1.
Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.1 × 10–12).
A.
5.0 × 10–5 M
B.
2.5 × 10–4 M
C.
1.3 × 10–4 M
D.
2.0 × 10–4 M
E.
8.1 × 10–4 M


2.
The overall Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. The Ksp for AgI is 1.5 × 10–16. What is the molar solubility of AgI in a solution that is 2.0 M in NH3?
A.
1.5 × 10–9
B.
1.3 × 10–3
C.
1.0 × 10–4
D.
5.8 × 10–12
E.
8.4 × 10–5


3.
Which of the following result(s) in an increase in the entropy of the system?
I.
 
The isothermal expansion shown in the diagram above.
II.
 
Br2(g) → Br2(l)
III
 
.NaBr(s) → Na+(aq) + Br–(aq)
IV.
 
O2(298 K) → O2(373 K)
V.
 
NH3(1 atm, 298 K) → NH3(3 atm, 298 K)
 
A.
I
B.
II, V
C.
I, III, IV
D.
I, II, III, IV
E.
I, II, III, V


4.
For a particular chemical reaction ΔH = 5.5 kJ and ΔS = –25 J/K Under what temperature condition is the reaction spontaneous?
A.
When T < –220 K.
B.
When T < 220 K.
C.
The reaction is spontaneous at all temperatures.
D.
The reaction is not spontaneous at any temperature.
E.
When T > 220 K.


5.
Which of the following statements is always true for a spontaneous process?
I.
 
ΔSsys > 0
II
 
.ΔSsurr > 0
III
 
.ΔSuniv > 0
IV.
 
ΔGsys > 0
 
A.
I
B.
III
C.
IV
D.
I and III
E.
III and IV


6.
Consider the freezing of liquid water at –10°C. For this process what are the signs for ΔH, ΔS, and ΔG?
   
ΔH
ΔS
ΔG
 
A.
   
+
–
0
 
B.
+
–
0
 
C.
–
+
0
 
D.
–
+
–
 
E.
–
–
–
 


7.
The melting point of water is 0°C at 1 atm pressure because under these conditions
A.
ΔS for the process H2O(s) → H2O(l) is positive.
B.
ΔS and ΔSsurr for the process H2O(s) → H2O(l) are both positive.
C.
ΔS and ΔSsurr for the process H2O(s) → H2O(l) are equal in magnitude and opposite in sign.
D.
ΔG is positive for the process H2O(s) → H2O(l).
E.
None of these is correct.


8.
For the reaction 2HF(g) H2(g) + F2(g), ΔG° = 38.3 kJ, at 1000 K. If, at this temperature, 5.00 moles of HF(g), 0.500 moles of H2(g), and 0.75 moles of F2(g) are mixed in a 1.00-L container:
A.
Some HF will decompose (to yield H2 and F2).
B.
The system is at equilibrium.
C.
Some HF will be formed (from H2 and F2).
D.
Not enough data are given to answer this question.
E.
None of the other choices.


9.
Calculate E at 25°C for the cell shown below, given the following data:  

Ksp for AgCl = 1.6 × 10–10
A.
0.83 V
B.
0.54 V
C.
1.01 V
D.
2.98 V
E.
E cannot be determined from the given data


10.
A galvanic cell is constructed with copper electrodes and Cu2+ in each compartment. In one compartment, the [Cu2+] = 1.0 × 10–3 M and in the other compartment, the [Cu2+] = 2.0 M. Calculate the potential for this cell at 25°C. The standard reduction potential for Cu2+ is +0.34 V.
A.
0.44 V
B.
–0.44 V
C.
0.098 V
D.
–0.098 V
E.
0.78 V


11.
Given the following standard reduction potentials,
Ag+(aq) + e– → Ag(s)
E° = 0.80 V
AgCN(s) + e– → Ag(s) + CN–(aq)
E° = –0.01 V

calculate the solubility product of AgCN at 25°C.
A.
4.3 × 10–14
B.
2.3 × 1013
C.
2.0 × 10–14
D.
5.1 × 1013
E.
None of the other choices


12.
To plate the metal bumper of an old car with chromium it is dipped into a solution containing Cr3+ ions and used as an elecrolytic cell cathode. How long will it take to deposit 100 × 102 grams of Cr(s) onto the bumper if the current passed is 10.0 amperes?
A.
10.3 h
B.
1.29 days
C.
309 min
D.
76.3 s
E.
85.5 days


13.
The standard potential of the galvanic cell :

       In In3+ (1.00 M)  Cu2+ (1.00 M)  Cu

is 0.68 V. What voltage will the cell have after it
is discharged until [Cu2+] = 0.010 M.
A.
0.62 V
B.
0.50 V
C.
0.74 V
D.
0.56 V
E.
0.68 V


14.
Given:
Br2 (l)     +     2 e -      =   2 Br - (aq) ,   = 1.07 V
Fe 3+ (aq)   +    e -     =   Fe 2+ (aq) ,   = 0.77 V
The oxidation of Br - (aq) by Fe 3+ (aq) is :
A.
nonspontaneous and (cell) = 0.30 V
B.
spontaneous and (cell) = 0.30 V
C.
spontaneous and (cell) = +1.84 V
D.
nonspontaneous and (cell) = 1.84 V
E.
spontaneous and (cell) = + 0.30 V


15.
Which nuclide is produced when a K nuclide captures an electron?
A.
Ca
B.
Ar
C.
He
D.
K–
E.
Ca


16.
Which one of the following processes is given the wrong label?
Process
Process Balanced Equation
Process Label
I
Bi + He → At + 2n
Fission
II
H + H → H + H
Fusion
III
Pu + n → Am +e
Bombardment
IV
U → Np + e
Beta production
V
Be + e → Li
Electron capture
 
A.
I
B.
II
C.
III
D.
IV
E.
V


17.
The ratio of nuclei to nuclei in an archeological sample is 0.400.
Given that the half-life of is 4.5 x 10 9 years calculate the age of the
sample assuming that all the came from and neglecting other
radioactive nuclei present in it.  
A.
2.93 x 10 7   years
B.
3.67 x 10 10 years
C.
2.18 x 10 9   years
D.
8.96 x 10 12 years
E.
3.54 x 10 9 years


18.
Calculate ΔE in kilojoules per mole for the following reaction:
              Th → He + Ra
Atomic masses: 230Th = 230.0332, 4He = 4.00260, 226Ra = 226.02544.
A.
–4.6 × 108 kJ/mol
B.
–2.4 × 106 kJ/mol
C.
0
D.
+2.4 × 106 kJ/mol
E.
+4.6 × 108 kJ/mol


19.
The nucleus undergoes only and decays to form . There are
X decays and Y decays. Which of the following values of X and Y are
correct?
A.
X = 8 , Y = 6
B.
X = 6 , Y = 8
C.
X = 6 , Y = 4
D.
X = 4 , Y = 6
E.
X = 4 , Y = 4


20.
Which types of processes are likely when the neutron-to-proton ratio in a nucleus is too low?
I.
 
α decay
II.
 
β decay
III
 
.pisitron production
IV.
 
electron capture
 
A.
I, II
B.
II, III
C.
III, IV
D.
II, III, IV
E.
II, IV


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