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Q:
Ag+(aq) + e- -> Ag(s) E = +0.800 VAgBr(s) + e- -> Ag(s) + Br-(aq) E = +0.071 VBr2(l) + 2 e- -> 2 Br-(aq) E = +1.066 VUse some of the data above to calculate Ksp at 25C for AgBr.A) 6.3 10-2B) 4.9 10-13C) 1.9 10-15D) 2.4 10-34
Q:
Calculate the equilibrium constant, K, at 25C for the galvanic cell reaction shown below: A) 3.2 10-63
B) 3.2 10-13
C) 3.2 1012
D) 3.2 1062
Q:
The equilibrium constant, K, can be calculated from
A) E.
B) E.
C) either E or E.
D) neither E nor E.
Q:
When a cell reaction reaches equilibrium,
A) E = 0.
B) E = 0.
C) both E and E = 0.
D) neither E nor E = 0.
Q:
Consider the following cell:Where pHA is the pH of the aqueous solution in the anode half-cell and pHC is the pH of the aqueous solution in the cathode half-cell. If the partial pressure of H2(g) is the same for both half-cells, (p1 = p2), then E for the cell at 25C isA) 0.0296 V log (pHA/pHC).B) 0.0296 V log (pHC/pHA).C) 0.0592 V (pHA - pHC).D) 0.0592 V (pHC - pHA).
Q:
Consider a cell based on the following reaction:GeO(s) + H2O(l) + 2 Ag+(aq) -> GeO2(s) + 2 H+(aq) + 2 Ag(s)If [Ag+] = 1 M, at 25C,A) pH = 2(E - E)/0.0592 V.B) pH = (E - E)/0.0592 V.C) pH = (E - E)/0.0592 V.D) pH = 2(E - E)/0.0592 V.
Q:
A cell based on the reaction below has a standard potential of +0.42 V at 25C. If all of the species are at standard conditions except [H+], at what pH will the cell have a potential of zero?H2O2(aq) + 2 H+(aq) + 2 Cl-(aq) -> Cl2(aq) + 2 H2O(l)A) 3.55B) 7.09C) 10.6D) 14.2
Q:
The following cell has a potential of 0.45 V at 25C.The standard half-cell potential for the half-reaction . What is the pH in the anode compartment?A) 2.9B) 4.7C) 7.6D) 12.3
Q:
Which is most often used in the laboratory to measure pH?
A) a standard hydrogen electrode
B) a glass electrode
C) a Daniell cell
D) a conductivity cell
Q:
Consider the half-reaction: MnO4- (aq) + 8 H+ (aq) + 5 e- -> Mn2+ (aq) + 4 H2O(l). The formation of MnO4- from Mn2+ occurs most readily when the solution isA) acidic.B) neutral.C) basic.D) The reaction is not dependent upon pH.
Q:
How many moles of electrons, n, are transferred in the following reduction-oxidation reaction?2 MnO4-(aq) + 16 H+(aq) + 10 Cl-(aq) -> 2 Mn2+(aq) + 5 Cl2(g) + 8 H2O(l)A) 2B) 4C) 5D) 10
Q:
If the cell reaction involves ions in solution, as the cell reaction in a galvanic cell continues,
A) E for the cell increases.
B) E for the cell decreases.
C) E for the cell increases.
D) E for the cell decreases.
Q:
Given pH2 = 0.100 atm, [Cd2+] = 0.200 M, and [H+] = 1.00 10-5 M, calculate E at 25C for a cell based on the reaction:Cd(s) + 2 H+(aq) -> H2(g) + Cd2+(aq) Eo = +0.40 V.A) -0.09 VB) +0.12 VC) +0.15 VD) +0.30 V
Q:
Given that Ered = -0.26 V for Ni2+/Ni at 25C, find E and E for the concentration cell expressed using shorthand notation below.A) E = 0.00 V and E = +0.24 VB) E = 0.00 V and E = +0.12 VC) E = -0.26 V and E = -0.02 VD) E = -0.26 V and E = -0.14 V
Q:
Given that E= +0.897 V, calculate E at 25C forA) +0.779 VB) +0.935 VC) +1.015 VD) +1.134 V
Q:
At 25C, E = +1.88 V for a cell based on the reaction3 AgCl(s) + Al(s) -> 3 Ag(s) + Al3+(aq) + 3 Cl-(aq).Find the cell potential E if [Al3+] = 0.20 M and [Cl-] = 0.010 M.A) +2.01 VB) +2.04 VC) +2.28 VD) cannot be calculated without the amounts of AgCl, Al, and Ag
Q:
Calculate the cell potential E at 25C for the reaction2 Al(s) + 3 Fe2+(aq) -> 2 Al3+(aq) + 3 Fe(s)given that [Fe2+] = 0.020 M, [Al3+] = 0.10 M, and the standard reduction potential is -1.66 V for Al3+/Al and -0.45 V for Fe2+/Fe.A) +1.03 VB) +1.17 VC) +1.18 VD) +1.20 V
Q:
Calculate the cell potential at 25C for the cellgiven that the standard reduction potential for Fe2+/Fe is -0.45 V and for Pd2+/Pd is +0.95 V.A) +1.16 VB) +1.28 VC) +1.52 VD) +1.68 V
Q:
Calculate the value of the reaction quotient, Q, for the galvanic cell expressed using shorthand notation below. Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients.A) 156B) 125C) 8.00 x10-3D) 6.40 x10-3
Q:
Consider the galvanic cell, Pt(s) | H2(1 atm) | H+(1 M) || Cl-(1 M) | Hg2Cl2(s) | Hg(l). Which one of the following changes to the cell would cause the cell potential to increase (i.e., become more positive)?
