Chemistry 1A
Practice Test II
1. The melting point of nitrogen is 63 K. This
temperature corresponds to
[A] 63°C.
[B] –63°C.
[C] –210°C.
[D] 483°C.
[E] –336°C.
2. A given mass of gas occupies a volume of
4.00 L at 60°C and 550 mmHg. Which of the
following mathematical expressions will yield
its pressure at 3.00 L and 30°C?
[A] 550 
4.00 30

3.00 60
[B] 550 
3.00 30

4.00 60
[C] 550 
3.00 333

4.00 303
[D] 550 
4.00 303

3.00 333
[E] 550 
3.00 303

4.00 333
3. How many moles of gas are in a gas sample
occupying 0.250 L at 215 mmHg and 25°C?
[A] 0.00217
[B] 0.00289
[C] 0.0345
[D] 0.416
[E] 1.27
4. At standard conditions, it was found that
1.17 L of a gas weighed 5.45 g. The gas is
[A] NH3.
[B] HNF2.
[C] N2F4.
[D] NH3.
[E] NO2.
5. What volume of nitrous oxide, N2O, has the
same number of ATOMS as 10.0 L of neon at
the same temperature and pressure?
[A] 1.67 L
[B] 2.50 L
[C] 3.33 L
[D] 7.50 L
[E] 10.0 L
6. Which of the following statements
concerning equal volumes of the gases
nitrogen(I) oxide, N2O, and propane, C3H8, at
the same temperature and pressure, is (are)
true?
1. They have the same number of atoms.
2. They have the same number of molecules.
3. They have the same density.
[A] 1 only
[B] 2 only
[C] 1 and 2 only
[D] 2 and 3 only
[E] 1, 2, and 3
7. If  is the density of a gas, M its relative
molecular mass, R the gas constant, T the
temperature, and P its pressure, which of the
following expressions represents the density of
a gas?
PM
RT
RTM
[D]
P
[A]
RM
PT
RT
[E]
PM
[B]
[C]
RMP
T
1
8. A sample of hydrogen was collected by
water displacement at 23.0°C and an
atmospheric pressure of 735 mmHg. Its
volume is 568 mL. After water vapor is
removed, what volume would the hydrogen
occupy at the same conditions of pressure and
temperature? (The vapor pressure of water at
23.0°C is 21 mmHg.)
[A] 509 mL
11. All the following are postulates of the
kinetic-molecular theory of gases except
[A] the collisions between molecules are
elastic.
[B] the gas molecules are in constant motion.
[C] at a constant temperature, each molecule
has the same kinetic energy.
[B] 539 mL
[C] 552 mL
[D] the volumes of the molecules are
negligible compared with the volume of the
container.
[D] 568 mL
[E] the gas molecules are in rapid motion.
[E] 585 mL
9. Equal volumes (1.0 L) of ozone, O3, and
methanethiol, CH3SH, under the same
conditions have equal
1. numbers of molecules.
2. numbers of atoms.
3. masses.
[A] 1 only
[B] 2 only
[C] 3 only
12. Which of the following statements is
LEAST likely to be true of a sample of
nitrogen gas?
[A] Molecules of gaseous nitrogen are in
constant random motion.
[B] The pressure exerted by gaseous nitrogen
is due to collisions of the molecules with the
walls of the container.
[C] The average kinetic energy of the gaseous
nitrogen is proportional to the absolute
temperature of the gas.
[D] 1 and 2 only
[E] 1 and 3 only
10. Real gases deviate from ideal behavior
because of the attractive forces between the
gas molecules and
[D] Collisions between the gaseous molecules
are elastic.
[E] The volume of the sample would be zero at
–273°C.
[A] ionization energies.
[B] molecular vibrations.
[C] pressures within the chemical bonds.
[D] the molecules all having different
velocities.
[E] the actual volume of the molecules.
2
13. The molecular weight of an unknown gas
was measured by an effusion experiment. It
was found that it took 64 seconds for the gas to
effuse, whereas nitrogen required 48 seconds.
The molecular mass of the gas is
[A] 16 g/mol.
[B] 24 g/mol.
[C] 30 g/mol.
[D] 40 g/mol.
[E] 50 g/mol.
14. From a consideration of the van der Waals
constants for water and sulfur dioxide,
a(atm• L2 / mol2 )
b(L / mol)
H2O
5.54
SO2
6.87
we can conclude that
0.0305
0.0568
[A] H2O molecules are smaller and less
attracted to each other than SO2 molecules.
[B] H2O molecules are smaller and more
attracted to each other than SO2 molecules.
[C] H2O molecules are larger and more
attracted to each other than SO2 molecules.
[D] H2O molecules are larger and less
attracted to each other than SO2 molecules.
[E] None of these conclusions is correct.
15. If U = –65 kJ for a certain process, that
process
[A] occurs rapidly.
[B] is exothermic.
[C] is endothermic.
[D] cannot occur.
[E] requires a catalyst.
16. The sign of H for the process CO2(s)
CO2(g) is


