Why is the standard reduction potential E, for the standard hydrogen electrode 0.00V? Please help me explain the reason why to this problem

21,369 results
  1. Chemistry

    Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl−(aq) | Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard

  2. chemistry

    Given these standard reduction potentials at 25oC: Cr3+ + e- -> Cr2+ (E1^o = -0.407V) Cr2+ + 2e- -> Cr(s) (E2^o = -0.913V) Determine the standard reduction potential at 25oC for the half-reaction equation: Cr3+ + 3e- -> Cr(s) This seems like a really

  3. Chemistry

    Based on the standard reduction potentials given below, which species is most likely to be oxidized? Ag+ + e- → Ag, Eo= 0.80 V Cu2+ + 2e- → Cu, Eo= 0.34 V Zn2+ + 2e- → Zn, Eo= -0.76 V Cd2+ + 2e- → Cd, Eo= -0.40 V I thought the answer would be Zn2+

  4. Chemistry

    What would the potential of a standard hydrogen (S.H.E.) electrode be if it was under the following conditions? [H+] = 0.38 P(H2) = 3.8 T = 298 K

  5. Chemistry

    1. Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. A standard reduction potential graph for the

  6. Chem

    Calculate the standard cell potential given the following standard reduction potentials: Al3++3e−→Al;E∘=−1.66 V Fe2++2e−→Fe;E∘=−0.440 V

  7. chemistry

    (AAAAA)The standard reduction potentials of lithium metal and chlorine gas are as follows: (for Li, reduction potential is -3.04, for Cl it is 1.36) In a galvanic cell, the two half-reactions combine to 2Li{+](s) + Cl{-}2(g) --> 2Li{+}Cl{-}(aq) Calculate

  8. CHEMISTRY

    The standard electrode potential for the reduction of Eu3+(aq) to Eu2+(aq) is −0.43 V. determine which of the following is capable of reducing Eu3+(aq) to Eu2+(aq) under standard-state conditions? (a) Sn2+(aq) (b) ln(s) (c) HCN(aq) (d) La(s)

  9. chemistry

    A. What is the standard potential, in volts, of a galvanic cell made of Ce4+ and Cu2+, given the standard reduction potentials below? Ce4+ + e− → Ce3+ Eº = 1.61 V Cu2+ + 2e− → Cu(s) Eº = 0.34 V I think it is 1.27 V but it might be 1.95V b. How

  10. Chemistry

    Consider the following cell: Pt|H2(g, 0.460 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.00 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion

  11. Electrochemistry

    In lab, we did an experiment with electrochemical cells with solutions of ZnSO4, CuSO4, Al2(SO4)3 and MgSO4 and their respective metal electrodes. There are a couple of post-lab questions that I'm not sure about: (1) Summarize Part A with a data table

  12. College Chemistry

    A Galvanic cell consists of Mg electrode in a 1.0 mol L -1 Mg(NO3)2 solution and a Ag electrode in a 1.0 mol L-1 AgNO3 solution. Calculate standard emf for the spontaneous reaction of this electrochemical cell at 25 C, given that the standard reduction

  13. Chemistry

    A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of fold in a 1.0 M gold (III) ion solution connected by a salt bridge. Calculate the standard potential for this cell at

  14. Chemistry

    Why are standard electrode potentials affected by the nature of the electrode?

  15. Chemistry

    Calculate the standard electrode potential for the reaction Cr2+ +3e=Cr(E=-0.74V Cr3+ +e-=Cr2+(E=-0.41V)

  16. Chemistry

    1) Assume that the reference half-cell is changed to a standard mercury-mercury (II) half-cell. a) What would be the reduction potential of a standard chlorine half-cell. c) What would be the cell potential of a standard chlorine-nickel cell. 2) For each

  17. Analytic Chemistry

    At 25 °C, you conduct a titration of 15.00 mL of a 0.0260 M AgNO3 solution with a 0.0130 M NaI solution within the following cell: Saturated Calomel Electrode || Titration Solution | Ag (s) For the cell as written, what is the voltage after the addition

  18. Chemistry (Electrochemistry)

    The standard potential for the following galvanic cell is 1.72V : Be(s)|Be2+(aq)||Pb2+(aq)|Pb(s) The standard reduction potential for the Pb2+/Pb half-cell: E = -.13V Calculate the standard reduction potential for the Be2+/Be half-cell. What I know: Be is

  19. chemistry

    Why is the standard reduction potential E, for the standard hydrogen electrode 0.00V? Please help me explain the reason why to this problem

  20. chemistry

    To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.124V V ? (Assume that the partial pressure of hydrogen gas remains at 1 atm.)

