Download MULTIPLE CHOICE

MULTIPLE CHOICE
1. At a specific temperature, the equilibrium constant for the following reaction is given.
2 SO2 (g) + O2 (g) ↔ 2 S03 (g)KC = 1.2
If 1.5 mol S0 2 , 4.0 mol 02 and 2.0 mol SO3 are introduced into a 1.00 liter flask, what
changes in concentration (if any) will be observed as the system reaches equilibrium?
a)
b)
*c)
d)
c)
[SO2 ] increases; [O2 ] increases; [S03 ] decreases
[SO2 ] increases; [O2 ] decreases; [SO3 ] decreases
[SO2 ] decreases; [O2 ] decreases; [SO3 ] increases
[SO2 ] decreases; [O2 ] increases; [SO3 ] increases
all concentrations remain the same
2 How many milliliters of bromine (density = 3.19 g/mL) are needed to react completely
with 85.0 grams of NH3 to produce ammonium bromine and nitrogen en according to the
equation below ?
3Br2 (1)+ 8NH 3 (g) → 6NH 4 Br(s) + N 2 (g)
a)
*b)
c)
d)
e)
46.9 mL
93.7 mL
249.9 mL
298.9 mL
315.4 mL
3 Under which of the following conditions does the equilibrium constant K change for the
reaction
H2 (g) + I2 (g) ↔ 2 HI(g)
a)
b)
c)
*d)
e)
changing the size of the container
introducing more I2 into the container
measuring the molar concentrations instead of pressures
changing the temperature
none of these, it is always constant
4 If 8.0 mol of the gas A is introduced in a 60.0 liter tank with 1.0 mol B at O - ° and 1.0
atm., they react according to the equation
2 A (g) + B(g) → 3 C(g) + D(g)
The temperature is held constant. What is the pressure in the flask when the reaction is
complete?
a)
b)
1.12 atm
1.49 atm
c)
d)
*e)
2.99 atm
3.36 atm
3.74 atm
5 . How many unpaired electrons are present in Fe• 2 ?
a)
b)
*c)
d)
e)
0
2
4
5
6
6 Which of the following has the rnost molecules?
a)
b)
c)
d)
*e)
1 00 L of CH4 at 0° C and 1 00 atm
1 00 L of N2 at 0° C and 1 00 atm
1 00 L of O2 at 20° C and 1 00 atm
1 00 L of CO2 at 50° C and 1 25 atm
1 00 L of CO at 0° C and 1 2S atm
7 . In which of the following reactions does a decrease in the volume of the container
increase the concentration of the products? Assume constant temperature
a)
b)
c)
d)
*e)
SO2 Cl2 (g) ↔ SO2 (g) + Cl2 (g)
C(s) + H 2 O(g) ↔ CO(g) + H2 (g)
2 S03 (g) ↔ 2 SO2 (g) + O2 (g)
I2 (g) + Cl2 (g) ↔ 2ICl(g)
2 NO + Br2 (g) ↔ 2 NOBr(g)
8. Which physical state(s ) of matter exhibit(s) the greatest change in volume with changes
in temperature or pressure?
a)
b)
c)
d)
*e)
none, they are all the same
liquids and gases change the same
solid
liquid
gas
9 . What is the pH of a 0 0144M Ca(0H)2 solution at 25° C?
a)
b)
1.54
1.84
c)
d)
*e)
10.84
12.16
12.45
10. What is the pH of a 3 18 M CH3 CO2 H solution at 25° C?
Ka=1.8 x 10-5
*a)
b)
c)
d)
e)
2.12
2.75
1.40
4.24
4.74
11. The following two-step process has equilibrium constants Kl and K2 .
Step l H2 (g) + ICl(g): ↔ HI(g) + HCl(g) K1
Step 2 HI(2) + ICl (g): ↔ HCl (g) +I2(g) K2
Overall H2 (g) + 2 ICl(g): ↔ 2 HCl(g) + I2 (g) K3
What is the expression for the equilibrium constant for the overall reaction K3 ?
*a)
b)
c)
d)
e)
K3 = K 1 K2
K3 = 1/[K1 ]2
K3 =K, 1 +K 2
K3 = (K 1 K2 )
K3 = K 2 /K1
12 . How many eleetrons can be described by the set of quantum numbers
n=3,1 =1, m~ =-l,ms=-1/2?
a)
b)
*c)
d)
e)
18
12
1
0
6
13 . Which formula represents the binary compound formed by magnesium and nitrogen?
a)
b)
c)
*d)
e)
MgN
Mg 2 N
MgN3
Mg3 N2
Mg 2 N3
14. The classification of the following reactions in order is
HCl(g) + NH, (g) → NH, Cl
2 HgO(s) → °2 (g) + 2 Hg(l)
HCl(aq) + AgNO3 (a → AgCl(s) + HNO3 (aq)
a)
b)
e)
*d)
e)
acid-base, precipitation, and redox respectively.
precipitation, acid-base, and redox respectively.
redox , precipitation, acid-base respectively.
acid-base, redox andprecipitation respectively.
redox, acid-base, precipitation respectively.
