Q&A Hero

Q: When a neutron in the nucleus is converted to a proton, which of the following is emitted? A) positron B) beta particle C) alpha particle D) deuteron E) neutron

Q: For which of the following radioactive decay processes does the atomic number not change?A) electron captureB) positron emissionC) alpha emissionD) gamma emissionE) beta emission

Q: When a nucleus undergoes radioactive decay, its new mass number is A) always less than its original mass number. B) never more than its original mass number. C) never less than its original mass number. D) always the same as its original mass number. E) always more than its original mass number.

Q: In the ejection of a beta particle from the nucleus, which of the following occurs? A) A neutron is converted to a proton and an electron. B) A neutron is converted to an electron and an alpha particle. C) A positron is converted to a neutron and a proton. D) A neutron is converted to a positron, an electron, and a gamma ray. E) A proton is converted to a neutron and a positron.

Q: Which of the following nuclear decay processes decreases the nuclear charge? 1) Electron capture 2) Beta emission 3) Positron emission A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1 and 3

Q: Which of the following statements is/are true? 1) Neutrons increase the average distance between protons within the nuclei, potentially leading to a more stable nucleus. 2) Neutrons increase the binding energy of a nucleus without adding electrostatic repulsion, potentially leading to a more stable nucleus. 3) The conversion of a proton to a neutron through beta emission may produce a stable isotope. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: Which of the following nuclides is most likely to be radioactive? A) B) C) D) E)

Q: Which of the following nuclides is most likely to be radioactive? A) B) C) D) E)

Q: A sodium nucleus, , is bombarded with alpha particles to form a radioactive nuclide. This product nuclide can decay by several routes. Which of the following sets of products does not represent a potential route of decay of the product nuclide?A) B) C) D) E)

Q: When the radioactive nuclide undergoes alpha emission, what is the product nuclide?A) B) C) D) E)

Q: When the radioactive nuclide undergoes electron capture, what is the product nuclide?A) B) C) D) E)

Q: When the radioactive nuclide undergoes positron emission, what is the product nuclide?A) B) C) D) E)

Q: The radioactive nuclide, , undergoes decay by emitting a positron. What is the nuclear composition of the product nuclide?A) 12 protons and 10 neutronsB) 11 protons and 11 neutronsC) 11 protons and 10 neutronsD) 9 protons and 12 neutronsE) 10 protons and 12 neutrons

Q: When undergoes beta emission, what is the product nuclide?A) B) C) D) E)

Q: When undergoes electron capture, what is the product nuclide?A) B) C) D) E)

Q: The gamma ray emission from the decay of cobalt-60 is used in cancer therapies. Cobalt-60 decays by the emission of two gamma rays followed by beta emission. What is the final product of this decay process? A) B) C) D) E)

Q: can be prepared by electron capture from which of the following? A) B) C) D) E)

Q: Which of the following statements about 248Bk is incorrect? A) If 248Bk were to undergo spontaneous fission, the products would be 247Bk and a neutron. B) If 248Bk were to undergo beta decay, the products would be 248Cf and a beta particle. C) If 248Bk were to undergo alpha decay, the products would be 244Am and an alpha particle. D) If 248Bk were to undergo electron capture, the only product would be 248Cm. E) If a metastable form of 248Bk were to undergo gamma decay, the products would be 248Bk and a gamma ray.

Q: Which of the following nuclides will produce 243Am upon undergoing alpha decay? A) 247Bk B) 239Np C) 243Pu D) 243Cm E) 244Am

Q: Which of the following nuclides will produce 233Pa upon undergoing alpha decay? A) 234Pa B) 233U C) 229Ra D) 237Np E) 233Th

Q: Which of the following nuclides will produce 192Pt upon undergoing beta decay? A) 192Ir B) 193Pt C) 192Au D) 196Hg E) 188Os

Q: Which particle has the same mass as a beta particle? A) a neutron B) a proton C) a gamma ray D) an alpha particle E) a positron

Q: Which of the following concerning nuclear chemistry is/are correct? 1) Beta particle emission produces a nucleus with one additional neutron and one additional proton. 2) No stable nuclides are known above atomic number 83. 3) In electron capture a proton is converted to a neutron through the capture of an inner orbital electron. A) 1 only B) 2 only C) 3 only D) 2 and 3 E) 1, 2, and 3

