R = 0.08206 L.atm/mol.K         R = 8.314 J/mol.K   
1 atm = 760 Torr            1 atm = 101.325 kPa
PV = nRT      Pi = XiP      Xi = ni/n         q = CΔT
M = m/n      d = m/V      d = MP/RT         q = mcΔT
urms = (3RT/M)1/2             teff(A)/teff(B) = (MA/MB)1/2   
ΔH° = Σ nΔHf°(products) - Σ nΔHf°(reactants)



1.
How many moles of H+(aq) ions are present in 750 mL of 0.65 M hydrochloric acid?
A.
1.2 mol
B.
0.98 mol
C.
0.87 mo1
D.
0.65 mol
E.
0.49 mol


2.
In the following reaction, what ions, if any, are spectator ions?
Pb(NO3)2(aq)    +    2NaCl(aq)    →    PbCl2(s)    +    2NaNO3(aq)
A.
Pb2+(aq), Cl-(aq)
B.
Na+(aq), NO3-(aq)
C.
Pb2+(aq), NO3-(aq)
D.
Na+(aq), Cl-(aq)
E.
There are no spectator ions


3.
Select the net ionic equation for the reaction between lithium hydroxide and hydrobromic acid.
LiOH(aq)   +    HBr(aq)    →    H2O(l)    +    LiBr(aq)
A.
LiOH(aq)    →    Li+(aq)    +    OH-(aq)
B.
HBr(aq)    →    H+(aq)    +    Br-(aq)
C.
H+(aq)    +    OH-(aq)    →    H2O(l)
D.
Li+(aq)    +    Br-(aq)    →    LiBr(aq)
E.
Li+(aq)    +    OH-(aq)   +    H+(aq)    +    Br-(aq)    →    H2O(l)    +    LiBr(aq)


4.
A 0.00100 mol sample of Ca(OH)2 requires 25.00 mL of aqueous HCl for neutralization according to the reaction below. What is the concentration of the HCl?
Equation: Ca(OH)2(s)    +    2HCl(aq) →    CaCl2(aq)    +    H2O(l)
A.
0.0200 M
B.
0.0400 M
C.
0.0800 M
D.
4.00 × 10-5 M
E.
0.100 M


5.
Calculate the oxidation number of the chlorine in perchloric acid, HClO4, a strong oxidizing agent.
A.
-1
B.
+4
C.
+5
D.
+7
E.
none of the above is the correct oxidation number


6.
Identify the oxidizing agent in the following redox reaction.
Hg2+(aq)    +    Cu(s)    →    Cu2+(aq)    +    Hg(l)
A.
Hg2+(aq)
B.
Cu(s)
C.
Cu(s) and Hg(s)
D.
Hg(l)
E.
Cu(s) and Cu2+(aq)


7.
Which one of the following is not a redox reaction?
A.
2H2(g)    +    O2(g)    →   2H2O(l)
B.
Zn(s)    +    H2SO4(aq)     →   ZnSO4(aq)    +    H2(g)
C.
H2O(l)    +    NH3(g)    →   NH4+(aq)   +   OH-(aq)
D.
6FeSO4(aq)     +    K2Cr2O7(aq)      +    7H2SO4(aq)    →
Cr2(SO4)3(aq)     +    3Fe2(SO4)3(aq)     +    K2SO4(aq)     +    7H2O(l)
E.
Cl2(g)    +    2KBr(aq)    →    Br2(l)    +    2KCl(aq)


8.
Select the classification for the following reaction.
2Na(s)    +    2H2O(l)    →    2NaOH(aq)    +    H2(g)
A.
precipitation
B.
acid-base
C.
redox
D.
combination
E.
none of the above


9.
The compound P4O10 is used in refining sugar. Select the classification for the reaction in which it is synthesized.
P4(s)    +    5O2(g)    →    P4O10(s)
A.
combination
B.
decomposition
C.
displacement
D.
acid-base
E.
precipitation


10.
The pressure of sulfur dioxide in a container is 159 kPa. What is this pressure in atmospheres?
A.
0.209 atm
B.
0.637 atm
C.
1.57 atm
D.
21.2 atm
E.
15900 atm


11.
Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its absolute temperature, other factors remaining constant?
A.
a
B.
b
C.
c
D.
d
E.
e