15. What is the empirical formula of a compound which is 64.80%carbon, 6.35%
hydrogen and 28.83% sulfur?
a)
b)
e)
*d)
e)
C5 H6 S
C6 H7 S2
C5 H7 S
C6 H7 S
C5 H5 S2
16 Which of the following elements is most likely to form compounds involving an
expanded valence shell of electrons ?
a)
b)
e)
d)
*e)
Li
N
F
Ne
S
17 . Based on the VSEPR Theory, what is the molecular shape of CIF3 ?
a)
*b)
e)
d)
e)
triangular planar
T-shaped
linear
tetrahedral
square planar
18 . Which one of the following substances would exhibit dipole-pole intermolecular
forces?
a)
b)
c)
*d)
CC14
C12
N2
NCl3
e)
CH4
19 . The chemical properties of sulfur would be most similar to
a)
b)
c)
*d)
e)
P
Cl
Ar
Se
Ge
20 . Which of the following atoms has the smallest first ionization energy?
a)
b)
c)
d)
*e)
Al
P
Sr
Ga
Rb
21. If an atom uses an sp3 d hybrid orbital set, how many unhybridized orbitals in the
same energy level remain on the atom?
a)
b)
c)
*d) 4
e)
0 (zero)
1
3
5
22 . Which of the following molecules would exhibit hydrogen bonding in the liquid state?
a)
b)
*c)
d)
e)
CH4
H2
NH 3
O2
H2 S
23 . If you dissolve 8.14 grams of calcium chloride, CaC12 , in enough water to make
125.0 mL of solution, what is the molarity of the solution?
a)
b)
*c)
d)
e)
0.00916 M
5.84 x 10 -4 M
0.586 M
1.71 M
2.24 M
24 . What is the density of a metal if a 5.4 gram sample has a volume of 1.96 cm3 ?
a)
b)
*c)
d)
e)
0.51l g/cm3
0.127 g/cm3
7.86 g/cm3
30.2 g/cm3
33.1 g/cm3
25 . Two ions which have a similar shape are
a)
b)
c)
d)
*e)
OH- and SO3 2SO3 2 - and C03 2PO3 3- and C O3 2PO3 3- - and NO3 SO3 2- and PO3 2--
26. Specific heat capacity is
*a)
amount of heat energy needed to change 1.00 g of substance by 1.00 K
b)
amount of heat energy needed to change 1.00 mol of substance by 1.00 K
c)
amount of energy required to melt 1.00 g of substance.
d)
amount of substance that is heated by 1.00 K
e)
the number of Kelvins that 1.00 g of substance is raised by heating it for 1.00
minute.
27 . How many moles are in 15.0 grams of potassium carbonate?
a)
b)
c)
*d)
e)
6.53 x 10 2 2 mol
2.07 x 10 2 3 mol
0.151 mol
0.109 mol
9.20 mol
28. The boiling points of NH3 , PH 3 , AsH 3 , and SbH3 follow a periodic trend except for
*a)
b)
c)
d)
e)
NH 3 which has an unexpectedly high boiling point.
NH 3 which has an unexpectedly low boiling point.
SbH 3 which has an unexpectedly high boiling point.
SbH 3 which has an unexpectedly low boiling point.
AsH3 which has an unexpectedly high boiling point.
29. The quantum number l represents the
a)
b)
*c)
d)
e)
number of valence electrons
number of orbitals
shape of the orbital
orientation of the orbital
momentum of the electron
30 . What is the frequency of yellow light having a wave length of 562 nanometers?
*a)
b)
e)
d)
e)
5.33 x 10 1 4 g -1
5.33 x 10 5 g -11 .87 x 10 -6h -1
l.87 x 10 - 1 5 g -1
1.87 x 10 - 2 7 g -1
31. Calculate the wavelength of light emitted when an electron changes from a state of
principal quantum number 3 (n=3) to a state of principal quantum number 1 (n=l ) in the H
atom.
a)
b)
*c)
d)
e)
3.44 x10 -9m
7.24 x 10 -4'm
1.02 x 10 -7m
1 57 x 10-5m
2.75 x 10 -3 7 m
32 . Which of the following particles would be predicted to be paramagnetic?
*a)
b)
e)
d)
e)
Na
Ne
Mg
O-2F-
33 . What is the relationship between Kp and Kc for the following reaction?