Q: Which particle does the nuclide symbol represent?A) helium nucleusB) electronC) positronD) protonE) gamma photon

Q: Electrolysis of a molten salt with the formula MCl, using a current of 3.86 A for 16.2 min, deposits 1.52 g of metal. Identify the metal. (1 faraday = 96,485 coulombs) A) Na B) Li C) Ca D) Rb E) K

Q: A solution of is electrolytically reduced to Mn3+. A current of 7.79 A is passed through the solution for 15.0 min. What is the number of moles of Mn3+produced in this process? (1 faraday = 96,486 coulombs)A) 0.218 molB) 1.61 x10-3 molC) 0.0242 molD) 0.0727 molE) 4.04 x10-4 mol

Q: A current of 15.0 A is passed through molten magnesium chloride for 15.0 h. How many moles of magnesium metal could be produced via this electrolysis? A) 0.0700 mol B) 4.20 mol C) 0.37 mol D) 0.22 mol E) 8.40 mol

Q: What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 160 min using a constant current of 15.0 A? (F= 96485 C/mol)A) 0.431 gB) 25.9 gC) 232.8 gD) 0.187 gE) 38.8 g

Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:2H2O(l)→O2(g) + 4H+(aq) + 4e-How many moles of O2 can be produced from a solution that was electrolyzed for 4.50 h using a current of 5.80 A?A) molB) molC) molD) 0.243 molE) 0.974 mol

Q: How many moles of electrons are produced from a current of 15.6 A in 3.20 h?A) 3.35 molB) 9.33 x103molC) 5.17 x10-4molD) 1.86 molE) 49.9 mol

Q: Copper is electroplated from CuSO4solution. A constant current of 4.39 A is applied by an external power supply. How long will it take to deposit 1.00 102g of Cu? The atomic mass of copper is 63.546. A) 19.2 h B) 13.17 s C) 1.48 days D) 9.6 min E) 2.74 h

Q: Gold (atomic mass = 197) is plated from a solution of chlorauric acid, HAuCl4; it deposits on the cathode. Calculate the time it takes to deposit 0.64 g of gold, passing a current of 0.10 A. (1 faraday = 96,485 coulombs) A) 54 min B) 0.87 h C) 0.29 h D) 2.6 h E) none of these

Q: If an electrolysis plant operates its electrolytic cells at a total current of 1.0 x106 A, how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs)A) 66 minB) 0.55 yearC) 2.2 hD) 2.2 daysE) 1.1 h

Q: How many faradays are required to convert a mole of AsO3-ions to AsH4+ions?A) 4B) 7C) 8D) 6E) 5

Q: How many faradays are involved in the conversion of a mole of to ? A) 5 B) 1 C) 2 D) 3 E) 4

Q: When Au is obtained by electrolysis from NaAu(CN)2, what is the minimum number of coulombs required to produce 1.06 mol of gold? A) C B) C C) C D) C E) C

Q: Which of the following statements is true concerning the electrolysis of a 1.0 M aqueous solution of NaI? Reduction Half-ReactionEº(V)Na+(aq) + e- Na(s)-2.712H2O(l) + 2e- H2(g) + 2OH-(aq)-0.832H+(aq) + 2e- H2(g)0.00I2(s) + 2e- 2I-(aq)0.54O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23A) The solution becomes more basic.B) Sodium is deposited at the cathode.C) Iodine is formed at the cathode.D) Oxygen is evolved at the anode.E) Hydrogen is evolved at the anode.

