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Stack #1420987
| Question | Answer |
|---|---|
| 1) Identify oxidation. | E) both A and B |
| 2) What element is being reduced in the following redox reaction? MnO4⁻ (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g) | C) Mn |
| 3) What element is being oxidized in the following redox reaction? MnO4⁻ (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g) | A) C |
| 4) What element is being oxidized in the following redox reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3⁻(aq) | B) N |
| 5) What element is being reduced in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g) | C) Cl |
| 6) What element is being oxidized in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g) | B) O |
| 7) What element is being oxidized in the following redox reaction? Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq) | A) Cr |
| 8) What element is being reduced in the following redox reaction? Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq) | D) Cl |
| 9) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻ (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g) | A) H2C2O4 = 5, H2O = 8 |
| 10) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq) + MnO4⁻(aq) → Fe3+(aq) + Mn2+(aq) | B) H⁺ = 8, Fe3+ = 5 |
| 11) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq) + NH4+(aq) → Zn(s) + NO3⁻(aq) | C) Zn = 4, H⁺ = 10 |
| 12) Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag+ in the balanced reaction? Cd(s) + Ag+(aq) → Ag(s) + Cd2+(aq) | A) Cd = 1, Ag⁺ = 2 |
| 13) Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br2 and OH⁻ in the balanced reaction? Br2(l) → BrO3⁻(aq) + Br⁻(aq) | D) Br2 = 3, OH⁻ = 6 |
| 14) Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of ClO2 and H2O in the balanced reaction? H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g) | E) ClO2 = 2, H2O = 2 |
| 15) Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4⁻ and ClO⁻ in the balanced reaction? Cr(OH)4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq) | A) Cr(OH)4⁻ = 2, ClO⁻ = 3 |
| 16) Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Al and F2 in the balanced reaction? Al(s) + F2(g)→ Al3+(aq) + F-(aq) | A) Al = 2, F2 = 3 |
| 17) Identify the location of oxidation in an electrochemical cell. | A) the anode |
| 18) Identify the location of reduction in an electrochemical cell. | B) the cathode |
| 19) Define a salt bridge. | E) A pathway by which counterions can flow between the half-cells without the solutions in the half-cell totally mixing. |
| 20) Determine the redox reaction represented by the following cell notation. Mg(s) ∣ Mg2+(aq) Cu2+(aq) ∣ Cu(s) | B) Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) |
| 21) Determine the cell notation for the redox reaction given below. Sn(s) + 2 Ag⁺(aq) → Sn2+(aq) + 2 Ag(s) | C) Sn(s) ∣ Sn2+(aq) Ag+(aq) ∣ Ag(s) |
| 22) Determine the cell notation for the redox reaction given below. Pb(s) + 2 H⁺(aq) → Pb2+(aq) + H2(g) | D) Pb(s) ∣ Pb2+(aq) H+(aq) ∣ H2(g) ∣ Pt |
| 23) Determine the cell notation for the redox reaction given below. 3 Cl2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe3+(aq) | E) Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt |
| 24) What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni2+(aq) Ag+(aq) ∣ Ag(s) | A) Ni(s) |
| 25) What is the oxidizing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni2+(aq) Ag+(aq) ∣ Ag(s) | C) Ag+(aq) |
| 26) What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn2+(aq) Ag+(aq) ∣ Ag(s) | B) Ag+(aq) |
| 27) What is the reducing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn2+(aq) Ag+(aq) ∣ Ag(s) | A) Sn(s) |
| 28) What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt | C) Cl2(g) |
| 29) What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt | A) Fe(s) |
| 30) What is undergoing oxidation in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb2+(aq) H+(aq) ∣ H2(g) ∣ Pt | D) Pb(s) |
| 31) What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb2+(aq) H+(aq) ∣ H2(g) ∣ Pt | B) H+(aq) |
| 32) What statement is NOT true about standard electrode potentials? | D) E°cell is the difference in voltage between the anode and the cathode. |
| 33) Which of the following is the strongest reducing agent? | D) Cr(s) E) Li(s) C) Mg(s) |
| 34) Which of the following is the weakest oxidizing agent? | D) Cr(s D) I2(s) |
| 1) Q = 1 | C) Ecell = E°cell |
| 2) Q > K | A) Ecell < 0 |
| 37) Which of the following is the weakest reducing agent? | B) Zn(s) B) Au3+(aq) |
