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Exam 4

Navigation   » List of Schools  »  Glendale Community College  »  Chemistry  »  Chem 102 – General Chemistry  »  Winter 2022  »  Exam 4

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Below are the questions for the exam with the choices of answers:

Question #1
What is the shorthand notation that represents the following galvanic cell reaction?  
2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2 Cl-(aq)
A  Fe2+(aq) , Fe3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
B  Pt I Fe2+(aq) , Fe3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
C  PtI Cl-(aq) ∣ Cl2(g) ∣∣ Fe3+(aq), Fe2+IPt
D  Pt I Fe2+(aq) , Fe3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) I Pt
Question #2
A voltaic cell prepared using zinc and iodine has the following line notation.

Zn(s) | Zn2+(aq) || I2(s) | I-(aq) | C (graphite)

Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

A  2I-(aq) + Zn(s) → I2(s) + Zn2+(aq)
B  2I-(aq) + Zn2+(aq) → I2(s) + Zn(s)
C  I2(s) + Zn(s) → 2I-(aq) + Zn2+(aq)
D  None of these, since graphite must be in the equation.
E  I2(s) + Zn2+(aq) → 2I-(aq) + Zn(s)
Question #3
In one episode of the 1960s television sitcom, Gilligan’s Island, the famous “professor” constructed voltaic cells to use as substitutes for their radio’s dead batteries. A single D-cell has an emf of 1.5 V. Which scraps of metal from their damaged boat, the Minnow, could best be used to create a 1.5 V voltaic cell? Assume that coconuts make great beakers and that seawater is a terrific electrolyte.
Metal/Metal ion
iron/iron(II) (the anchor) –0.44 V
lead/lead(II) (fishing weights) –0.126 V
silver/silver(I) (Mrs. Howell’s brooch) +0.799 V
aluminum/aluminum(III) (the boat’s flagpole) –1.677 V
A  aluminum anode and lead cathode
B  silver anode and lead cathode
C    
D  lead cathode and silver anode
E  iron anode and aluminum cathode
F  aluminum anode and silver cathode
Question #4
According to the standard reduction potentials
Pb2+(aq) + 2e- → Pb(s) E˚= -0.12 V
Fe2+(aq) + 2e- → Fe(s) E˚= -0.44 V
Zn2+(aq) + 2e- → Zn(s) E˚= -0.76 V
Which species will reduce Mn3+ to Mn2+ (E° = 1.51 V),
but will NOT reduce Cr3+ to Cr2+ (E° = –0.40 V)?
A  Zn only
B  none of these
C  Pb, Fe, and Zn
D  Pb only
E  Pb and Fe onnly
Question #5
Consider the galvanic cell, Zn(s) ∣ Zn2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s).
Which one of the following changes to the cell would cause the cell potential to decrease (i.e., become Less positive)?
A  decrease the [ Zn2+] concentration
B  decrease the mass of Zn(s)
C  increase the [ Pb2+] concentration
D  increase the [ Zn2+] concentration
E  decrease the mass of Pb(s)
Question #6
3Ag2S(s) + 2Al(s) +6OH–(aq) –> 6Ag(s) + 2Al(OH)3(s) + 3S2–-(aq)
For the above reaction would the Ecell increase  decrease or remain the same if a strong acid is added on the anode.
A  increases
B  decreases
C  can’t tell
D  remains the same
Question #7
Consider the following balanced redox reaction
Mn2+(aq) + S2O82-(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2SO42-(aq)
Which of the following statements is true? 
A  Mn2+(aq) is the oxidizing agent and is oxidized.
B  Mn2+(aq) is the oxidizing agent and is reduced
C  S2O82-(aq) is the reducing agent and is oxidized.
D  Mn2+(aq) is the reducing agent and is oxidized.
E  Mn2+(aq) is the reducing agent and is reduced.
Question #8
Which substance would have the largest standard molar entropy?
A  H2O2(aq)
B  H2O2(l)
C  NO2(l)
D  NO2(aq)
Question #9
The reaction  Cr(en)33+(aq) + 6 NH3(aq) –> Cr(NH3)63+(aq) + 3en(aq)  where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction.
A  the reaction is non-spontaneous for all temperatures.
B  the reaction is spontaneous for all temperatures.
C  the reaction is spontaneous for low temperatures.
D  not enough info to tell.
E  the reaction is spontaneous for high temperatures.
Question #10
Place the following in order of decreasing standard molar entropy.
NaCl(g)            Na3PO4(aq)            NaCl(aq)
A  NaCl(aq) > Na3PO4(aq)  >  NaCl(g)
B  Na3PO4(aq)  >  NaCl(aq)  >  NaCl(g)
C   NaCl(g) > Na3PO4(aq)  >  NaCl(aq) 
D   NaCl(aq) >  NaCl(g) > Na3PO4(aq)
E   NaCl(g) >  NaCl(aq) > Na3PO4(aq)
Question #11
When a solution of DNA in water is heated (energy as heat is transferred), the double helix separates into two single strands. This process is called melting. What can be deduced from this information about the signs of the enthalpy and entropy changes for DNA melting?
A  This information is not sufficient to determine the signs of ΔH and ΔS.
B  ΔH < 0 and ΔS > 0
C  ΔH > 0 and ΔS < 0
D  ΔH < 0 and ΔS < 0
E  ΔH > 0 and ΔS > 0
Question #12
Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 35oC. Predict whether or not this reaction will be spontaneous at this temperature.

CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) ΔHorxn = -890.4 kJ

A  ΔSsurr = +25.44 kJ/K, reaction is spontaneous
B  ΔSsurr = -25.44 kJ/K, reaction is spontaneous
C  ΔSsurr = -25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.
D  ΔSsurr = -2.89 kJ/K, reaction is non-spontaneous
E  ΔSsurr = +25.44 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.
F  ΔSsurr = +2.89 kJ/K, it is not possible to predict the spontaneity of this reaction without more information.
Question #13
The reaction   4 Ag(s) + O2(g)  → 2 Ag2O(s) favors Ag2O at low temperature, but it favors Ag and O2 at high temperatures. How can this be explained in terms of ΔH and ΔS?   
A  None of the choices are correct
B  ΔH is positive and ΔS is positive.
C  ΔH is negative and ΔS is negative.
D  ΔH is positive and ΔS is negative.
E  ΔH is negative and ΔS is positive.
Question #14
For a chemical reaction that is spontaneous in the reverse direction, it is found that ΔSsys > 0. This means ________
A  ΔSsurr > 0 and its magnitude does not matter.
B  ΔSsurr > 0 and its magnitude is > ΔSsys.
C  an error has been made, because ΔSsys > 0 by necessity for a spontaneous process.
D  ΔSsurr < 0 and its magnitude is > ΔSsys.
E  ΔSsurr > 0 and its magnitude is < ΔSsys.
F  ΔSsurr < 0 and its magnitude is < ΔSsys.
Question #15
For a process with ΔSsys < 0, which one of the following statements is correct? 
A  The process will definitely be spontaneous if ΔH < 0.
B  The process can never be spontaneous.
C  The process will definitely be spontaneous if ΔSsurr > 0.
D  The process will be definitely be spontaneous if ΔH < TΔSsys.
E  The process will definitely be spontaneous, regardless of ΔH
Question #16
The molar solubility of __________ is not affected by the pH of the solution.
A  NaF
B  Na3PO4
C  MnS
D  NaCN
E  KNO3
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