Q: What reaction occurs at the anode during the electrolysis of aqueous CuSO4? Reduction Half-ReactionEº(V)2H2O(l) + 2e- H2(g) + 2OH-(aq)-0.832H+(aq) + 2e- H2(g)0.00Cu2+(aq) + 2e- Cu(s)0.34O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23A) 2H2O(l) →O2(g) + 4H+(aq) + 4e-B) Cu(s) →Cu2+(aq) + 2e-C) 2H2O(l) + 2e-→H2(g) + 2OH-(aq)D) Cu2+(aq) + 2e-→Cu(s)E) 2H+(aq) + 2e-→H2(g)

Q: When an aqueous solution of AgNO3 is electrolyzed, a gas is formed at the anode. What is the identity of the gas? Reduction Half-ReactionEº(V)2H2O(l) + 2e- H2(g) + 2OH-(aq)-0.832H+(aq) + 2e- H2(g)0.00Ag+(aq) + e- Ag(s)0.80NO3-(aq) + 4H+(aq) + 3e- NO(g) + 2H2O(l)0.96O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23A) H2OB) NOC) AgD) O2E) H2

Q: When an aqueous solution of lithium sulfate is electrolyzed, what are the expected products? Reduction Half-ReactionEº(V)Li(s)-3.042H2O(l) + 2e- H2(g) + 2OH-(aq)-0.832H+(aq) + 2e- H2(g)0.00O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23S2O82-(aq) + 2e- 2SO42-(aq)2.01A) Li(s) and H2(g)B) H2(g), OH-(aq), O2(g), and H+(aq)C) O2(g), H+(aq), and Li(s)D) H2(g), OH-aq), and Li(s)E) H2(g), OH-(aq), and S2O82-(aq)

Q: What is the half-reaction that occurs at the cathode during electrolysis of an aqueous potassium iodide solution? Reduction Half-ReactionEº(V)K+(aq) + e- K(s)-2.93Mg2+(aq) + 2e- Mg(s)-2.372H2O(l) + 2e- H2(g) + 2OH-(aq)-0.832H+(aq) + 2e- H2(g)0.00I2(s) + 2e- 2I-(aq)0.54O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23A) H2O(l) → O2(g) + 2H+(aq) + 2e-B) 2H2O(l) + 2e-→H2(g) + 2OH-(aq)C) K(s) → K+(aq) + e-D) K+(aq) + e-→K(s)E) I2(aq) + 2e-→2I-(aq)

Q: What is one of the major products in the electrolysis of a saturated aqueous sodium chloride solution? Reduction Half-ReactionEº(V)Na+(aq) + e- Na(s)-2.71Mg2+(aq) + 2e- Mg(s)-2.372H2O(l) + 2e- H2(g) + 2OH-(aq)-0.83O2(g) + 4H+(aq) + 4e- 2H2O(l)1.23Cl2(g) + 2e- 2Cl-(aq)1.36A) MgB) O2C) H2OD) NaE) Cl2

Q: Molten magnesium chloride is electrolyzed using inert electrodes and reactions represented by the following two half-reactions:2Cl-(l)→Cl2(g) + 2e-Mg2+(l) + 2e- →Mg(s)Concerning this electrolysis, which of the following statements is true?A) The anions in the electrolyte undergo reduction.B) Mg2+ions are reduced at the anode.C) Oxidation occurs at the cathode.D) Electrons pass through the metallic part of the circuit from Mg2+ions to the Cl-ion.E) Cl-ions are reducing agents.

Q: What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?A) K(s)→K+(l) + e-B) Br2(l) + 2e- → 2Br-(l)C) 2Br-(l)→Br2(l) + 2e-D) K+(l) + e- → K(s)E) 2H2O(l) + 2e- → H2(g) + 2OH-(l)

Q: Protection of iron (Eº(Fe2+/Fe) = -.23 V; (Eº(Fe3+/Fe) = -0.04 V) from corrosion can be accomplished by making an electrical contact between iron and certain other metals. Metal(s) that would provide protection is(are)1) Mg (Eº= -.38 V).2) Ni (Eº= -.23 V).3) Zn (Eº= -.76 V).4) Pb(Eº= -.13 V).A) 1 onlyB) 4 onlyC) 1 and 3D) 2 and 4E) 3 and 4

Q: Cathodic protection results when A) iron is amalgamated with mercury. B) iron is made amphoteric. C) iron is painted to protect it from corrosion. D) iron is tin-plated for use as a tin can. E) iron is attached to a more active metal.

Q: A piece of iron half-immersed in a sodium chloride solution will corrode more rapidly than a piece of iron half-immersed in pure water, because A) the ions, which are not present in pure water, balance the accumulation of charge in each of the half-cells. B) the chloride ions increase the pH of the solution. C) the sodium ions oxidize the iron atoms. D) the chloride ions form a precipitate with iron. E) the chloride ions oxidize the iron atoms.

