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What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s) ∣ Ba2+(aq) What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s) ∣ Ba<sup>2+</sup>(aq)    Ag<sup>+</sup>(aq) ∣ Ag(s)  A)  Ba(s)  B)  Ag<sup>+</sup>(aq)  C)  Ba<sup>2+</sup>(aq)  D)  Ag(s)  E)  Pt Ag+(aq) ∣ Ag(s)


A) Ba(s)
B) Ag+(aq)
C) Ba2+(aq)
D) Ag(s)
E) Pt

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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) 1
B) 2
C) 3
D) 6

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Predict the species that will be reduced first if the following mixture of molten salts undergoes electrolysis. Zn2+,Fe3+,Mg2+,Br-,I-


A) Zn2+
B) Mg2+
C) Br-
D) Fe3+
E) I-

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Identify a component in the formation of rust.


A) salt
B) moisture
C) acid
D) all of the above
E) none of the above

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What is the reduction half-reaction for the following overall galvanic cell reaction? Pb2+(aq) + 2 Ag(s) → Pb(s) + 2 Ag+(aq)


A) Ag(s) + e- → Ag+(aq)
B) Ag+(aq) + e- → Ag(s)
C) Pb2+(aq) + 2 e- → Pb(s)
D) Pb2+(aq) + e- → Pb(s)

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A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s) + e- → Ag(s) + Cl-(aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0100 M and 1.55 M,respectively.The cell emf is ________ V.


A) 0.216
B) 0.130
C) 0.00143
D) 34.4
E) 0.228

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Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.


A) Pb2+(aq) + Au(s)
B) Ag+(aq) + Br⁻(aq)
C) Li+(aq) + Cr(s)
D) Fe3+(aq) + Ni(s)
E) None of the above pairs will react.

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Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Ni and Ag+ in the balanced reaction? Ni(s) + Ag+(aq) → Ag(s) + Ni2+(aq)


A) Ni = 1, Ag⁺ = 2
B) Ni = 1, Ag⁺ = 1
C) Ni = 2, Ag⁺ = 1
D) Ni = 2, Ag⁺ = 2
E) Ni = 3, Ag⁺ = 1

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What element is being oxidized in the following redox reaction? Cr(OH) 4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)


A) Cr
B) O
C) H
D) Cl

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 3 Cl2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe3+(aq) Cl2(g) + 2 e⁻ → 2 Cl⁻(aq) E° = +1.36 V Fe3+(aq) + 3 e⁻ → Fe(s) E° = -0.04 V


A) +4.16 V
B) -1.40 V
C) -1.32 V
D) +1.32 V
E) +1.40 V

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Using the following standard reduction potentials, Fe3+(aq) + e- →Fe2+(aq) E° = +0.77 V Cu2+(aq) + 2 e- →Cu(s) E° = +0.34 V Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions. Cu2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Cu(s)


A) E° = - 0.43 V, nonspontaneous
B) E° = - 0.43 V, spontaneous
C) E° = + 0.43 V, nonspontaneous
D) E° = + 0.43 V, spontaneous

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What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? Ag⁺(aq) + e⁻ → Ag(s)


A) 19.6 g
B) 0.326 g
C) 9.78 g
D) 3.07 g
E) 0.102 g

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What is the difference between a voltaic cell and an electrolytic cell?

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A voltaic cell contains a redox reaction...

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How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq)


A) 1
B) 2
C) 6
D) 3
E) 4

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) Mg2+(aq) + 2 e⁻ → Mg(s) E° = -2.38 V Cu2+(aq) + 2 e⁻ → Cu(s) E° = +0.34 V


A) +2.04 V
B) -2.04 V
C) +2.72 V
D) -1.36 V
E) +1.36 V

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Balance the following redox reaction if it occurs in H2SO4.What are the coefficients in front of C3H8O2 and H2SO4 in the balanced reaction? C3H8O2(aq) + K2Cr2O7(aq) → C3H4O4(aq) + Cr2(SO4) 3(aq)


A) C3H8O2 = 3, H2SO4 = 8
B) C3H8O2 = 2, H2SO4 = 8
C) C3H8O2 = 1, H2SO4 = 16
D) C3H8O2 = 3, H2SO4 = 16
E) C3H8O2 = 2, H2SO4 = 4

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 2F2(g) + Mn(s) → 4 F⁻(aq) + Mn2+(aq) F2(g) + e⁻ → 2 F⁻(aq) E° = +2.87 V Mn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V