  21. Chemistry

    Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2 ] = 0.842 M and [Ni2 ] = 0.0100 M. Standard reduction potentials can be found here. reaction: Zn(s)+Ni^2+(aq)--->Zn^2+(aq)+Ni(s) standard reduction Zn: -.76

  22. Biochem

    5. The glass electrode used in commercial pH meters gives an electrical response proportional to the concentration of hydrogen ion. To convert these responses to a pH reading, the electrode must be calibrated against standard solutions of known H+

  23. AP Chemistry!!!

    Explain the reaction that would occur in a galvanic cell between solutions of Al3+ and Pb2+. Identify the oxidation and reduction reactions and the location of each reaction. Then, use the standard reduction potential tables to determine the cell

  24. Chemistry

    Explain the reaction that would occur in a galvanic cell between solutions of Al3+ and Pb2+. Identify the oxidation and reduction reactions and the location of each reaction. Then, use the standard reduction potential tables to determine the cell

  25. chem

    Q: Calculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible

  26. chemistry

    how do you find the standard electrode potentials of KMnO4 and MnCl2? and is the standard electrode potential of MnO2 1.28?

  27. Chemistry

    The Ksp value for PbS(s) is 8.0x10^-28. By using this value with an electrode potential from Appendix E in the textbook, determine the value of the standard reduction potential for the reaction: PbS(s) + 2e- --> Pb(s) + S2- (aq)

  28. Chemistry

    Suppose a galvanic cell contains one nickel electrode and one copper electrode. At 25°C, nickel has a negative reduction potential and copper has a positive reduction potential. At which electrode will reduction occur? Explain. I believe the copper will

  29. Chemistry: Please check answers

    12. What balances charges that may build up as reduction and oxidation occur in a voltaic cell? *the salt bridge one of the half-cells the electrolyte solutions the moving electrons 13. What is the electrode in the center of the most common dry cell made

  30. chemistry

    A voltaic cell is contructed in which a copper wire is placed in a 1.0 M Cu(NO3)2 solution and a strip of gold i placed in a 1.0 M AuNO3 solution. The measured potential of the cell is found to be 1.36V and the copper electrode is negative. The Ered for

  31. Chemistry

    In a standard hydrogen electrode, why does increasing the partial pressure of H2 gas reduce the standard potential (E) of the cell?

  32. Chemistry ASAP

    Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+ (aq) solution

  33. chemistry

    A galvanic cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of silver in a 1.0 M silver ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.

  34. Chemistry

    1) Assume that the reference half-cell is changed to a standard mercury-mercury (II) half-cell. a) What would be the reduction potential of a standard chlorine half-cell. c) What would be the cell potential of a standard chlorine-nickel cell. 2) For each

  35. Chemistry

    A galvanic cell consists of La^3+/La half-cell and a standard hydrogen electrode. If the La^3+/La half cell functions as the anode and the cell potential is 2.52 V, what is the reduction potential for the La^3+/La half cell? the choices are -2.52V,-0.84V,

  36. CHEMISTRY

    Consider the following cell: Pt|H2(g, 0.130 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 0.90 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion

  37. chemistry

    1. If half cell A has a standard reduction potential of E= -1.10 V and half cell B has a standard reduction potential of E= 0.65 V, which half-cell is the anode? 2. Which half cell has the higher potential energy? 3. Calculate Ecell for this voltaic cell.

