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If the Fe2+(aq) + 2e---> Fe(s) was used as a reference for the electrode potential table instead of the standard hydrogen half cell what would the potential of the following half cell be? Ni2+(aq) + 2e---> Ni(s) A) -0.19 V

17,568 results
  1. Chemistry

    If the Fe2+(aq) + 2e---> Fe(s) was used as a reference for the electrode potential table instead of the standard hydrogen half cell what would the potential of the following half cell be? Ni2+(aq) + 2e---> Ni(s) A) -0.19 V B) -0.71 V C) +0.19 V D) +0.71 V
  2. 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?
  3. 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
  4. 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).
  5. CHEMSTRY

    . A small amount of solid Hg2Cl2 and 25 ml of metallic mercury were added to a solution of 5.03 x 10-2 M NaCl. A platinum electrode immersed in the layer of mercury was connected to a reference half-cell whose electrode potential was 0.222V. The voltage of
  6. Chemistry...please help

    A galvanic cell is based on the following half-reactions: Fe2+ + 2e- --> Fe(s) E= –0.440 V 2H+ + 2e- --> H2(g) E= 0.000 V where the iron compartment contains an iron electrode and [Fe2+] = 1.00 x 10-3 M and the hydrogen compartment contains a platinum
  7. Analytical Chemistry

    A solution prepared by mixing 51.4 mL of 0.340 M AgNO3 and 51.4 mL of 0.340 M TlNO3 was titrated with 0.680 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is
  8. Analytical Chemistry

    A solution prepared by mixing 51.4 mL of 0.340 M AgNO3 and 51.4 mL of 0.340 M TlNO3 was titrated with 0.680 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is
  9. chemistry

    How do you calculate the theoretical cell voltage? 1) Zn|Zn^+2 (1M)| Cu|Cu^+2 (1M) okay so by looking at example this example Calculate the emf (voltage) for the following reaction: Zn(s) + Fe2+ → Zn2+ + Fe(s) Write the 2 half reactions: Zn(s) → Zn2+ +
  10. Analytical Chemistry

    A solution prepared by mixing 51.4 mL of 0.340 M AgNO3 and 51.4 mL of 0.340 M TlNO3 was titrated with 0.680 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is
  11. chemistry

    A solution prepared by mixing 47.1 mL of 0.4 M AgNO3 and 47.1 mL of 0.4 M TlNO3 was titrated with 0.8 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is attached to
  12. 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
  13. 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
  14. 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
  15. chemistry ap ...urgent! please help me!

    The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25.00 degrees C is given by the equation: E(measured)= E(ref) +.591pH where ref contains the potential of the reference electrode and all other
  16. Chemistry

    I dont quite understand how to find out if it's capable of reducing/oxidizing. My understanding is we check each potential and identify which is reduce = highest potential, oxidize = lowest potential. These are my predictions: yes Is Fe2+(aq) capable of
  17. 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
  18. AP CHEMISTRY

    A solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10. (A) Assuming that the hydroxide is 1.0
  19. chemistry - exam practice help!!

    For the cell shown below, which will increase the cell voltage the most? Fe2+ | Fe3+ || Cu2+ | Cu A) Halve[Cu2+] B) Double[Cu2+] C) Double[Fe2+] D) Halve[Fe2+] E) Cut Cu electrode in half ... Ecell = E0 cell + 0.059/n * log([Cu+]/[Fe2+]) Ecell is directly
  20. chemistry

    When an ion-selective electrode for X was immersed in 0.0210 M XCl, the measured potential was 0.0480 V. What is the concentration of X when the potential is 0.0630 V? Assume that the electrode follows the Nernst equation, the temperature is at 25°C, and
  21. 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
  22. 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
  23. 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
  24. AP Chem

    An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminum metal electrode. (a) What is the potential of this cell at 25°C if the aluminum electrode is placed in a
  25. Chemistr repost

    Determine the cell potential (in V) for a platinum electrode in an acidic solution of 0.004M H+(aq), 3.226M ClO4-(aq) and 4.445M ClO3- (aq) ions, coupled to a gold electrode in 3.238 M Au3+ (aq) at 307.10 K. Im confused about the mulitple molarities given
  26. Chemistry

    Determine the cell potential (in V) for a platinum electrode in an acidic solution of 0.004M H+(aq), 3.226M ClO4-(aq) and 4.445M ClO3- (aq) ions, coupled to a gold electrode in 3.238 M Au3+ (aq) at 307.10 K. Im confused about the mulitple molarities given
  27. 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
  28. chemistry

    Determine the cell potential for Ni(s) + Fe²⁺(aq) → Ni²⁺(aq) + Fe(s) where [Ni²⁺] = 0.60 M and [Fe²⁺] = 0.0030 M using the following standard reduction potentials. Ni²⁺(aq) + 2e⁻ → Ni(s) E° = -0.25 V and Fe²⁺(aq) + 2e⁻ → Fe(s)
  29. AP CHEMISTRY