| 38) Which of the following is the strongest oxidizing agent? | E) MnO4⁻(aq) B) Au3+(aq) A) H2O2(aq) |
| 3) Q < K | D) Ecell > 0 |
| 4) ΔG° < 0 | B) E°cell > 0 |
| 5) ΔG° > 0 | F) E°cell < 0 |
| 6) Q = K | E) Ecell = 0 |
| 43) 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 | E) +1.40 V |
| 44) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq) Pb2+(aq) + 2 e⁻ → Pb(s) E° = -0.13 V Br2(l) + 2 e⁻ → 2 Br⁻(aq) E° = +1.07 V | A) +1.20 V |
| 45) Sn(s) + 2 Ag⁺(aq) → Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e⁻ → Sn(s) E° = -0.14 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V | B) +0.94 V |
| 46) 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 | C) +2.72 V |
| 47) 2 K(s) + I2(s) → 2 K⁺(aq) + 2 I⁻(aq) K+(aq) + e⁻ → K (s) E° = -2.93 V I2(s) + 2 e⁻ → 2 I⁻(aq) E° = +0.54 V | D) +3.47 V |
| 48) Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. | D) Fe3+(aq) + Ni(s) |
| 49) Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. | A) Sn4+(aq) + Mg(s) |
| 50) Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. | B) Ca(s) + Mg2+(aq) |
| 51) Which of the following metals will dissolve in nitric acid but not hydrochloric? | C) Cu |
| 52) Which of the following metals will dissolve in nitric acid but not hydrochloric? | D) Ag |
| 53) Which of the following metals will dissolve in HCl? | E) all of the above |
| 54) Which of the following metals will not dissolve in nitric acid or hydrochloric acid? | D) Au |
| 55) Which of the following metals will not dissolve in nitric acid or hydrochloric acid? | E) none of the above |
| 56) Identify the characteristics of a spontaneous reaction. | D) all of the above |
| 57) How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Mg(s) + Al3+(aq) → Al(s) + Mg2+(aq) | A) 6 |
| 58) How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Fe2+(aq) + K(s) → Fe(s) + K+(aq) | B) 2 |
| 59) How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq) | C) 6 |
| 60) Which of the following reactions would have the smallest value of K at 298 K? | C) A + B → 2 C; E°cell = -0.030 V |
| 61) Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) | D) +91 kJ |
| 62) Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) | E) -3.3 x 102 kJ |
| 63) Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) | A) +4.1 x 102 kJ |
| 64) Which of the following reactions would be the most spontaneous at 298 K? | D) A + B → C; E°cell = +1.22 V |
| 65) 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) | C) 1.1 x 10-72 |
| 66) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) | C) 2.4 × 1058 |
| 67) Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) | D) 1.3 × 10-16 |
| 68) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ∣ Sn2+(aq, 1.8 M) Ag+(aq, 0.055 M) ∣ Ag(s) | E) +0.86 V |
| 69) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ∣ Sn2+(aq, 0.022 M) Ag+(aq, 2.7 M) ∣ Ag(s) | A) +1.01 V |
| 70) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 2.74 M) Cu2+(aq, 0.0033 M) ∣ Cu(s) | B) +2.62 V |
| 71) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Fe(s) ∣ Fe3+(aq, 0.0011 M) Fe3+(aq, 2.33 M) ∣ Fe(s) | A) +0.066 V |
| 72) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ∣ Cu2+(aq, 0.0032 M) Cu2+(aq, 4.48 M) ∣ Cu(s) | B) +0.093 V |
| 73) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s) ∣ Al3+(aq, 0.115 M) Al3+(aq, 3.89 M) ∣ Al(s) | E) +0.030 V |
| 74) Identify the battery that is in most automobiles. | C) lead-acid storage battery |
| 75) Identify the battery that is used as a common flashlight battery. | A) dry-cell battery |
| 76) Identify the components of a fuel cell. | C) hydrogen-oxygen |
| 77) Identify the battery type that has a high overcharge tolerance. | D) lead storage |
| 78) What is the reaction at the anode in a breathalyzer? | A) Ethanol is oxidized to acetic acid. |
| 79) What is the reaction at the cathode in a breathalyzer? | C) Oxygen is reduced. |
| 80) Describe how water can be a good conductor of current. | C) add salt |
| 81) 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 |
| 82) What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current? | B) 24.5 g |
| 83) Nickel can be plated from aqueous solution according to the following half reaction. How long would it take (in min) to plate 29.6 g of nickel at 4.7 A? Ni2+(aq) + 2 e⁻ → Ni(s) | C) 3.5 × 102 min |
| 84) Identify a component in the formation of rust. | D) all of the above |
| 85) Predict the species that will be reduced first if the following mixture of molten salts undergoes electrolysis. Na+, Ca2+, Cl⁻, Br⁻, F⁻ | A) Na⁺ |