  38. Chemistry

    An electrochemical cell that uses the reaction Ti^3+ + 2Cr^2+ -> Ti^1+ + 2Cr^3+ Has a standard cell potential of E¢ªcell = +1.19V a. Write the two half-cell reactions. b. Labeling all parts and show the direction of flow of electrons. (Place the anode

  39. chemistry

    The mercury cell is still sometimes used in industry to prepare chlorine, Cl2, and caustic soda, NaOH. (a)In the first stage of the process a solution of sodium chloride is electrolysed using a voltage of 4.00V. Chlorine gas is obtained at one of the

  40. Chemistry

    Reduction Reaction E0 (V) Cadmium (Cd) Cd2+ + 2e– → Cd -0.40 Silver (Ag) Ag+ + e– → Ag +0.80 If the standard cell potential of a cadmium-silver cell is 1.20 V and the reduction potential of Cd is –0.40 V, what is the oxidation potential of Ag?

  41. Chemistry

    Is this correct? Thanks. What is the standard cell potential? Pb2+ ( aq ) + 2e „³ Pb (s) -0.13V Mn2+ ( aq ) + 2e „³ Mn (s) -1.19V Pb2+ ( aq ) + 2e „³ Pb (s) -0.13V Mn (s) „³ Mn2+ ( aq ) + 2e ¡V +1.19V The electrode potential for a given cell,

  42. AP Chemistry

    (a) When 300.0 milliliters of a solution of 0.200 molar AgNO3 is mixed with 100.0 milliliters of a 0.0500 molar CaCl2 solution, what is the concentration of silver ion after the reaction has gone to completion? (b)Write the net cell reaction for a cell

  43. Chemistry

    how can you tell if something with oxidize or reduce some other thing, based on the standard reduction potential table?

  44. chemistry

    Why is the standard reduction potential E, for the standard hydrogen electrode 0.00V? Please help me explain the reason why to this problem

  45. chemistry - Science

    A zinc-copper battery is constructed as follows (standard reduction potentials given below): Zn | Zn2+ (0.10 M) || Cu2+ (2.50 M) | Cu Zn2+ + 2 e- → Zn(s) Eº = -0.76 V Cu2+ + 2 e- → Cu(s) Eº = 0.34 V The mass of each electrode is 200 g. Each half-cell

  46. chemistry - Science

    A zinc-copper battery is constructed as follows (standard reduction potentials given below): Zn | Zn2+ (0.10 M) || Cu2+ (2.50 M) | Cu Zn2+ + 2 e- → Zn(s) Eº = -0.76 V Cu2+ + 2 e- → Cu(s) Eº = 0.34 V The mass of each electrode is 200 g. Each half-cell

  47. Chemistry

    If E Cu+2 had been chosen as the standard reference electrode and had been assigned a potential of 0.00 V, what would the reduction potential of the hydrogen electrode be relative to it?

  48. Chem

    In conjunction with a standard hydrogen electrode, the La3+|La half-cell is the anode and the standard cell potential is 2.52V. What is the standard reduction potential for the La3+|La half-cell?

  49. Chemistry

    To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.122 V ? (Assume that the partial pressure of hydrogen gas remains at 1 atm.)

  50. Chemistry

    A half-cell that consists of a copper wire in 1.00 M CuNO3 solution is connected by a salt bridge to a half cell containing a 1.00 M X(II) acetate solution and an electrode of metal X. The voltage of the cell is 2.00 V, with metal X as the positive

  51. chemistry

    Q1) How many resonances are expected in the 13C NMR spectrum of propan-1-ol? Q2) A student measures the EMF of the following electrochemical cell at 31oC in a solution that is 0.22 molL-1 in Hg2+ against a Saturated Calomel Electrode as the reference. The

  52. chemistry

    'Aluminium displaces hydrogen from dilute HCl whereas silver does not. The E.M.F. of a cell prepared by combining Al /Al 3 andAg/Ag is 2.46 V. The reduction potential of silver electrode is 0.80 V. The reduction potential of aluminium electrode is :

  53. Chemistry

    1) Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution

  54. Chemistry

    Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution

  55. chemistry

    A galvanic cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of silver in a 1.0 M silver ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.