A) decrease the mass of Pt
B) increase the mass of Pt
C) decrease the pH
D) increase the pH
Q:
Consider the galvanic cell, Pb(s) | Pb2+(aq) || Cu2+(aq) | Cu(s). Which one of the following changes to the cell would cause the cell potential to increase (i.e., become more positive)?
A) increase the [Pb2+] concentration
B) increase the [Cu2+] concentration
C) increase the mass of Pb(s)
D) decrease the mass of Pb(s)
Q:
What is the Al3+:Ag+concentration ratio in the cell if the measured cell potential is 2.34 V?A) 0.0094:1B) 0.21:1C) 4.7:1D) 110:1
Q:
Consider the following table of standard half-cell potentials:A2 + 2 e- -> 2 A- E = + 1.09 VB4+ + 2 e- -> B2+ E = + 0.15 VC3+ + 3 e- -> C E = - 1.66 VD2+ + 2 e- -> D E = - 2.37 VWhich substance is the strongest oxidizing agent?A) A2B) B4+C) C3+D) D2+
Q:
Use Table 17.1 to determine which of the following is the best oxidizing agent.
A) Fe3+
B) I2
C) MnO4-
D) Pb2+
Q:
Use Table 17.1 to calculate the standard potential for the reactionO2(g) + 4 H+(aq) + 2 Cu(s) -> 2 Cu2+(aq) + 2 H2O(l).A) -1.57 VB) -0.89 VC) +0.89 VD) +1.57 V
Q:
Using Table 17.1, find E for 2 H2O(l) -> 2 H2(g) + O2(g).A) -2.06 VB) -1.23 VC) -0.80 VD) -0.40 V
Q:
According to Table 17.1, which will reduce water but not Mg2+?
A) Al3+(aq)
B) Al(s)
C) Na+(aq)
D) Na(s)
Q:
According to Table 17.1, which aqueous metal ion will reduce Ag+, but not Cu2+?
A) Fe2+
B) Fe3+
C) Mn2+
D) Sn2+
Q:
Based on the half-reactions and their respective standard reduction potentials below, which addition to an aqueous solution containing Fe(NO3)2 will result in a reaction under standard-state conditions?O2(g) + 4 H+ +4 e- -> 2 H2O(l) 1.23 VFe3+(aq) + e- -> Fe2+(aq) 0.77 VCu2+(aq) + 2 e- -> Cu(s) 0.34 V2 H+(aq) + 2 e- -> H2(g) 0.00 VNi2+(aq) + + 2 e- -> Ni(s) -0.26 VFe2+(aq) + 2 e- -> Fe(s) -0.45 VA) aqueous copper(II) acetateB) nickel wireC) hydrogen gasD) oxygen gas
Q:
Based on the half-reactions and their respective standard reduction potentials below, what is the standard cell potential for the reaction that is expected to occur?Fe3+(aq) + e- -> Fe2+(aq) 0.77 VSn4+(aq) + 2 e- -> Sn2+(aq) 0.15 VPb2+(aq) + 2 e- -> Pb(s) -0.13 VA) 0.28 VB) 0.64 VC) 0.90 VD) 1.03 V
Q:
Given: Ag+(aq) + e- -> Ag(s) E = +0.799 VAgI(s) + e- -> Ag(s) + I-(aq) E = -0.152 VNi2+(aq) + 2 e- -> Ni(s) E = -0.267 VWhich of the following reactions should be spontaneous under standard conditions?I. 2 AgI(s) + Ni(s) -> 2 Ag(s) + 2 I-(aq) + Ni2+(aq)II. Ag+(aq) + I-(aq) -> AgI(s)A) I and II are both nonspontaneous.B) I is nonspontaneous and II is spontaneous.C) I is spontaneous and II is nonspontaneous.D) I and II are both spontaneous.