| 86) Predict the species that will be reduced first if the following mixture of molten salts undergoes electrolysis. Zn2+, Fe3+, Mg2+, Br-, I- | D) Fe3+ |
| 87) Predict the species that will be oxidized first if the following mixture of molten salts undergoes electrolysis. Cu2+, Mg2+, Cl⁻, Br⁻, F⁻ | E) Br⁻ |
| 1) What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq) + 2 Ag(s) → Co(s) + 2 Ag+(aq) | C) Co2+(aq) + 2 e- → Co(s) |
| 2) What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO3)2(aq) → Pb(NO3)2(aq) + Cu(s) | A) Pb(s) ∣ Pb2+(aq) ∣∣ Cu2+(aq) ∣ Cu(s) |
| 3) What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe2+(aq) + F2(g) → 2 Fe3+(aq) + 2 F-(aq) | D) Pt(s) ∣ Fe2+(aq), Fe3+(aq) ∣∣ F2(g) ∣ F-(aq) ∣ C(s) |
| 4) For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn2+(aq) ∣∣ Ni2+(aq) ∣ Ni(s) | D) Ni2+(aq) + 2 e- → Ni(s) |
| 5) What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s) ∣ Al3+(aq) ∣∣ Fe2+(aq) ∣ Fe(s) | A) 2 Al(s) + 3 Fe2+(aq) → 2 Al3+(aq) + 3 Fe(s) |
| 6) What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?. Ni(s) ∣ Ni2+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) | B) Ni(s) + Cl2(g) → Ni2+(aq) + 2 Cl-(aq) |
| 7) 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 | A) - 0.26 V |
| 8) 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 V Cu2+(aq) + 2 | B) Ag(s) is formed at the cathode, and Cu2+(aq) is formed at the anode. |
| 9) Consider the following standard reduction potentials, Ni2+(aq) + 2 e- → Ni(s) E° = - 0.26 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions, | B) I2(s) is a stronger oxidizing agent than Ni2+(aq) and Ni(s) is a stronger reducing agent than I-(aq). |
| 10) 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 increase (i.e., become more positive)? | B) increase the [ Pb2+] concentration |
| 11) Based on the following information, Cl2(g) + 2 e- → 2 Cl-(aq) E° = + 1.36 V Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V which of the following chemical species is the strongest reducing agent? | D) Mg(s) |
| 12) Using the following standard reduction potentials, Fe3+(aq) + e- →Fe2+(aq) E° = +0. 77 V Ni2+(aq) + 2 e- →Ni(s) E° = -0.23 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this r | A) E° = - 1.00 V, nonspontaneous |
| 13) The gas OF2 can be produced from the electrolysis of an aqueous solution of KF, as shown in the equation below. OF2(g) + 2 H+(aq) + 4 e- → H2O(l) + 2 F-(aq) E° = +2.15 V Using the given standard reduction potential, calculate the amount of OF2 that | A) 6.48 g of OF2 at the anode. |
| 14) Given that E°red = -1.66 V for Al3+/ Al at 25°C, find E° and E for the concentration cell expressed using shorthand notation below. Al(s) ∣ Al3+(1.0 × 10-5 M) ∣∣ Al3+(0.100 M) ∣ Al(s) | B) E° = 0.00 V and E = +0.12 V |
| 15) The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.66 V. The concentration of H+ in th | A) 2.0 × 10-2 |
| 16) 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 0.0222 M and 2.22 M, respect | B) 0.118 |
| 17) A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M, respectively. The cell emf is _____ | C) 0.0798 |
| 18) The standard emf for the cell using the overall cell reaction below is +2.20 V: 2 Al (s) + 3 I2 (s) → 2 Al3+ (aq) + 6 I- (aq) The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [I-] = 0.15 M is __________ V. | B) 2.32 |
| 19) The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn (s) + Ni2+ (aq) → Zn2+ (aq) + Ni (s) The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is __________ V. | C) 0.52 |
| 20) The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces __________ g of aluminum metal. | D) 16.4 |
| 21) 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 mol es of Cr2O72-? | C) 9 |
| 22) How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V? | D) 29.8 |
| 23) The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al2O3 · xH2O. The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is __________ when the | E) 59.6 |
| 24) How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl3 with an electrical current of 12.0 A? | E) 3.57 × 103 |
| 25) 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 |
| 26) 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? | B) 16.4 g |
| 27) 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? | D) 5.36 hours |
| 28) The town of Natrium, West Virginia, derives its name from the sodium produced in the electrolysis of molten sodium chloride (NaCl) mined from ancient salt deposits. The number of kilowatt-hours of electricity required to produce 4.60 kg of metallic s | A) 24.1 |
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