 0.641
D) 2.78
E) 3.21
12) Of the compounds below, a 0.1 M aqueous solution of ________ will have the
highest pH.
A) KCN, Ka of HCN = 4.0 x 10-10
B) NH4NO3, Kb of NH3 = 1.8 x 10-5
C) NaOAc, Ka of HOAc = 1.8 x 10-5
D) NaClO, Ka of HClO = 3.2 x 10-8
E) NaHS, Kb of HS– = 1.8 x 10-7
13) How many moles of sodium carbonate contain 1.773 x 1017 carbon atoms?
A) 5.890 x 10-7
B) 2.945 x 10-7
C) 1.473 x 10-7
D) 8.836 x 10-7
E) 9.817 x 10-8
14) Consider the following reaction at equilibrium:
2CO2 (g) 2CO (g) + O2 (g)Ho = -514 kJ
Le Ch¢telier’s principle predicts that an increase in temperature will ________.
A) increase the partial pressure of O2 (g)
B) decrease the partial pressure of CO2 (g)
C) decrease the value of the equilibrium constant
D) increase the value of the equilibrium constant
E) increase the partial pressure of CO
15) Using the table of average bond energies below, the ³H for the reaction is ________
kJ.
→
A) +276
B) -276
C) +735
D) -735
E) -116
16) Which of the following is an isoelectronic series?
A) B5-, Si4-, As3-, Te2-
B) F–, Cl–, Br–, I–
C) S, Cl, Ar, K
D) Si2-, P2-, S2-, Cl2-
E) O2-, F–, Ne, Na+