A) 1.69 V
B) 4.050 V
C) -4.050 V
D) -4.060 V
E) +2.87 V

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. Cu(s) + Mg2+(aq) → Mg(s) + Cu2+(aq) Mg2+(aq) + 2 e⁻ → Mg(s) E° = -2.38 V Cu2+(aq) + 2 e⁻ → Cu(s) E° = +0.34 V


A) +2.04 V
B) -2.04 V
C) +2.72 V
D) -2.72 V
E) -1.36 V

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Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)


A) 1.1 × 1072
B) 8.9 × 10-73
C) 1.1 × 10-72
D) 1.0 × 1024
E) 4.6 × 1031

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Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn2+(aq) + H2(g)


A) H+(aq) ∣ H2(g) ∣ Pt Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn<sup>2+</sup>(aq) + H<sub>2</sub>(g)  A)  H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt   Sn(s)  ∣ Sn<sup>2+</sup>(aq)  B)  H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt   Sn<sup>2+</sup>(aq)  ∣ Sn(s)  C)  Sn<sup>2+</sup>(aq)  ∣ Sn(s)    H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt D)  Sn(s)  ∣ Sn<sup>2+</sup>(aq)    H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt E)  Sn(s)  ∣ H<sub>2</sub>(g)    Sn<sup>2+</sup>(aq)  ∣ H<sup>+</sup>(aq)  ∣ Pt Sn(s) ∣ Sn2+(aq)
B) H2(g) ∣ H+(aq) ∣ Pt Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn<sup>2+</sup>(aq) + H<sub>2</sub>(g)  A)  H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt   Sn(s)  ∣ Sn<sup>2+</sup>(aq)  B)  H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt   Sn<sup>2+</sup>(aq)  ∣ Sn(s)  C)  Sn<sup>2+</sup>(aq)  ∣ Sn(s)    H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt D)  Sn(s)  ∣ Sn<sup>2+</sup>(aq)    H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt E)  Sn(s)  ∣ H<sub>2</sub>(g)    Sn<sup>2+</sup>(aq)  ∣ H<sup>+</sup>(aq)  ∣ Pt Sn2+(aq) ∣ Sn(s)
C) Sn2+(aq) ∣ Sn(s) Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn<sup>2+</sup>(aq) + H<sub>2</sub>(g)  A)  H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt   Sn(s)  ∣ Sn<sup>2+</sup>(aq)  B)  H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt   Sn<sup>2+</sup>(aq)  ∣ Sn(s)  C)  Sn<sup>2+</sup>(aq)  ∣ Sn(s)    H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt D)  Sn(s)  ∣ Sn<sup>2+</sup>(aq)    H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt E)  Sn(s)  ∣ H<sub>2</sub>(g)    Sn<sup>2+</sup>(aq)  ∣ H<sup>+</sup>(aq)  ∣ Pt H2(g) ∣ H+(aq) ∣ Pt
D) Sn(s) ∣ Sn2+(aq) Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn<sup>2+</sup>(aq) + H<sub>2</sub>(g)  A)  H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt   Sn(s)  ∣ Sn<sup>2+</sup>(aq)  B)  H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt   Sn<sup>2+</sup>(aq)  ∣ Sn(s)  C)  Sn<sup>2+</sup>(aq)  ∣ Sn(s)    H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt D)  Sn(s)  ∣ Sn<sup>2+</sup>(aq)    H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt E)  Sn(s)  ∣ H<sub>2</sub>(g)    Sn<sup>2+</sup>(aq)  ∣ H<sup>+</sup>(aq)  ∣ Pt H+(aq) ∣ H2(g) ∣ Pt
E) Sn(s) ∣ H2(g) Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn<sup>2+</sup>(aq) + H<sub>2</sub>(g)  A)  H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt   Sn(s)  ∣ Sn<sup>2+</sup>(aq)  B)  H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt   Sn<sup>2+</sup>(aq)  ∣ Sn(s)  C)  Sn<sup>2+</sup>(aq)  ∣ Sn(s)    H<sub>2</sub>(g)  ∣ H<sup>+</sup>(aq)  ∣ Pt D)  Sn(s)  ∣ Sn<sup>2+</sup>(aq)    H<sup>+</sup>(aq)  ∣ H<sub>2</sub>(g)  ∣ Pt E)  Sn(s)  ∣ H<sub>2</sub>(g)    Sn<sup>2+</sup>(aq)  ∣ H<sup>+</sup>(aq)  ∣ Pt Sn2+(aq) ∣ H+(aq) ∣ Pt

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