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Chemistry
Q:
For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode?
Q:
What is the shorthand notation that represents the following galvanic cell reaction?
Q:
What is the shorthand notation that represents the following galvanic cell reaction?
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):Identify the two half-reactions in the above reaction.oxidation half-reaction reduction half-reactionA) Fe2+(aq) + e-->Fe3+(aq) Ce4+(aq) -> Ce3+(aq) + e-B) Fe2+(aq) → Fe3+(aq) + e- Ce4+(aq) + e- -> Ce3+(aq)C) Ce4+(aq) + e- -> Ce3+(aq) Fe2+(aq) -> Fe3+(aq) + e-D) Ce4+(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 reaction 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:
The two half-reactions that are used in the direct methanol fuel cell are shown below.I 2 CH3OH(aq) + 2 H2O(l) -> 2 CO2(g) + 12 H+(aq) + 12 e"II 3 O2(g) + 12 H+(aq) + 12 e- -> 6 H2O(l)The electrode at which half-reaction I occurs is the ________ at which ________ is oxidized, and half-reaction II occurs at the ________ at which ________ is reduced.
Q:
The standard cell potential for the following galvanic cell is 0.71 V.
Mg(s)|Mg2+(aq)||Al3+(aq)|Al
This reaction has an equilibrium constant, K = ________.
Q:
The standard reduction potential Eo = - 0.45 V for the half-reaction Fe2+ + 2 e- -> Fe. If the measured cell potential at 25C is 0.35 V, the pH in the anode compartment of the following cell is ________.Pt(s)|H2(1 atm)|H+(? M)||Fe2+(1 M)|Fe(s)
Q:
The standard cell potential for the following galvanic cell is 1.21 V.
Al(s)|Al3+(aq)||Fe2+(aq)|Fe(s)
When [Al3+] = 0.10 M and [Fe2+] = 0.10 M, will the cell potential at 25C be less than, the same as, or greater than 1.21 V?
Q:
Reduction half-reactions with corresponding standard half-cell potentials are shown below.Ag+(aq) + 1 e--> Ag(s) E = + 0.80 VZn2+(aq) + 2 e- -> Zn(s) E = - 0.76 VAl3+(aq) + 3 e- -> Al(s) E = - 1.66 VOf the species above, the strongest oxidizing agent is ________, and the strongest reducing agent is ________.
Q:
Reduction half-reactions with corresponding standard half-cell potentials are shown below.Zn2+(aq) + 2 e- -> Zn(s) E = - 0.76 VAl3+(aq) + 3 e- -> Al(s) E = - 1.66 VThe standard potential for the galvanic cell that uses these two half-reactions is ________ V.
Q:
For the galvanic cell that uses the reaction2 Al(s) + 3 Zn2+(aq) -> 2 Al3+(aq) + 3 Zn(s)the value of n in the relationship G = - nFE is ________.
Q:
In the galvanic cell represented by the shorthand notation
Al(s)|Al3+(aq)||Fe3+(aq)|Fe(s)
the anode is ________ and the cathode is ________.
Q:
A galvanic cell uses the reactionMg(s) + Pb2+(aq) -> Mg2+(aq) + Pb(s).Mg(s) -> Mg2+(aq) + 2 e- is the ________ half-reaction, which occurs at the ________.
Q:
How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 5.00 moles of copper metal?A) 0.187 hoursB) 0.373 hoursC) 2.68 hoursD) 5.36 hours
Q:
How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl2 for 60.0 minutes?
A) 10.9 g
B) 16.4 g
C) 32.8 g
D) 36.3 g
Q:
How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320. minutes?
A) 27.6 g
B) 49.2 g
C) 82.4 g
D) 248 g
Q:
The equilibrium constant, K, for a redox reaction at 25 C is 3.3 . What is the value of E if the overall reaction transfers 2 electrons?
A) 0.93 V
B) 1.9 V
C) 2.2 V
D) 0.60 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) 132B) 115C) 8.70 10-3D) 7.56 10-3
Q:
Consider the galvanic cell, Which one of the following changes to the cell would cause the cell potential to increase (i.e., become more positive)?