Q: Which of the following statements about batteries is false? A) A fuel cell is a galvanic cell for which the reactants are continuously supplied. B) Lithium"iodine batteries have low current, but extremely long life. C) Lead storage batteries contain lead at the anode and lead coated with lead dioxide at the cathode. D) It is not safe to recharge a nickel"cadmium battery. E) Dry cell batteries are used in flashlights and portable radios.

Q: Which of the following statements is true concerning the electrochemical cell described below at 25oC?Ni | || | NiA) The cell reaction is spontaneous with a cell potential of 20.8 mV.B) The cell reaction is nonspontaneous with a cell potential of -0.23 V.C) The cell reaction is nonspontaneous with a cell potential of -10.6 mV.D) The cell reaction is spontaneous with a cell potential of 10.6 mV.E) The cell reaction is nonspontaneous with a cell potential of -20.8 mV.

Q: In order to determine the identity of a particular lanthanide metal (M), a voltaic cell is constructed at 25ºC with the anode consisting of the lanthanide metal as the electrode immersed in a solution of 0.0873 M MCl3, and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3)2 solution. The two half-reactions are as follows:M(s) M3+(aq) + 3e-Cu2+(aq) + 2e- Cu(s)The potential measured across the cell is 2.68 V. What is the identity of the metal? Reduction Half-ReactionEº(V)Cu2+(aq) + 2e- Cu(s)0.34Ce3+(aq) + 3e- Ce(s)-2.336Tm3+(aq) + 3e- Tm(s)-2.319Eu3+(aq) + 3e- Eu(s)-1.991Gd3+(aq) + 3e- Gd(s)-2.279Sm3+(aq) + 3e- Sm(s)-2.304A) SmB) GdC) TmD) EuE) Ce

Q: What is the reduction potential for the half-reaction Al3+(aq) + 3e- Al(s) at 25ºC if [Al3+] = 0.44 M and Eº= -1.66 V?A) -1.66 VB) -1.65 VC) -1.84 VD) -1.72 VE) -1.67 V

Q: In order to determine the identity of a particular transition metal (M), a voltaic cell is constructed at 25ºC with the anode consisting of the transition metal as the electrode immersed in a solution of 0.0977 M M(NO3)2, and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3)2 solution. The two half-reactions are as follows:M(s) M2+(aq) + 2e-Cu2+(aq) + 2e- Cu(s)The potential measured across the cell is 0.77 V. What is the identity of the metal M? Reduction Half-ReactionEº(V)Cu2+(aq) + 2e- Cu(s)+0.34Ni2+(aq) + 2e- Ni(s)-0.23Cd2+(aq) + 2e- Cd(s)-0.40Zn2+(aq) + 2e- Zn(s)-0.76Mn2+(aq) + 2e- Mn(s)-1.18A) CdB) NiC) CuD) MnE) Zn

Q: The following cell is initially at standard-state conditions. Which of the following statements is true after the cell is allowed to discharge (do work) for a period of time?Zn2+(aq) + 2e- Zn(s); E= -0.76 VCu2+(aq) + 2e- Cu(s); E= 0.34 VA) Initially Eºcell= - 1.10 V, and it will become more negative with time.B) Eºcell does not change with time.C) Initially Eºcell= - 1.10 V, and it will become more positive with time.D) Initially Eºcell= + 1.10 V, and it will become more negative with time.E) Initially Eºcell= + 1.10 V, and it will becomes more positive with time.

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+concentration is 2.5 x10-5 M and by placing a Pt electrode in the other compartment, in which the H+concentration is 3.70 M and = 1.00 atm. The Fe2+/Fe half-cell reduction potential is -0.41 V, and the H+/H2 half-cell reduction potential is 0.00 V. What is Eº for the cell at 25oC?A) 0.10 VB) 0.58 VC) 0.27 VD) 0.24 VE) 0.56 V

Q: A cell consists of a magnesium electrode immersed in a solution of magnesium chloride and a silver electrode immersed in a solution of silver nitrate. The two half-cells are connected by means of a salt bridge. It is possible to increase the voltage of the cell byA) decreasing the concentration of Mg2+vand increasing the concentration of Ag+.B) adding sodium chloride to both half-cells.C) increasing the size of the Mg electrode and decreasing the size of the Ag electrode.D) decreasing the size of the Mg electrode and increasing the size of the Ag electrode.E) increasing the concentration of Mg2+.