Q:
Using the following standard reduction potentialsFe3+(aq) + e- -> Fe2+(aq) E = +0.77 VPb2+(aq) + 2 e- -> Pb(s) E = -0.13 Vcalculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.Pb2+(aq) + 2 Fe2+(aq) -> 2 Fe3+(aq) + Pb(s)A) E = -0.90 V, nonspontaneousB) E = -0.90 V, spontaneousC) E = +0.90 V, nonspontaneousD) E = +0.90 V, spontaneous
Q:
Based on the following information,F2(g) + 2 e- -> 2 F-(aq) E = +2.87 VMg2+(aq) + 2 e- -> 2 Mg(s) E = -2.37 Vwhich of the following chemical species is the strongest reducing agent?A) F2(g)B) Mg2+(aq)C) F-(aq)D) Mg(s)
Q:
Consider the following standard reduction potentials,Al3+(aq) + 3 e- -> Al(s) E = -1.66 VI2(s) + 2 e- -> 2 I-(aq) E = +0.54 VUnder standard conditions,A) Al3+(aq) is a stronger oxidizing agent than I2(s), and I-(aq) is a stronger reducing agent than Al(s).B) I2(s) is a stronger oxidizing agent than Al3+(aq), and Al(s) is a stronger reducing agent than I-(aq).C) Al(s) is a stronger oxidizing agent than I-(aq), and Al3+(aq) is a stronger reducing agent than I2(s).D) I-(aq) is a stronger oxidizing agent than Al(s), and I2(s) is a stronger reducing agent than Al3+(aq).
Q:
Based on the half-reactions and their respective standard reduction potentials below, the strongest reducing agent is ________, and the strongest oxidizing agent is ________.Ag+(aq) + e- -> Ag(s) 0.80 V2 H+(aq) + 2 e- -> H2(g) 0.00 VCd2+(aq) + 2 e- -> Cd(s) -0.40 VA) Ag, Cd2+B) Ag+, CdC) Cd, Ag+D) Cd2+, Ag
Q:
A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions?Ag+(aq) + e- -> Ag(s) E = +0.80 VCu2+(aq) + 2 e- -> Cu(s) E = +0.34 VA) Ag(s) is formed at the cathode, and Cu(s) is formed at the anode.B) Ag(s) is formed at the cathode, and Cu2+ (aq) is formed at the anode.C) Cu(s) is formed at the cathode, and Ag+(aq) is formed at the anode.D) Cu2+(aq) is formed at the cathode, and Cu(s) is formed at the anode.
Q:
A galvanic cell consists of a La3+/La half-cell and a standard hydrogen electrode. If the La3+/La half-cell standard cell functions as the anode, and the standard cell potential is 2.52 V, what is the standard reduction potential for the La3+/La half-cell?
A) -2.52 V
B) -0.84 V
C) +0.84 V
D) +2.52 V
Q:
The standard potential for the following galvanic cell is +0.90 V:3 Cu2+(aq) + 2 Ga(s) 3 Cu(s) + 2 Ga3+(aq)Given that the standard reduction potential for the Cu2+/Cu half-cell is +0.34 V, what is the standard reduction potential for the Ga3+/Ga half-cell?A) -1.34 VB) -0.56 VC) +0.56 VD) +1.36 V
Q:
What is the standard cell potential for the reaction below?Mg(s) + Br2(l) -> Mg2+(aq) + 2 Br-(aq)The standard reduction potential is -2.37 V for the Mg2+/Mg half-cell and +1.09 V for the Br2/Br- half-cell.A) -3.46 VB) -1.28 VC) +1.28 VD) +3.46 V
Q:
What is the relationship between the standard cell potentials, E, for the following two galvanic cell reactions?I. 2 Ag+(aq) + Sn2+(aq) -> Sn4+(aq) + 2 Ag(s)II. Ag(s) + 1/2 Sn4+(aq) -> 1/2 Sn2+(aq) + Ag+(aq)A) E(I) = E(II)B) E(I) = 2E(II)C) E(I) = - E(II)D) E(I) = - 2E(II)
Q:
What is the relationship between the standard cell potentials, E, for the following two galvanic cell reactions?I. 3 Cu2+(aq) + 2 Al(s) -> 3 Cu(s) + 2 Al3+(aq)II. 6 Cu2+(aq) + 4 Al(s) -> 6 Cu(s) + 4 Al3+(aq)A) E(I) = E(II)B) E(I) = E(II)C) E(I) = 2E(II)D) E(I) = E(II)2
Q:
Which is not true for standard electrode potentials?