[A] positive, and the process is endothermic.
[B] negative, and the process is endothermic.
[C] positive, and the process is exothermic.
[D] negative, and the process is exothermic.
[E] impossible to predict with confidence
because H of for CO2(s) and H of for CO2(g)
are not given.
17. Consider the following specific heats of
metals.
Metal
Specific Heat
copper
0.385 J (g   C)
magnesium 1.02 J (g   C)
mercury
silver
0.138 J (g   C)
0.237 J (g   C)
lead
0.129 J (g   C)
If the same amount of heat is added to 25.0 g
of each of the metals, which are all at the same
temperature, which metal will have the highest
temperature?
[A] copper
[B] magnesium
[C] mercury
[D] silver
[E] lead
18. The sign of H for the process NaCl(s)
NaCl(l) is


[A] negative, and the process is endothermic.
[B] positive, and the process is exothermic.
[C] positive, and the process is endothermic.
[D] negative, and the process is exothermic.
[E] impossible to predict because H of for
NaCl(s) and H of for NaCl(l) are not given.
3
19. Which of the following would be needed
to determine the energy of combustion of
ethanol in a bomb calorimeter?
1. temperature increase
2. amount of ethanol
3. heat capacity of calorimeter
[A] 1 only
[B] 1 and 2 only
[C] 1 and 3 only
[D] 2 and 3 only
[E] 1, 2, and 3
20. When 0.0500 mol of HCl is reacted with
0.0500 mol of NaOH in 50.0 mL of water, the
temperature of the water increases by 13.7°C.
Calculate the heat of the reaction for the
following thermochemical equation:
HCl(aq) + NaOH(aq) 
NaCl(aq) +

H2O(l)
Assume that the heat capacity of the system is
209.2 J/°C.
[A] –57,300 J/mol
[B] –2870 J/mol
[C] + 2870 J/mol
[D] +57,300 J/mol
[E] +115,000 J/mol
21. All the following are state functions
EXCEPT
[A] w.
[B] H.
[C] U.
[D] P.
[E] T.
22. What is the quantity of heat evolved when
200. g H2O(l) is formed from the combustion
of H2(g) and O2(g)?
1
H2(g) +
O2(g) 
H2O(l)
H° = –

2
285.8 kJ
[A] 285.8 kJ
[B] 1590 kJ
[C] 3170 kJ
[D] 4360 kJ
[E] 57200 kJ
23. Calculate the change in enthalpy when
52.0 g of Cr at 25°C and 1 atm pressure is
oxidized. (H of for Cr2O3(s) is –1140
kJ/mol.)
4Cr(s) + 3O2(g) 
2Cr2O3(s)

[A] –1140 kJ
[B] +1140 kJ
[C] –570 kJ
[D] +570 kJ
[E] –285 kJ
24. Which substance has a heat of formation
equal to zero at 25°C and 1 atm?
[A] C2H6(g)
[B] C2H6(l)
[C] Br2(s)
[D] Br2(l)
[E] Br2(g)
25. All the following statements are true for an
exothermic reaction EXCEPT
[A] the temperature of the reaction system
increases.
[B] the temperature of the surroundings
increases.
[C] heat passes from the reaction system to the
surroundings.
[D] the products have a higher heat content
than the reactants.
[E] the enthalpy change for the reaction is
negative.
4
26. The equation for the standard enthalpy of
formation of potassium bromate, KBrO3,
corresponds to which reaction?
[A] K(s) +
KBrO3(s)
1
2
Br2(g) +
3
2
O2(g) 

[B] K(g) +
KBrO3(s)
1
2
Br2(g) +
3
2
O2(g) 