A) increase the [Zn2+] concentration
B) increase the [Pb2+] concentration
C) increase the mass of Zn(s)
D) decrease the mass of Zn(s)
Q:
Using the following standard reduction potentials,Fe3+(aq) + e- ->Fe2+(aq) E = +0.77 VCd2+(aq) + 2 e- -> Cd(s) E = -0.40 Vcalculate the standard cell potential for the cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions.Cd2+(aq) + 2 Fe2+(aq) -> 2 Fe3+(aq) + Cd(s)A) E = -1.17 V, nonspontaneousB) E = -1.17 V, spontaneousC) E = +1.17 V, nonspontaneousD) E = +1.17 V, spontaneous
Q:
Calculate G for the following galvanic cell given these reduction potentials:A) -59.8 kJB) 59.8 kJC) -29.8 kJD) 29.8 kJ
Q:
Based on the following information,Cl2(g) + 2 e- -> 2 Cl-(aq) E° = +1.36 VMg2+(aq) + 2 e- ->2 Mg(s) E° = -2.37 Vwhich of the following chemical species is the strongest reducing agent?A) Cl2(g)B) Mg2+(aq)C) Cl-(aq)D) Mg(s)
Q:
Consider the following standard reduction potentials,VUnder standard conditions,A) Ni2+(aq) is a stronger oxidizing agent than I2(s) and I-(aq) is a stronger reducing agent than Ni(s).B) I2(s) is a stronger oxidizing agent than Ni2+(aq) and Ni(s) is a stronger reducing agent than I-(aq).C) Ni(s) is a stronger oxidizing agent than I-(aq) and Ni2+(aq) is a stronger reducing agent than I2(s).D) I-(aq) is a stronger oxidizing agent than Ni(s) and I2(s) is a stronger reducing agent than Ni2+(aq).
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?A) Ag(aq) 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 Ni2+/Ni half-cell and a standard hydrogen electrode. If the Ni2+/Ni half-cell standard cell functions as the anode, and the standard cell potential is 0.26 V, what is the standard reduction potential for the Ni2+/Ni half-cell?
A) -0.26 V
B) -0.13 V
C) +0.13 V
D) +0.26 V
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 cathode?
Q:
What is the shorthand notation that represents the following galvanic cell reaction?
Q:
What is the shorthand notation that represents the following galvanic cell reaction?
Q:
What is the reduction half-reaction for the following overall cell reaction?Co2+(aq) + 2 Ag(s) -> Co(s) + 2 Ag+(aq)A) Ag(s) + e- -> Ag+(aq)B) Ag+(aq) + e- -> Ag(s)C) Co2+(aq) + 2 e- -> Co(s)D) Co2+(aq) + e- -> Co(s)
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 three moles of Cr2O72-?A) 3B) 6C) 9D) 18
Q:
Determine the direction of electron flow and the direction of ion flow.A) Electrons flow from a to c; K+ ions flow toward a and Cl- ions flow toward c.B) Electrons flow from a to c; Cl- ions flow toward a and K+ ions flow toward c.C) Electrons flow from c to a; K+ ions flow toward a and Cl- ions flow toward c.D) Electrons flow from c to a; Cl- ions flow toward a and K+ ions flow toward c.
Q:
Shown below is an electrochemical cell with anode a and cathode c. Both the anode and the cathode are inert electrodes. The liquid shown in compartment b of the cell is molten potassium chloride, KCl(l).Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the anode and the reaction occurring at the cathode.A) Electrolytic cellAnode reaction: K(s) -> K+(l) + e-Cathode reaction: Cl2(g) + 2e- -> 2 Cl-(l)B) Electrolytic cellAnode reaction: 2 Cl-(l) -> Cl2(g) + 2e-Cathode reaction: K+(l) + e- -> K(s)C) Galvanic cellAnode reaction: K(s) -> K+(l) + e-Cathode reaction: Cl2(g) + 2e- -> 2 Cl-(l)D) Galvanic cellAnode reaction: K(s) - K+(l) + e-Cathode reaction: Cl2(g) + 2e- -> 2 Cl-(l)
Q:
Is the cell shown above a galvanic or an electrolytic cell? What is the direction of ion flow?A) Electolytic cell; Cu2+ ions flow toward electrode x and SO42- ions flow toward electrode y.B) Electolytic cell; Cu2+ ions flow toward electrode y and SO42- ions flow toward electrode x.C) Galvanic cell; Cu2+ ions flow toward electrode x and SO42- ions flow toward electrode y.D) Galvanic cell; Cu2+ ions flow toward electrode y and SO42- ions flow toward electrode x.
Q:
Is the cell shown above a galvanic or an electrolytic cell? Which is the anode and which is the cathode?A) Electolytic cell; electrode x is the anode and electrode y is the cathode.B) Electolytic cell; electrode y is the anode and electrode x is the cathode.C) Galvanic cell; electrode x is the anode and electrode y is the cathode.D) Galvanic cell; electrode y is the anode and electrode x is the cathode.