A) Cell constituents are in their standard states.
B) E for oxidation is the negative of E for reduction.
C) The half-reactions are written as reductions.
D) The potential for the standard hydrogen electrode is chosen to be +1.00 V.
Q:
For the hypothetical reaction A + 2 Bx -> Ay + 2 B, E = 1.50 V = and G = -305 kJ. For this reaction, if the value of x is 4, then the value of y = .A) 1B) 2C) 3D) 4
Q:
For the hypothetical reaction A + Bx -> Ax + B, E = 1.19 V = and G = -115 kJ. For this reaction the value of x = .A) 1B) 2C) 3D) 4
Q:
What is the relation between G and E for the cell reaction below?Ni2+(aq) + Cd(s) -> Cd2+(aq) + Ni(s)A) G = F EB) G = 2 F EC) G = -F ED) G = -2 F E
Q:
Doubling all the coefficients in the equation for the cell reactionA) doubles both E and G.B) doubles E, but does not change G.C) doubles G, but does not change E.D) does not change E or G.
Q:
The nickel-cadmium battery cell has a standard potential of +1.20 V. The cell reaction is2 NiO(OH)(s) + Cd(s) + 2 H2O(l) -> 2 Ni(OH)2(s) + Cd(OH)2(s).What is the standard free energy change for this reaction?A) -38.7 kJB) -116 kJC) -232 kJD) -463 kJ
Q:
For the reaction 2 Al(s) + 3 Co2+(aq) -> 2 Al3+(aq) + 3 Co(s), G is -799 kJ. What is E for a standard cell based on this reaction?A) +1.38 VB) +2.76 VC) +4.14 VD) +8.28 V
Q:
The cell reaction for a dry cell battery isZn(s) + 2 MnO2(s) + 2 NH4+(aq) -> 2 NH3(aq) + Mn2O3(s) + Zn2+(aq) + H2O(l).The standard cell potential for this cell is 1.56 V. What is the standard free energy change for this cell?A) +151 kJB) -151 kJC) -301 kJD) -602 kJ
Q:
In the relationship G = -nFE, what is the value of n for the reaction shown below?3 Cu2+(aq) + 2 Al(s) -> 3 Cu(s) + 2 Al3+(aq)A) 1B) 2C) 3D) 6
Q:
What is the relation between joules (J), volts (V), and coulombs (C)?
A) 1 J = 1 V 1 C
B) 1 J = 1 V 1 C
C) 1 J = 1 C 1 V
D) 1 J = 1 V 1 C2
Q:
Write the overall cell reaction for the galvanic cell given below.D) No reaction would occur because there is no salt bridge.
Q:
For the galvanic cell , what is the function of the Pt(s)?A) Pt is the anode and is a reactant in the overall cell reaction.B) Pt is the anode and does not appear in the overall cell reaction.C) Pt is the cathode and is a product in the overall cell reaction.D) Pt is the cathode and does not appear in the overall cell reaction.
Q:
What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?
Q:
What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below?
Q:
For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the anode?
Q:
For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode?
Q:
In the shorthand notation for a galvanic cell, a double vertical line representsA) a double phase boundaryB) an inert electrodeC) a phase boundaryD) a salt bridge
Q:
The shorthand notation for the galvanic cell reaction Fe3+(aq) + 2 I-(aq) -> Fe2+(aq) + I2(s) requires an inert electrode onA) both sides of the salt bridgeB) neither side of the salt bridgeC) only on the left side of the salt bridgeD) only on the right side of the salt bridge
Q:
What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?
Q:
What is the shorthand notation for a galvanic cell that represents the following galvanic cell reaction?Br2(l) + 2 I-(aq) ->2 Br-(aq) + I2(s)
Q:
What is the shorthand notation that represents the following galvanic cell reaction?2 Fe2+(aq) + Cl2(g) -> 2 Fe3+(aq) + 2 Cl-(aq)
Q:
What is the shorthand notation that represents the following galvanic cell reaction?Fe(s) + Cu(NO3)2(aq) -> Fe(NO3)2(aq) + Cu(s)
Q:
A galvanic cell employs the reactionMg2+(aq) + Cu(s) -> Mg(s) + Cu2+(aq)and NaNO3 is the salt used in the salt bridge. During the course of the reactionA) Na+ leaves the salt bridge and enters the anode compartment.B) NaNO3 leaves the salt bridge and enters the anode compartment.C) Na+ leaves the salt bridge and enters the cathode compartment.D) NaNO3 leaves the salt bridge and enters the cathode compartment.