  56. chemistry (electrochemistry)

    1) For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s) write the net cell equation. Calculate the following values using standard potentials as needed. Eo cell and dGo for each

  57. Chemistry

    Using the standard reduction potentials, calculate the equilibrium constant for each of the following reactions at 298 K. 10Br- + 2MnO4- + 16H+ -> 2Mn2+ + 8H20 + 5Br2 Work: 2Br- -> Br2 + 2e- (This would be multiplied by 5 to balance out with the upper

  58. chemistry

    Calculate the potential of the following two half-cells that are connected by a salt bridge: a galvanic cell consisting of a standard hydrogen electrode on the left and a platinum electrode immersed in a solution that is 3.50 3 1023 M in TiO21, 0.07000 M

  59. chemistry

    A voltaic cell consists of two half-cells. One half-cell contains a chromium electrode immersed in 1.00 M Cr(NO3)3 solution. The second half-cell contains a nickel electrode immersed in 1.00 M Ni(NO3)2 solution. Nickel plates out on the nickel electrode as

  60. Chemistry

    1) Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution

  61. Ap Chemistry

    Suppose a galvanic cell contains one nickel electrode and one copper electrode. At 25°C, nickel has a negative reduction potential and copper has a positive reduction potential. At which electrode will reduction occur? - I believe copper will be oxidised

  62. Chem HELP !!!

    Using a table of standard electrode potentials (as in Appendix M of your text), calculate the standard cell potential, Eo, for: 2 Fe2+(aq) + Cl2(g) 2 Fe3+(aq) + 2 Cl(aq).

  63. chemistry

    Using the given data, and the table of Standard Reduction Potentials, find the standard reduction potential for this half reaction: 8H^+ + BaCrO4(s) + 3e- -> Ba^2+ + Cr^3+ + 4H2O(l) given: Ksp (BaCrO4)=2.1E-10 DeltaGf* (kJ/mol): CrO4^2- (-727.75), Cr2O7^2-

  64. Chemistry

    The standard reduction potential for Cr3+(aq) is −0.74 V. The half-reaction for the reduction of Cr3+(aq) is the following. Cr3+(aq) + 3 e− → Cr(s) The standard reduction potential for Ni2+(aq) is −0.26 V. The half-reaction for the reduction of

  65. CHEMISTRY

    Assuming that this half cell I2 + 2e- + =>2I- as standard electrode and assumed its potential that is 0.00 V : a) what is standard potential of this half cell : Br2 + 2e- + => 2Br- b) what is standard potential of this half cell : Al^+3 + 3e- => Al

  66. Chemistry

    Calculate the cell potential for the following reaction as written at 79C given that [Zn^+2] = 0.819 M and [Ni^+2] = 0.014 M. Zn + Ni^+2 = Zn^+2 + Ni I know: E=E -RT/nF ln Q reduction potential for Ni= -0.26 reduction potential for Zn = -0.76 so E standard

  67. Chemistry

    Given these standard reduction potentials at 25 C 1. Cr3+ + e- ===> Cr2+ E1=-0.407 V 2. Cr2+ + 2e- ===> Cr(s) E2=-0.913 V determine the standard reduction potential at 25C for the half-reaction equation Cr3+ + 3e- ===> Cr(s) E=? When I tried, I got 1.08V

  68. CHEMISTRY

    The standard potential of this cell Sn|Sn^+2 || Cr^+3|Cr is -0.60 V , what is the reductional standard potential of Cr^+3|Cr ? if we know that reduction potential of Sn is Sn^+2 + 2e- Sn : -0.14 V

  69. chemistry

    An electrochemical cell of notation Pd | Pd²⁺ || Cu²⁺ | Cu has E° = -0.65 V. If we know that the standard reduction potential of Cu²⁺/Cu is E° = 0.34 V, what is the standard reduction potential for Pd²⁺/Pd?