[C] K(s) +
KBrO3(s)
1
2
Br2(l) +
3
2
29. Using the following data, determine the
heat of reaction for the combustion of 1 mol of
ethylene, C2H4.
C2H4(g) + 3O2(g) 
2CO2(g) + 2H2O(l)


Compound H f (kJ / mol)
C2 H 4 ( g )
+ 52.3
CO 2 ( g )
H 2 O(l )
O2(g) 

[A] +731.4 kJ
[B] +1411.1 kJ
[C] –1411.1 kJ
[D] –1306.5 kJ
[E] +1306.5 kJ
[D] K(g) + Br(g) + 3O(g) 
KBrO3(s)

[E] K(s) + Br(g) + 3O(g) 
KBrO3(s)

27. Given the following data,
S( s) + O 2 ( g )
S( s) + O 2 ( g ) 
 SO 2 ( g )  618
find the heat required for the reaction
converting solid sulfur to gaseous sulfur at 298
K and 1 atm pressure.
[A] –1013 kJ/mol
[B] +618 kJ/mol
[C] –618 kJ/mol
[D] –223 kJ/mol
[E] +223 kJ/mol
30. Given the following data at 25°C and 1.00
atm pressure:
H ( kJ mol)

 SO 2 ( g )  395
 393.5
 285.9

Pb( s) + PbO 2 ( s) + 2H 2SO 4 (l ) 
 2PbSO 4 ( s) + 2H 2 O(l )
SO 3 ( g ) + H 2 O(l ) 
 H 2SO 4 (l )
evaluate H° for the reaction below at 25°C.
Pb(s) + PbO2(s) + 2SO3(g) 
2PbSO4(s)

[A] –3.77  103 kJ
[B] 3.77  103 kJ
[C] –639 kJ
[D] –521 kJ
[E] –769 kJ
31. All of the following statements are TRUE
EXCEPT
28. Given the following data:
3
N 2 ( g)  O2 ( g) 
 N 2 O 3 ( s) H  83.7 kJ[A] the value of q is positive when heat flows
2
N 2 ( g)  O2 ( g)