Q:
For a galvanic cell that uses the following two half-reactions,Cr2O72-(aq) + 14 H+(aq) + 6 e- -> 2 Cr3+(aq) + 7 H2O(l)Pb(s) -> Pb2+(aq) + 2 e-how many moles of Pb(s) are oxidized by one mole of Cr2O72-?A) 1B) 2C) 3D) 6
Q:
The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing the iron(III) to iron(II), and titrating with cerium(IV):Fe2+(aq) + Ce4+(aq) -> Fe3+(aq) + Ce3+(aq).Identify the two half-reactions in the above reaction.A) oxidation half-reaction reduction half-reactionFe2+(aq) + e- -> Fe3+(aq) Ce4+(aq) -> Ce3+(aq) + e-B) oxidation half-reaction reduction half-reactionFe2+(aq) -> Fe3+(aq) + e- Ce4+(aq) + e- -> Ce3+(aq)C) oxidation half-reaction reduction half-reactionCe4+(aq) + e- -> Ce3+(aq) Fe2+(aq) -> Fe3+(aq) + e-D) oxidation half-reaction reduction half-reactionCe4+(aq) -> Ce3+(aq) + e- Fe2+(aq) + e- -> Fe3+(aq)
Q:
What is the reduction half-reaction for the following overall cell reaction?Ni2+(aq) + 2 Ag(s) -> Ni(s) + 2 Ag+(aq)A) Ag(s) + e- -> Ag+(aq)B) Ag+(aq) + e- -> Ag(s)C) Ni2+(aq) + 2 e- -> Ni(s)D) Ni2+(aq) + e- -> Ni(s)
Q:
Given that Cl2(g) + 2 e- -> 2 Cl-(aq) is the reduction half-reaction for the overall reaction2 Ag(s) + Cl2 (g) -> 2 AgCl(s), what is the oxidation half reaction?A) Ag(s) -> Ag+(aq) + e-B) Ag(s) + Cl-(aq) -> AgCl(s) + e-C) Ag(s) + Cl2(g) + e- -> AgCl(s) + Cl-(aq)D) 2 Cl-(aq) -> Cl2(g) + 2 e-
Q:
What species is oxidized in the reaction: CuSO4(aq) + Fe(s) -> FeSO4(aq) + Cu(s)?A) CuSO4 (aq)B) Fe (s)C) FeSO4 (aq)D) Cu (s)
Q:
In a galvanic cell, the half-reaction H2(g) + 2 OH-(aq) -> 2 H2O(l) + 2 e- isA) an oxidation half-reaction and occurs at the anode.B) an oxidation half-reaction and occurs at the cathode.C) a reduction half-reaction and occurs at the anode.D) a reduction half-reaction and occurs at the cathode.
Q:
In a galvanic cell, the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- -> Mn2+(aq) + 4 H2O(l) isA) an oxidation half-reaction and occurs at the anode.B) an oxidation half-reaction and occurs at the cathode.C) a reduction half-reaction and occurs at the anode.D) a reduction half-reaction and occurs at the cathode.
Q:
A salt bridge is used to
A) provide reactants in a fuel cell.
B) determine the direction of the cell reaction.
C) control whether the cell is electrolytic or galvanic.
D) allow the ion flow necessary for cell neutrality.
Q:
For a galvanic cell, the cathode has a ________ sign and is the site of ________.
A) negative, oxidation
B) negative, reduction
C) positive, oxidation
D) positive, reduction
Q:
During an electrochemical reaction, electrons move through the external circuit toward the ________ and positive ions in the cell move toward the ________.
A) anode, anode
B) anode, cathode
C) cathode, anode
D) cathode, cathode
Q:
Which cell involves a nonspontaneous redox reaction?
A) concentration cell
B) electrolytic cell
C) fuel cell
D) galvanic cell
Q:
Which of the following terms can be used to describe an electrochemical cell in which a spontaneous chemical reaction generates an electric current?
I. an electrolytic cell
II. a galvanic cell
III. a voltaic cell
A) only I
B) only II
C) only III
D) II and III
Q:
A 1.0 mole sample of gas at STP has a ________ entropy than 1.0 mole of gas at 273 K and
835 mm Hg.
Q:
If the entropy of a collection of molecules in 5000 boxes is 1.76 10-20 J/K, how many molecules are there?
Q:
By what factor does the entropy increase for a collection of 100 molecules from a system of 1 105 boxes to 1 106 boxes?
Q:
What is the entropy of 10 molecules in a system of 1000 boxes?