CH3 OH(g) ↔ CO(g) + 2 H2 (g)
a)
b)
c)
d)
*e)
Kp = K c
Kp =K c (RT)-1
Kp = K c (RT)
Kp = K c (RT)-2
Kp = K c (RT)2
34 . What is the approximate H-C-C bond angle in H2 C=CH 2 ?
a)
*b)
e)
d)
e)
180°
120°
109.5°
90°
60°
35. A chemist knows the empirical formula of a new compound but not the molecular
formula What must be determined experimentally so that the molecular formula can be
determined?
a)
b)
e)
d)
*e)
density
viscosity
% composition
melting point
molar mass
36. The empirical formula for a compound is C2 H3 . Which of the following could be a
molecular formula for the
compound?
a)
b)
*c)
d)
e)
CH3
C3 H4
C1 2 H1 8
C3 0 H2 0
C4 H9
37. Which of the following would have an enthalpy of formation value (∆Hf ) of zero?
a)
b)
c)
*d)
e)
H2 O(g)
O(g)
H2 0(1)
O2 (g)
H(g)
38 . What pressure (in atmospheres) is exerted by 82.5 grams of CH4 in a 75.0 liter
container at 35.0°C?
a)
b)
*c)
d)
e)
0.197 atm
0.339 atm
1.73 atm
2.57 atm
27.8 atm
39 . Calculate the standard enthalpy of formation of sulfuric acid from the following
information.
Cu(s) + 2H 2 SO4 (aq) → CuSO4 (aq) + 2H2 O(l) + SO2(aq)
∆H° rxn = 178kJ; ∆Hf° (CuSO4 ) = -771kJ/mol;
∆Hf° (H2 O) = -286 kJ/mol; ∆Hf° (SO2 ) = -297 kJ/mol
a)
b)
c)
*d)
e)
-1532 kJ/mol
-766 kJ/mol
-1818 kJ/mol
-909 kJ/mol
1640 kJ/mol
40. Non-ideal behavior for a gas is most likely to be observed under conditions of
a)
*b)
c)
d)
e)
standard temperature and pressure
low temperature and high pressure
low temperature and low pressure
high temperature and high pressure
high temperature and low pressure
41 Which of the following would probably have the highest boiling point?
a)
b)
c)
d)
*e)
Ar
He
Kr
Ne
Xe
42. Which of the following compounds exhibits ionic bonding?
a)
*b)
c)
d)
e)
CCl
MgC12
Cl2
PC13
OF2
43 . When a pure solid substance was heated a student obtained another solid and a gas,
each of which was a pure substance. From this information which of the following
statements is ALWAYS a correct conclusion?
*a)
b)
c)
d)
e)
The original solid is not an element.
Both products are elements.
The original solid is a compound and the gas is an element.
The original solid is an element and the gas is a compound.
Both products are compounds.
44. How many neutrons are in
a)
b)
*c)
d)
e)
7
3
9
Se?
4
113
34
45
79
11
45. Which equation below best represents the balanced net ionic equation for the reaction
of a solution of barium nitrate with a solution of potassium carbonate? (Note that barium
carbonate is insoluble.)
*a)
b)
c)
d)
e)
Ba2 + (aq) + CO3 2- (aq) → BaCO3 (s)
K + (aq) + NO3 - (aq) → KNO3 (s)
Ba2+ (aq) + NO3 -(aq) K2 CO3 (aq) → + Ba2 + (s)
Ba(NO3 )2 (aq) + K+ (aq) → KNO3 (s) + Ba2 + (aq)
Ba(NO3 )2 (aq) + CO2 3- (aq) → BaCO3 (s) + 2 N 2 (g) + 3 O2 (g)
46 . If 35.0 grams of bromine and 20.0 grams of ammonia are allowed to react according
to the equation below what is the maximum number of grams of N2 that can be produced?
3 Br2 (1) + 8 NH 3 (g) → 6 NH 4 Br(s) + N 2 (g)
*a)
b)
c)
d)
e)
2.05 g
5.15 g
6.13 g
41 .2 g
60.5 g
47. A sample of 20.0 grams of calcium contains
*a)
b)
c)
d)
e)
0.500
1.000
2.00
3.01 x l0 2 3
1.20 x 2 4
48. At equilibrium. what is equal?
? moles .
a)
b)
*c)
d)
e)
concentrations of products and reactants
rate constants for the forward and reverse reactions
the rate of the forward and reverse reaction
the partial pressures of the reactants and products
the reaction quotient and the rate of both reactions
49 . Which of the following diatomic molecules has the greatest bond strength?
a)
b)
*c)
d)
e)
F2
O2
N2
HF
HC1
50 When 0.25 mol of gold is cooled from 500° C to 20.0° C what is the energy transferred?
The specific heat of gold is 0.128 J/g K
a)
b)
c)
*d)
e)
+0.96 J
+189 J
+756 J
-189 J
-756 J
51 When glucose undergoes complete combustion the products are carbon dioxide and
water.
______C6 H1 2 O6 +_____ O2 → ______CO2 +
______ H2 O
Which of the following is the most correct set of stoichiometric coefficients to balance this
equation?
*a)
b)
e)
d)
e)
1, 9, 6, 6
l, 6, 6, 6
2, 12, 6, 12
2, 12, 12, 12
l, 9, 12, 12
52 Which of tbe following pairs have the same number of electrons ?
a)
*b)
e)
d)
e)
Fe2+ and Fe3+
Ca2+ and K+
K+ and Na+
O2 - and O2H+ and H-