    A solution is prepared in which a trace or small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10^-2 M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x10^-10. A. Assuming that the hydroxide is 1.0 x
  30. Chem

    When an ion-selective electrode for sulfate was immersed in 0.0300 M sodium sulfate, the measured potential was 0.0460 V. What is the concentration of sulfate when the potential is 0.0610 V? Assume that the electrode follows the Nernst equation, the
  31. Physics

    A table can be modeled as a flat block supported by four identical legs. If the mass of the top block is 10 kg and each leg is a uniform rod with height of 1m and mass of 5 kg. Find the gravitational potential energy of the table. Take the ground as the
  32. chemistry

    A galvanic cell consists of a Mn/Mn^2+ electrode (E° = -1.18v) and a Fe/Fe^2+ electrode (E° = -0.44v). Calculate the ratio [Mn2+]/[Fe2+] if E_cell = .78v at 25°C. I know to use the nernst eq. E_cell = E°_cell - RT/nF * ln(Q) where Q is the ratio I'm
  33. chemistry

    what is the cell potential of the following cell: a platinum wire placed into a mixture of: KIO4 (0.02M), KIO3 (0.040M), H3PO4 (0.10M), KH2PO4 (0.40M) assuming it is put against a Ag/AgCl reference electrode?
  34. chemistry

    I posted this que before but got no answers pls help me :( A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 ´ 10-5 M and by placing a Pt electrode in the other compartment, in which the H+
  35. Chemistry

    3Fe2+(aq) + 2Al(s) --> 3Fe(s) + 2Al3+(aq) Which of the following statements is true about Fe2+? 1.Fe2+ is losing electrons. 2.Fe2+ is oxidized. 3.Fe2+ is the oxidizing agent. 4.Fe2+ is the reducing agent.
  36. 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 :
  37. 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
  38. Chemistry

    A solution of K2CrO4 was titrated with AgNO3, using a silver indicator electrode (E=0.799V) and a S.C.E. electrode (E=0.241V). The product, Ag2CrO4, has a Ksp = 1.1x10^-12. What is the potential at the equivalence point?
  39. electric chem

    A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 ´ 10-5 M and by placing a Pt electrode in the other compartment, in which the H+ concentration is 3.4 M and = 1.00 atm.
  40. ChemISTRY (WEBWORK)

    A student measures the potential for cells containing A+B+and C+ ions and their metals and records his data in the table below: ............. Overall Reaction ................Potential (V) Cell#1'''''''A(s) A+(aq) B+(aq) B(s)''''''''''''0.90
  41. Chemistry

    The following galvanic cell at standard conditions has a potential of 0.03 V: Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s). What would be the effect of increasing the concentration of Ag+? A. The cell potential will decrease. B. The cell potential will
  42. Chemistry

    The following galvanic cell at standard conditions has a potential of 0.03 V: Ag+(aq) + Fe2+(aq) → Fe3+(aq) + Ag(s). What would be the effect of increasing the concentration of Ag+? A. The cell potential will decrease. B. The cell potential will
  43. 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.)
  44. 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.)
  45. Science - Electrochemistry

    In an experiment 0.0500 M AgNO3 was used to titrate 20 mL of 0.12 M NaCl solution. When silver electrode is used together with the pH electrode to measure potential at each point during the titration, the potential measured at equivalence point is 0.055 V.
  46. chemistry

    how do you find the standard electrode potentials of KMnO4 and MnCl2? and is the standard electrode potential of MnO2 1.28?
  47. Chem. help please

    A zinc-copper battery is constructed as follows at 25 degree C: Zn | Zn2+(0.15 M) || Cu2+(1.70 M) | Cu The mass of each electrode is 250. g. I found the cell potential to be 1.13V and the cell potential after 5.00 A of current has flowed for 8.00 h is
  48. 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
  49. Chemistry

    Im having trouble on a question Im not sure what it is they are asking for. A voltaic cell similar to that shown in Figure 20.5 is constructed. One electrode compartment consists of a silver strip placed in a solution of AgNO3, and the other has a iron
  50. 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
  51. 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
  52. 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
  53. chemistry

    The mean activity coefficients of HBrin 5.0 and 20.0 mmol kg –1 are 0.930 and 0.879, respectively. Consider a hydrogen electrode in HBr(aq) solution at 25 °C operating at 1.15 atm. Calculate the change in the electrode potential when the molality of the
  54. Chem Check Please!!!

    1) Calculate the cell potential, at 25 C, based upon the overall reaction Zn2+(aq) + 2 Fe2+(aq) -> Zn(s) + 2 Fe3+(aq) if [Zn2+] = 1.50 x 10^-4 M, [Fe3+] = 0.0200 M, and [Fe2+] = 0.0100 M. The standard reduction potentials are as follows: Zn2+(aq) + 2
  55. URGENT AP CHEM HELP!!