Q:
What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?A) +0.03 VB) +0.02 VC) -0.02 VD) -0.03 V
Q:
Consider the galvanic cell shown below.What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?A) +0.03 VB) +0.02 VC) -0.02 VD) -0.03 V
Q:
What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?A) +0.06 VB) +0.03 VC) -0.03 VD) -0.06 V
Q:
Consider the following galvanic cell.What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?A) +0.06 VB) +0.03 VC) -0.03 VD) -0.06 V
Q:
The initial concentrations of Ag+(aq) and Cu2+(aq) are both What will happen to the cell voltage if AgNO3 is added to the compartment containing the Ag+(aq)? The cell voltage willA) decrease.B) increase.C) remain the same.D) can't tell from the information given
Q:
The initial concentrations of Ag+(aq) and Cu2+(aq) are both What will happen to the cell voltage if Cu(NO3)2 is added to the compartment containing the Cu2+(aq)? The cell voltage will
A) decrease.
B) increase.
C) remain the same.
D) can't tell from the information given
Q:
The initial concentrations of Ag+(aq) and Cu2+(aq) are both What will happen to the cell voltage if Cu(NO3)2 is added to the compartment containing the Cu2+(aq)? The cell voltage will
A) decrease.
B) increase.
C) remain the same.
D) can't tell from the information given
Q:
If the concentrations of Ag+(aq) and Cu2+(aq) are varied in this galvanic cell, which of the following four cells has the largest cell potential?
A) [Ag+] = 0.10 M and [Cu2+] = 0.10 M
B) [Ag+] = 1.0 M and [Cu2+] = 0.10 M
C) [Ag+] = 0.10 M and [Cu2+] = 1.0 M
D) [Ag+] = 1.0 M and [Cu2+] = 1.0 M
Q:
Given the half-cell potentials below, calculate the cell potential.Ag+(aq) + e- -> Ag(s) 0.80 VCu2+(aq) + 2 e- -> Cu(s) 0.34 VA) 0.46 VB) 1.14 VC) 1.26 VD) 1.94 V
Q:
What is the shorthand notation for this cell?
Q:
Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.A) Anode reaction: Ag+(aq) + e- -> Ag(s) (oxidation)Cathode reaction: Cu(s) -> Cu2+(aq) + 2e- (reduction)B) Anode reaction: Ag+(aq) + e- -> Ag(s) (reduction)Cathode reaction: Cu(s) -> Cu2+(aq) + 2e- (oxidation)C) Anode reaction: Cu(s) -> Cu2+(aq) + 2e- (oxidation)Cathode reaction: Ag+(aq) + e- -> Ag(s) (reduction)D) Anode reaction: Cu(s) -> Cu2+(aq) + 2e- (reduction)Cathode reaction: Ag+(aq) + e- -> Ag(s) (oxidation)
Q:
NaNO3(aq) is employed in the salt bridge. Give the direction of electron flow and the direction of ion flow from the salt bridge.
A) Electrons flow from a to c; Na+ flows into b and NO3- flows into d.
B) Electrons flow from a to c; NO3- flows into b and Na+ flows into d.
C) Electrons flow from c to a; Na+ flows into b and NO3- flows into d.
D) Electrons flow from c to a; NO3- flows into b and Na+ flows into d.
Q:
Identify and give the sign of each electrode.
A) a is Ag and (+), c is Cu and (-).
B) a is Ag and (-), c is Cu and (+).
C) a is Cu and (+), c is Ag and (-).
D) a is Cu and (-), c is Ag and (+).
Q:
Shown below is a galvanic cell with anode compartment b containing anode a and cathode compartment d containing cathode c. Electrons flow through wire f, ions flow through salt bridge e, and the cell potential is read using voltmeter g.This galvanic cell uses the reaction: Identify the electrodes and the direction of electron flow.A) a is Ag, c is Cu and electrons flow from a to c.B) a is Ag, c is Cu and electrons flow from c to a.C) a is Cu, c is Ag and electrons flow from a to c.D) a is Cu, c is Ag and electrons flow from c to a.
Q:
What is the shorthand notation for the cell?A) Fe(s) | Fe2+(aq) || Sn(s) | Sn2+(aq)B) Fe(s) | Fe2+(aq) || Sn2+(aq) | Sn(s)C) Sn(s) | Sn2+(aq) || Fe(s) | Fe2+(aq)D) Sn(s) | Sn2+(aq) || Fe2+(aq) | Fe(s)
Q:
What is the balanced equation for the cell reaction?A) Fe(s) + Sn(s) -> Fe2+(aq) + Sn2+(aq)B) Fe2+(aq) + Sn2+(aq) -> Fe(s) + Sn(s)C) Fe(s) + Sn2+(aq) -> Fe2+(aq) + Sn(s)D) Fe2+(aq) + Sn(s) -> Fe(s) + Sn2+(aq)
Q:
Identify the anode and cathode, and indicate the direction of ion flow to and from each electrode.