  70. ap chemistry

    I have a lot of questions actually. it's electrochemistry (which is obviously a bunch of fun) 2 electrodes Cr(s)/Cr3+ and Sn(s)/Sn2+ are combined to afford a spontaneous electrochemical reaction. the standard reduction potention in V for Cr3+ and Sn2+ are

  71. Chemistry

    Please check to see if i did it right.. if the reduction potential for Cu^2+ + 2e---> Cu is 0.00V. Then the remaining reduction potentials for the voltages between Cu[cathode]/Zn[anode] is like??? Ecell=1.043v My answers:Zn-->Zn2+ 2e- voltage = -1.043V

  72. Chemistry

    2. A fluoride electrode is used to determine fluoride in a water sample. Standards and samples are diluted 1:10 with TISAB solution. For a 1.00 x10-3M(before dilution) standard, the potential reading relative to the reference electrode is -211.3mV and for

  73. Chemistry

    What will be the potential of a cell constructed of a standard hydrogen electrode as one half-cell and a silver wire coated with AgBr dipping into 0.13 M HBr as the other half-cell? The value of Ksp for AgBr is 5.4 × 10-13. For the Ag/AgBr electrode,

  74. chemistry

    I posted this question last night but did not get an answer- I am posting again because I have an exam I am studying for and do not understand this concept! Thanks! Using the given data, and the table of Standard Reduction Potentials, find the standard

  75. Chemistry - Science (Dr. Bob222)

    Posted by Ana on Saturday, May 3, 2014 at 11:23am. A zinc-copper battery is constructed as follows (standard reduction potentials given below): Zn | Zn2+ (0.10 M) || Cu2+ (2.50 M) | Cu Zn2+ + 2 e- → Zn(s) Eº = -0.76 V Cu2+ + 2 e- → Cu(s) Eº = 0.34 V

  76. Chemistry

    If the standard cell potential of zinc-copper cell is 1.10 V and the reduction potential of Cu is 0.34 V, what is the reduction potential of Zn? The answer is -0.76, correct?

  77. chemistry

    From the indicated voltages for the voltaic cell pictured, determine the standard electrode potential, E°M3+/M, if the metal, M, is each of the following. description on the image: in the left beaker there is one Cr3+ and one Cr2+ on the right beaker

  78. Chemistry

    Some bacteria get their energy from reduction of CO2 to CH4 by H2. 1. How many electrons are required to reduce CO2 to CH4? 2. Calculate the G for formation of methane based on the two standard reduction potential of -0.171V for reduction of CO2 to CH4 and

  79. Chemistry

    Some bacteria get their energy from reduction of CO2 to CH4 by H2. 1. How many electrons are required to reduce CO2 to CH4? 2. Calculate the G for formation of methane based on the two standard reduction potential of -0.171V for reduction of CO2 to CH4 and

  80. Chemistry

    A voltaic cell designed to measure [Cu2+]is constructed of a standard hydrogen electrode and a copper metal electrode in the Cu2+ solution of interest. 1. If you wanted to construct a calibration curve for how the cell potential varies with the

  81. CHEMISTRY

    What is the function ( or role ) of platinum in electrochemistry in general ? I read a question about platinum in electric potential , and in standard electrode potential ?! thank you a lot

  82. Chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact with a saturated

  83. chemistry... HELP

    Equilibrium constant question!!!? Standard reduction potentials Reduction half-reaction E(V) Ag+(aq) + e- ---> Ag (s) 0.80 Cu ^2+ (aq) + 2e- ---> Cu (s) 0.34 Sn^4+(aq) + 4e- ---> Sn (s) 0.15 2 H+(aq) + 2e- ---> H2 (g) 0 Ni^2+(aq) + 2e- ---> Ni (s) -0.26

  84. Chem 152

    Given the measured cell potential, E cell is -0.3603 V at 25°C in the following cell, calculate the H+ concentration Pt(s)|H2(g,0.713 atm)|H+(aq, ? M)||Cd2+(aq 1.00 M)|Cd(s) The balanced reduction half-reactions for the cell, and their respective standard

  85. Inorganic chemistry

    The following electrochemical cell has the potential of +0.617V at 25 degrees Celsius Pt ! H2(g, 1.00 atm) ! H+ (aq, 1.00M !! Ag^+(aq) ! Ag The standard reduction potential, E naught, of Ag^+ = 0.799V. What is the Ag+ concentration?