12.
A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?
A.
22.3 L
B.
31.2 L
C.
44.9 L
D.
112 L
E.
380 L


13.
Assuming ideal behavior, what is the density of argon gas at STP, in g/L?
A.
0.0176 g/L
B.
0.0250 g/L
C.
0.0561 g/L
D.
1.78 g/L
E.
181. g/L


14.
A 250.0-mL sample of ammonia, NH3(g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia is in the container?
A.
0.0787 g
B.
0.180 g
C.
8.04 g
D.
17.0 g
E.
59.8 g


15.
A gas mixture, with a total pressure of 300 torr, consists of equal masses (80 g each) of Ne (atomic weight 20) and Ar (atomic weight 40). What is the partial pressure of Ar, in torr?
A.
75 torr
B.
100 torr
C.
150 torr
D.
200 torr
E.
250 torr


16.
A sample of 0.100 mol magnesium metal and an excess of aqueous hydrochloric acid are combined and react to completion. How many liters of hydrogen gas, measured at STP, are produced?
Mg(s)    +    2HCl(aq)    →    MgCl2(aq)    +    H2(g)
A.
2.24 L of H2
B.
4.48 L of H2
C.
5.60 L of H2
D.
11.2 L of H2
E.
22.4 L of H2


17.
Which of the following gases will be the slowest to diffuse through a room?
A.
methane, CH4
B.
hydrogen sulfide, H2S
C.
carbon dioxide, CO2
D.
water, H2O
E.
neon, Ne


18.
Select the gas with the highest average kinetic energy per mole at 298 K.
A.
O2
B.
CO2
C.
H2O
D.
H2
E.
All have the same average kinetic energy.


19.
A system receives 575 J of heat and delivers 425 J of work. Calculate the change in the internal energy, ΔE, of the system.
A.
-150 J
B.
150 J
C.
-l000 J
D.
1000 J
E.
575 J


20.
Which of the following is not a state function?
A.
internal energy
B.
volume
C.
work
D.
pressure
E.
enthalpy


21.
A 36.0 g piece of copper metal is initially at 100.0°C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0°C. After stirring, the final temperature of both copper and water is 25.0°C. Assuming no heat losses, what is the specific heat capacity of copper? (The specific heat capacity of water is 4.18 J/g·K)
A.
0.279 J/g·K
B.
0.291 J/g·K
C.
0.301 J/g·K
D.
0.387 J/g·K
E.
0.456 J/g·K


22.
Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by the ancient Romans as mortar in stone structures. The reaction for this process is
Ca(OH)2(s)   +   CO2(g)   →   CaCO3(s)   +   H2O(g)       ΔH = -69.1 kJ
What is the enthalpy change if 3.8 mol of calcium carbonate is formed?
A.
-18 kJ
B.
-69 kJ
C.
-73 kJ
D.
-260 kJ
E.
-530 kJ


23.
Use Hess's Law to calculate the enthalpy change for the reaction
WO3(s)    +    3H2(g)    →    W(s)    +    3H2O(g)
from the following data:
W(s)     +    3/2 O2(g)    →    WO3(s)      ΔH = -842.7 kJ
H2(g)    +    1/2 O2(g)    →    H2O(g)      ΔH = -238.9 kJ
A.
126.0 kJ
B.
252.9 kJ
C.
364.9 kJ
D.
1207.6 kJ
E.
66.8 kJ


24.
Which one of the following equations represents the formation reaction of CH3OH(l)?
A.
C(g)   +   2H2(g)   +   ½O2 (g)   →   CH3OH(l)
B.
C(g)   +   4H(g)   +   O(g)   →   CH3OH(l)
C.
C(graphite)   +   4H(g)   +   O(g)   →   CH3OH(l)
D.
C(diamond)   +   4H(g)   +   O(g)   →   CH3OH(l)
E.
C(graphite)   +   2H2(g)   +   ½O2(g)   →   CH3OH(l)


25.
An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide.
4NH3(g)    +    5O2(g)    →    4NO(g)    +    6H2O(g)
Calculate ΔH°rxn for this reaction if:
ΔH°f [NH3(g)] = -45.9 kJ/mol
ΔH°f [NO(g)] = 90.3 kJ/mol       ΔH°f [H2O(g)] = -241.8 kJ/mol
A.
-906.0 kJ
B.
-197.4 kJ
C.
-105.6 kJ
D.
197.4 kJ
E.
906.0 kJ


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