Q: Given:What is the cell potential at 25ºC for the following cell?Cr(s) | Cr3+(0.010 M) || Ag+(0.00020 M) | Ag(s)A) 0.95 VB) 2.09 VC) 1.51 VD) 1.36 VE) 1.72 V

Q: What is the value of the reaction quotient, Q, for the voltaic cell constructed from the following two half-reactions when the Zn2+ concentration is 0.0120 M and the Ag+ concentration is 1.31 M?A) 9.16 x10-3B) 6.99 x10-3C) 109D) 1.25 x10-2E) 143

Q: For the cell the standard cell potential is 0.46 V. A cell using these reagents was made, and the observed potential was 0.31 V at 25oC. What is a possible explanation for the observed voltage? A) The volume of the solution was larger than the volume of the Ag+solution. B) The volume of the Ag+solution was larger than the volume of the solution. C) The concentration was larger than the Ag+concentration. D) The Ag electrode was twice as large as the Cu electrode. E) The Ag+concentration was larger than the concentration.

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 x10-5 M and by placing a Pt electrode in the other compartment, in which the H+ concentration is 3.4 M and = 1.00 atm. The Fe2+/Fe half-cell reduction potential is -0.41 V, and the H+/H2 half-cell reduction potential is 0.00 V. What is E for the cell at equilibrium?A) -0.41 VB) 0.41 VC) 0.69 VD) 0.00 VE) 0.28 V

Q: Given:Zn2+(aq) + 2e- Zn(s); Eº= -0.76 VCu2+(aq) + 2e- Cu(s); Eº= 0.34 VWhat is the cell potential of the following electrochemical cell at 25ºC?Zn(s) | Zn2+(1.0 M) || Cu2+(0.0010 M) | Cu(s)A) between 0.34 and 0.76 VB) less than 0.42 VC) between 0.00 and 0.76 VD) between 0.76 and 1.10 VE) greater than 1.10 V

Q: What is the copper(II)-ion concentration at 25ºC in the cell Zn(s) | Zn2+(1.0 M) || Cu2+(aq) | Cu(s) if the measured cell potential is 1.01 V? The standard cell potential is 1.10 V.A) 0.030 MB) 0.99 MC) 0.00091 MD) 1.0 ME) 0.99 M

Q: For the cell reaction2MnO4-(aq) + 5H2SO3(aq) → 2Mn2+(aq) + 5SO42-(aq) + 4H+(aq) + 3H2O(l)the standard cell potential is 1.34 V. Which change(s) will result in an increase in the cell potential?1) increasing the permanganate-ion concentration2) decreasing the pH3) increasing the sulfurous acid concentrationA) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 2E) 1 and 3

Q: For the cell reactionl)the standard cell potential is 1.34 V. To determine the cell potential at nonstandard conditions, what is the value that should be used for n in the Nernst equation?A) 8B) 10C) 5D) 2E) 6

Q: What is Eof the following cell reaction at 25ºC? Eºcell= 0.460 V.A) 0.468 VB) 0.282 VC) 0.460 VD) 0.490 VE) 0.479 V

Q: If the cell is initially at standard-state conditions, which of the following statements is true?Zn2+(aq) + 2e" Zn(s); Eº= "0.76 VCu2+(aq) + 2e" Cu(s); Eº= 0.34 VA) Initially Kc= 2 x10"37, and it decreases with time.B) Initially Kc= 2 x1037, and it does not change with time.C) Initially Kc= 2 x1037, and it decreases with time.D) Initially Kc= 2 x1037, and it increases with time.E) Initially Kc= 2 x10"37, and it increases with time.