A) Fe is the anode and Sn is the cathode; Fe2+ ions flow to the anode and Sn2+ ions flow from the cathode.
B) Fe is the anode and Sn is the cathode; Sn2+ ions flow to the cathode and Fe2+ ions flow from the anode.
C) Sn is the anode and Al is the cathode; Fe2+ ions flow to the cathode and Sn2+ ions flow from the anode.
D) Sn is the anode and Al is the cathode; Sn2+ ions flow to the anode and Fe2+ ions flow from the cathode.
Q:
Consider the following galvanic cell.Identify the anode and cathode, and indicate the direction of Na+ ion and NO3- ion flow from the salt bridge.A) Fe is the anode and Sn is the cathode; Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B).B) Fe is the anode and Sn is the cathode; NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B).C) Sn is the anode and Fe is the cathode; Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B).D) Sn is the anode and Fe is the cathode; NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B).
Q:
What is the shorthand notation for the cell?A) Al(s) | Al3+(aq) || Co(s) | Co2+(aq)B) Al(s) | Al3+(aq) || Co2+(aq) | Co(s)C) Co(s) | Co2+(aq) || Al(s) | Al3+(aq)D) Co(s) | Co2+(aq) || Al3+(aq)| Al(s)
Q:
What is the balanced equation for the cell reaction?A) 2 Al(s) + 3 Co(s) -> 2 Al3+(aq) + 3 Co2+(aq)B) 2 Al3+(aq) + 3 Co2+(aq) -> 2 Al(s) + 3 Co(s)C) 2 Al(s) + 3 Co2+(aq) -> 2 Al3+(aq) + 3 Co(s)D) 2 Al3+(aq) + 3 Co(s) -> 2 Al(s) + 3 Co2+(aq)
Q:
Identify the anode and cathode, and indicate the direction of ion flow to and from each electrode.
A) Al is the anode and Co is the cathode; Al3+ ions flow to the anode and Co2+ ions flow from the cathode.
B) Al is the anode and Co is the cathode; Co2+ ions flow to the cathode and Al3+ ions flow from the anode.
C) Co is the anode and Al is the cathode; Al3+ ions flow to the cathode and Co2+ ions flow from the anode.
D) Co is the anode and Al is the cathode; Co2+ ions flow to the anode and Al3+ ions flow from the cathode.
Q:
Consider the galvanic cell shown below.Identify the anode and cathode, and indicate the direction of Na+ ion and NO3- ion flow from the salt bridge.A) Al is the anode and Co is the cathode; Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B).B) Al is the anode and Co is the cathode; NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B).C) Co is the anode and Al is the cathode; Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B).D) Co is the anode and Al is the cathode; NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B).
Q:
The standard free energy for a reaction is G = - 33.0 kJ. At 25C the equilibrium constant for this reaction , Kp = ________.
Q:
Standard free energies of formation, G, in kJ/mol, are given below each reactant and product in the reaction shown below. The standard free energy of reaction, G, for this reaction is ________ kJ.CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l)- 50.8 0 - 394.4 - 237.2
Q:
Acetylene, C2H2, has a standard enthalpy of formation, H = 226.7 kJ/mol, and a standard entropy change for its formation from its elements, S = 58.8 J/Kmol. The standard free energy of formation of acetylene is ________ kJ/mol.
Q:
A reaction has G = + 21.5 kJ/mol, H = + 25.0 kJ/mol, and S= +15.0 J/molK can become spontaneous at a temperature of ________ K.
Q:
A reaction for which H = + 98.8 kJ and S = + 141.5 J/K is ________ (spontaneous or nonspontaneous) at low temperatures and ________ (spontaneous or nonspontaneous) at high temperatures.
Q:
Standard molar entropies, S, in J/Kmol, are given below each reactant and product in the reaction shown below. The standard entropy of reaction, S, for this reaction is ________ J.CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l)186.2 205.0 213.6 69.9
Q:
The entropy of water at 25 is ________ than the entropy of water at 35C.
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:
The sign (+ or ") of â–³H is ________ and the sign (+ or ") of â–³S is ________ for the evaporation of water.
Q:
Chemical and physical changes can be classified as spontaneous or nonspontaneous. At 25C and 1 atm pressure the decomposition of water into hydrogen and oxygen is classified as ________, and the melting of ice is classified as ________.