  86. Chemistry Check Please!!!

    Using a table of standard electrode potentials (as in Appendix M of your text), calculate the standard cell potential, Eo, for: 2 Fe2+(aq) + Cl2(g) 2 Fe3+(aq) + 2 Cl(aq). Answer: Anode: 2 Fe2+ 2 Fe3+ + 2 e Eox = 0.771 V Cathode: Cl2 + 2 e 2 Cl Ered = +1.36

  87. chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact with a saturated

  88. Inorganic chemistry

    I do not know how I should approach this problem either. The following electrochemial cell has a potential of+0.617V at 25 degrees Celsius Pt ! H2(g,1.00atm) ! H^+(aq,1.00M) !! Ag^+(aq) ! Ag The standard reduction potential ,E naught of Ag^+ = 0.700V. What

  89. Chemistry

    Using standard reduction potentials, show that one can prepare an ammine complex from CoCl2 and hydrogen peroxide in the presence of ammoinia but not in its absence. (need to write two redux reactions, calculate standard potentials for the reactions, and

  90. chemistry

    The standard reduction potentials of lithium metal and chlorine gas are as follows: (for Li, reduction potential is -3.04, for Cl it is 1.36) In a galvanic cell, the two half-reactions combine to 2Li{+](s) + Cl{-}2(g) --> 2Li{+}Cl{-}(aq) cell potential=4.4

  91. Chemistry

    Given the following half-reactions and their standard reduction potentials, Ni2+ + 2e− Ni E° = -0.25 V 2H+ + 2e− H2 E° = 0.00 V Ag+ + e− Ag E° = 0.80 V a spontaneous reaction will occur between: a. Ni2+ and H2 b. H+ and Ag c. Ag+ and Ni d. Ni2+

  92. Chem

    Calibration of a glass electrode gave a reading of 139.3 mV with 0.05 m potassium dihydrogen citrate buffer standard (pH = 3.766) and a reading of -79.0 mV with 0.08 m HEPES, 0.08 m NaHEPES, 0.08 m NaCl buffer standard (pH = 7.454), both measured at 30°C.

  93. riga technical university

    At what concentration of silver electrolyte the potential of the silver elevtrode will be greater than 0.1V of the silver electrode standard potential?

  94. chemistry

    Calculate the standard reduction potential for the reaction of Cu(III) to Cu(II) Use the following data: 1) Cu^+3 + 2e^- -> Cu^+, E°1 = 1.28 V 2) Cu^+2 + e^- -> Cu^+, E°2 = 0.15 V 3) Cu^+2 + 2e^- -> Cu(s), E°3 = 0.34 V 4) Cu^+ + e^- -> Cu(s), E°4 =

  95. Chemistry DR BOB

    Under standard conditions of 1 atm and 298.15K, the half-cell reduction potential E,zero for the anode in a voltaic cell is 0.37V. The half-cell reduction potential E,zero for the cathode of the cell is 0.67V. The number of moles, n, of electrons

  96. Chemistry

    how can you tell if something with oxidize or reduce some other thing, based on the standard reduction potential table?

  97. chemistry

    (b) (i)The e.m.f. of the cell was measured as 0.62 volts. Taking the standard electrode potential of Cu/Cu2+ as = +0.34 volts, calculate the standard potential of the Co/Co2+ system. Be careful to indicate whether your answer is positive or negative. (ii)

  98. Chemistry

    Cadmium and a solution of cadmium(II) nitrate are used with tin and a solution of tin(II) nitrate to construct a galvanic cell. 1) The reaction run initially at standard state with 100-mL samples of each solution is allowed to proceed until 8.0 g of tin

  99. Chemistry

    The standard electrode potentials for three electrode systems are: Ti^3+(aq) + e^- --> Ti^2+ E= -0.37 Fe^3+ ---> Fe^2+(aq) E= +0.77 Ce^4(aq) + e^- ---> Ce^3+(aq) E= +1.45 Using the data above, deduce which species is the best reducing agent, giving a

  100. Chemistiy

    based on standard reduction potentials which metals would i) inhibit rusting ii)promote rusting My general statement is: > If the reduction potential is higher it will inhibits rusting and if it is lower it will promote rusting But im not sure because it

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