Q: The cell potential of the following cell is determined using an unspecified concentration of acid. What is the pH of the acid solution given that the measured cell potential is -0.562 V and the anode reduction potential (Eº) is 0.222 V at 25ºC?Ag(s) | AgCl(s) | Cl-(1.0 M) || H+(aq, ?M) | H2(g, 1.0 atm) | Pt(s)A) 5.74B) 13.2C) 6.24D) 11.5E) 1.26

Q: The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H+] given that the measured cell potential is "0.366 V and the anode reduction potential (Eº) is 0.222 V at 25ºC?Ag(s) | AgCl(s) | Cl-(1.0 M) || H+(aq, ?M) | H2(g, 1.0 atm) | Pt(s)A) MB) MC) MD) ME) M

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the concentration is 2.0 x10-5M and by placing a Pt electrode in the other compartment, in which the H+concentration is 3.4 M and PH2= 1.00 atm. The /Fe half-cell reduction potential is -0.41 V, and the H+/H2 half-cell reduction potential is 0.00 V. What is the equilibrium constant at 25ºC for the spontaneous cell reaction?A) 4 x104B) 5 x1020C) 5 x1022D) E)

Q: Calculate the solubility product of silver iodide at 25ºC given the following data: Eº(V)AgI(s) + e-→Ag(s) + I- -0.15I2(s) + 2e-→2I- +0.54Ag++ e-→Ag(s) +0.80A) 2 x10-12B) 3 x10-3C) 2 x10-24D) 9 x10-17E) 2 x10-4

Q: What is the equilibrium constant (K) at 25ºC for the following cell reaction?A) 0.010B) 1.5C) 0.25D) 1.0E) 2.2

Q: What is the logarithm of the equilibrium constant, log K, at 25ºC of the voltaic cell constructed from the following two half-reactions?Ag+(aq) + e-Ag(s); Eº= 0.80 VA) 6.7B) 40.6C) 20.3D) 13.5E) 67.6

Q: For a certain reaction, kJ and J/K. If , calculate Eºcell for the reaction at 25ºC.A) 0.0164 VB) 0.0961 VC) 0.346 VD) 0.736 VE) 0.0654 V

Q: If Eºcell for a certain reaction is "1.68 V (n= 1), and Sº is 31.1 J/(K·mol), what is Hº in units of J/mol at 25ºC?A) J/molB) J/molC) J/molD) J/molE) J/mol

Q: For a reaction in a voltaic cell, both Hº and Sº are positive. Which of the following statements is true?A) Eºcell will increase with an increase in temperature.B) Eºcell will not change when the temperature increases.C) Eºcell will decrease with an increase in temperature.D) Gº> 0 for all temperatures.E) None of the above statements is true.

Q: Calculate the maximum electrical work obtainable at 25oC from the following voltaic cell. A) B) C) D) E)

Q: Given: What is the standard Gibbs free-energy change for the following reaction? A) B) C) D) E)

Q: Given: What is for the following cell reaction? 2AlCl3(aq) 2Al(s) + 3Cl2(g) A) B) C) D) E)

Q: If the cell is initially at standard-state conditions, which of the following statements is true?Zn2+(aq) + 2e- Zn(s); Eº= -0.76 VCu2+(aq) + 2e- Cu(s); Eº= 0.34 VA) Initially , and it will become more positive with time.B) Initially , and it will not change with time.C) Initially , and it will become more negative with time.D) Initially , and it will become more positive with time.E) Initially , and it will become more negative with time.

Q: Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals)M1 | M12+(aq) || M2+(aq) | M2M12+(aq) + 2e- M1(s); Eº= -2.38 VM22+(aq) + e- M2(s); Eº= -2.98 VA) The cell reaction is nonspontaneous with a standard cell potential of .B) The cell reaction is spontaneous with a standard cell potential of .C) The cell is at equilibrium.D) The cell reaction is spontaneous with a standard cell potential of .E) The cell reaction is nonspontaneous with a standard cell potential of .

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 x10"5M and by placing a Pt electrode in the other compartment, in which the H+ concentration is 3.4 M and = 1.00 atm. The Fe2+/Fe half-cell reduction potential is -0.41 V, and the H+/H2 half-cell reduction potential is 0.00 V. What is the value of Eº for this cell, and which electrode is the anode?A) 0.41 V, FeB) 0.90 V, PtC) -0.41 V, PtD) -0.41 V, FeE) 0.41 V, Pt