1) Consider the following equilibrium.
2 SO2 (g) + O2 (g) 2 SO3 (g)
The equilibrium cannot be established when ________ is/are placed in a 1.0-L
container.
A) 0.25 mol SO2 (g) and 0.25 mol O2 (g)
B) 0.75 mol SO2 (g)
C) 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g)
D) 0.50 mol O2 (g) and 0.50 mol SO3 (g)
E) 1.0 mol SO3 (g)
2) A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of
gas. If the partial pressure of Ne is 2.75 atm, how many moles of Ar are in the mixture?
A) 11.0
B) 5.00
C) 6.75
D) 9.25
E) 12.0
3) What volume (mL) of 7.48 10-2 M perchloric acid can be neutralized with 115 mL of
0.244 M sodium hydroxide?
A) 125
B) 8.60
C) 188
D) 750
E) 375
4) The principal quantum number of the first d subshell is ________.
A) 1
B) 2
C) 3
D) 4
E) 0
5) The concentration of sodium sulfate solution is 18.6% by mass. There are ________
g of sodium sulfate present in a 236.5 g sample of this solution.
A) 44.0
B) 4400
C) 0.000786
D) 7.86
E) 1270
6) According to kinetic-molecular theory, in which of the following gases will the
root-mean-square speed of the molecules be the highest at 200 °C?
A) HCl
B) Cl2
C) H2O
D) SF6
E) None. The molecules of all gases have the same root-mean-square speed at any
given temperature.
7) The quantity ________ m is the same as 4 km.
A) 4000
B) 400
C) 0.004
D) 0.04
E) 40
8) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si
and Ar?
A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na
9) The tertiary structure of proteins is maintained by ________ bonds.
A) hydrogen
B) dipole-dipole
C) ion-dipole
D) covalent
E) all of the above
10) Automotive air bags inflate when sodium azide decomposes explosively to its
constituent elements:
2NaN3 (s) → 2Na (s) + 3N2 (g)
How many grams of sodium azide are required to produce 28.0 g of nitrogen?
A) 1.50
B) 0.666
C) 65.0
D) 43.3
E) 97.5
11) The bond order of a homonuclear diatomic molecule can be decreased by
________.
A) removing electrons from a bonding MO or adding electrons to an antibonding MO
B) adding electrons to a bonding MO or removing electrons from an antibonding MO
C) adding electrons to any MO
D) removing electrons from any MO
E) The bond order of a homonuclear diatomic molecule cannot be decreased by any
means.
12) What order process is radioactive decay?
A) zeroth
B) first
C) second
D) third
E) fourth
13) An atom of the most common isotope of gold, Au, has ________ protons,
________ neutrons, and ________ electrons.
A) 197, 79, 118
B) 118, 79, 39
C) 79, 197, 197
D) 79, 118, 118
E) 79, 118, 79
14) A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr.
The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr,
respectively. The partial pressure of neon in the vessel was ________ torr.
A) 42.4
B) 521
C) 19.4
D) 239
E) 760
15) Complete the following: P4O10 + 6H2O →
16) A spectrum containing radiation of specific wavelengths is called a(n) ________.
17) Explain why silicon does not form any allotropes with structures analogous to that
of graphite or buckminsterfullerenes, even though it is in the same group as carbon.
18) Given the electronegativities below, which covalent single bond is most polar?
19) The first nuclear transmutation resulted in the conversion of nitrogen-14 to
________.
20) The number obtained by substituting starting reactant and product concentrations
into an equilibrium-constant expression is known as the ________.
21) D2O is known as ________.
22) Complete and balance the following reaction, given that elemental rubidium reacts
with elemental sulfur to form Rb2S (s).
Na (s) + S (s) → ________
23) Explain why hydrofluoric acid etches glass.
24) The temperature and pressure specified by STP are ________ °C and ________
atm.