 2NO(g) H  180.4 into
kJ a system from the surroundings.
[B]
heat flows from a system into the
1
N 2 ( g)  O2 ( g) 
 NO 2 ( g ) H  33.2 kJsurroundings in an endothermic process.
2
[C] enthalpy is a state property.
what is H for the reaction
[D] energy is a state property.
N2O3(g) 
 NO(g) + NO2(g)
[E] the value of q is positive in an endothermic
process.
[A] –207.1 kJ [B] –39.7 kJ [C] 24.3 kJ
[D] 39.7 kJ
[E] 207.1 kJ
5
32. Rank the following regions of the
electromagnetic spectrum in order of
decreasing energy.
X-rays, Microwaves, Infrared, Ultraviolet
[A] x-rays, microwaves, infrared, ultraviolet
[B] microwaves, ultraviolet, infrared, x-rays
[C] microwaves, infrared, ultraviolet, x-rays
[D] infrared, microwaves, ultraviolet, x-rays
[E] x-rays, ultraviolet, infrared, microwaves
33. What is the wavelength of light associated
with the radiation
of 7.26  1019 J / photon?
ch  6.63  10
 34
h
J  s.
1. 3 3
2. 4 3
3. 3 2
34. What is the wavelength of light emitted
when the hydrogen atom undergoes a
transition from level n = 5 to level n = 2?
R H  2.180  1018 J
[A] 663 nm
[B] 833 nm
[C] 546 nm
[D] 521 nm
[E] 434 nm
1
0
1
1/ 2
1/ 2
1/ 2
[A] 1 only
[B] 2 only
[C] 3 only
[D] 1 and 2 only
[E] 2 and 3 only
38. What orbital has the quantum numbers n =
4, l = 3, m1 = –1?
[A] s [B] p [C] d D] f
35. Einstein’s work on the photoelectric effect
made extensive use of the equation
[E] E =  R H
[A] his statement that an electron can exist in
an atom only in discrete energy levels.
[B] his statement that no electron can have
identical values for all four quantum numbers.
[C] his proposal that particles of matter should
be associated with wavelike behavior.
[D] his statement that elements show periodic
repetition of properties.
[E] his statement that electrons occupy all the
orbitals of a given sublevel singly before
pairing begins.
37. Which of the following combinations of
quantum numbers are permissible?
n l ml
ms
[A] 137 nm
[B] 231 nm
[C] 274 nm
[D] 548 nm
[E] 684 nm
[A] E = mc2.
[B]  = c/
R
[C] E =  2H .
n
[D] E = h.
36. The contribution for which de Broglie is
remembered in modern science is
F
1
1I
 J
G
Hn n K.
2
2
E] g
39. Which one of the orbital occupancy
designations shown below does NOT make
sense?
[A] 2s1
[B] 3d10
[C] 4p7
[D] 4f7
[E] 2p6
2
1
6
40. The maximum number of electrons in a 4d
subshell is
45. Which of the following electron
configurations represents an excited state?
[A] 1.1[B] 3. [C] 5. [D] 8. [E] 10.
[A] He: 1s2
[B] Ne: 1s2 2s2 2p6
[C] Na: 1s2 2s2 2p6 3s2 3p2 4s1
[D] P: 1s2 2s2 2p6 3s2 3p2 4s1
[E] N: 1s2 2s2 2p3
41. The angular momentum quantum number
of the first two valence electrons in an atom of
lead is
[A] 1. [B] 2. [C] 3. [D] 4. E] 5.
42. The maximum number of 5d electrons is
[A] 10. [B] 7. [C] 5. [D] 4. [E] 3.
43. An element that has the same valence
electron configuration as tin is
[A] antimony.
[B] tellurium.
[C] indium.
[D] selenium.
[E] germanium.
44. Which of the following orbital diagrams is
IMPOSSIBLE according to the Pauli
exclusion principle?
46. The elements that are filling the 5f subshell
is (are) called
1. lanthanides.
2. inner transition elements.
3. actinides.
[A] 1 only
[B] 2 only
[C] 3 only
[D] 1 and 2 only
[E] 2 and 3 only
47. The formula that one would expect for
calcium nitride is
[A] Ca3N2.
[B] Ca2N3.
[C] CaNO2.
[D] Ca(NO2)2.
[E] Ca(NO3)2.
48. Which of the following atoms has the
LARGEST atomic radius?
[A] Option 1
[B] Option 2
[C] Option 3
[D] Option 4
[E] Option 5
[A] Sr
[B] Mg
[C] P
[D] I
[E] Kr
7
49. Which of the following atoms designated
by electronic configurations has the highest
ionization energy?
[A] [Ne] 3s2 3p2
[B] [Ne] 3s2 3p3
[C] [Ar] 3d10 4s2 4p3
[D] [Kr] 4d10 5s2 5p3
[E] [Xe] 4f14 5d10 6s2 6p3
50. Which one of the following elements
would be expected to have the SMALLEST
atomic radius?
53. Which of the following equations
represents the first ionization energy of
calcium?
[A] Ca(s) 
 Ca+(s) + e[B] Ca(s) + e- 
 Ca-(s)
[C] Ca(g) 
 Ca+(g) + e[D] Ca(s) 
 Ca+(g) + e[E] Ca(g) 
 Ca2+(g) + 2e-
[A] Li
[B] Cs
[C] F
[D] Br
[E] I
51. Which of the following atoms has the most
negative electron affinity?
[A] Na
[B] Cl
[C] Br
[D] S
[E] As
52. When arranged in order of increasing
atomic number, the elements exhibit
periodicity for all the following properties
EXCEPT
[A] ionization energy.
[B] atomic radii.
[C] electron configurations.
[D] electron affinity.
[E] atomic masses.
8
ANSWERS
[1] [C]
[2] [D]
[3] [B]
[4] [C]
[5] [C]
[6] [B]
[7] [A]
[8] [C]
[9] [E]
[10] [E]
[11] [C]
[12] [E]
[13] [E]
[14] [A]
[15] [B]
[16] [A]
[17] [E]
[18] [C]
[19] [E]
[20] [A]
[21] [A]
[22] [C]
[23] [C]
[24] [D]
[25] [D]
[26] [C]
[27] [E]
[28] [D]
[29] [C]
[30] [E]
[31] [B]
[32] [E]
[33] [C]
[34] [E]
[35] [D]
[36] [C]
[37] [E]
[38] [D]
[39] [C]
[40] [E]
[41] [A]
[42] [A]
[43] [E]
[44] [B]
[45] [D]
[46] [E]
[47] [A]
[48] [A]
[49] [B]
[50] [C]
[51] [B]
[52] [E]
[53] [C]
9