    Write 2-3 sentences describing and identifying the type of chemical reaction that occurs when Fe2+ reacts with potassium permanganate (KMnO4) and specifying the type of solution required for the reaction to occur. b. using standard reduction potential
  56. Chemistry

    calculate cell potential at 25C for: 3Fe3+(aq) + AL(s)= 3Fe2+(aq)+ Al3+ (aq) if Fe3+ = 0.300 M, Fe2+ = 0.150M Al3+ = 0.300M. The standard reduction potentials are as follows: Fe3+ (aq) + e- = Fe2+ (aq) Al3+ (aq) + 3e-=Al (s) Eo = +0.771 V Eo = -1.66 V
  57. Chemistry

    Which statement is true for the cell as it discharges? Zn | Zn2+(1 .0 M) || Sn2+(1.0 M) | Sn (A) Oxidation occurs at the tin electrode. (B) Electrons will flow from the tin electrode to the zinc electrode. (C) The concentration of Zn2+ will increase. (D)
  58. Chemistry

    2 Ag+(aq) + Fe(s) --> 2 Ag(s) + Fe2+(aq) Which electrode is the anode, and which is the cathode. and In which directions do the cations and anions migrate through the solution? cations thanks
  59. Chemistry -please help!

    A zinc-copper battery is constructed as follows at 25°C. Zn|Zn^2+ (0.15 M)||Cu2+(3.00 M)|Cu The mass of each electrode is 200. g. a) Calculate the cell potential when this battery is first connected. - i got this to be 1.14V b.) Calculate the cell
  60. Chemistry

    A zinc-copper battery is constructed as follows at 25°C. Zn|Zn^2+ (0.15 M)||Cu2+(3.00 M)|Cu The mass of each electrode is 200. g. a) Calculate the cell potential when this battery is first connected. - i got this to be 1.14V b.) Calculate the cell
  61. AP Chem

    Redox Titrations: a. write 2-3 sentences describing and identifying the type of chemical reaction that occurs when Fe2+ reacts with potassium permanganate (KMnO4) and specifying the type of solution for the reaction to occur. b. using a standard reduction
  62. college chemistry

    A zinc-copper battery is constructed as follows: Zn | Zn+2(0.10 M) || Cu+2 (2.50 M)| Cu The mass of each electrode is 200.0 g. Each half cell contains 1.00 liter of solution. a) Calculate the cell potential when this battery is first connected. b)
  63. science

    if the same 1.0 kg book is lifted to 0.5 meters above the table, but the table top is 1.0 meters above the floor,, what would be the potential energy of the book if the reference level were the floor??
  64. Physics

    Can someone please explain how to tackle this problem? Cu - Anode electrode Zn - Cathode electrode A current of 2 amps is sustained for 16 minutes. what mass of Cu(s) is deposited on the zinc electrode? (Faradays' constant: 96500 C/mol e-) Please and thank
  65. Chem

    Can someone please explain how to tackle this problem? Cu - Anode electrode Zn - Cathode electrode A current of 2 amps is sustained for 16 minutes. what mass of Cu(s) is deposited on the zinc electrode? (Faradays' constant: 96500 C/mol e-)
  66. 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)
  67. 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
  68. operating system

    please tell me if i have solved these correctly question: Consider a paging system with the page table stored in memory. 1)If a memory reference takes 50 nanoseconds, how long does a paged memory reference take? answer=2x50=100ns 2). If we add TABs, and 75
  69. Chemistry

    One half-cell in a voltaic cell is constructed from a silver wire electrode in a .25 M solution of AgNO3 . The other half-cell consists of a zinc electrode in a .001 M solution of Zn(NO3)2. Calculate the cell potential I have no idea and am so stressed,
  70. Chemistry

    What initial concentration of Cd2+ is required to result in a cell potential of 0.200 V in a voltaic cell constructed by connecting a nickel electrode that is dipped into 1.00 M NiSO4 solution to a cadmium electrode that is dipped into a solution
  71. chemistry

    A galvanic cell has an iron electrode in contact with 0.20 M FeSO4 and a copper electrode in contact with a CuSO4 solution. If the measured cell potential at 25 degrees Celcius is 0.61 V , what is the concentration of Cu2+ in the CuSO4 solution?
  72. Chem

    Calibration data for a bromide ion-selective electrode (ISE) was collected and recorded below. The potential of the ISE was measured against a saturated calomel electrode (SCE). All solutions were buffered at a pH of 7.56. A linear calibration curve can be
  73. 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
  74. physical chemistry PLEASE HELP!!!

    how do i calculate a ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+ given E(mV) at 25 C and pH7 as 100 and absorbance at 550nm as 1.5 E is relative to standard hydrogen electrode i don't know how im supposed to calculate it from this data
  75. physical chemistry

    how do i calculate a ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+ given E(mV) at 25 C and pH7 as 100 and absorbance at 550nm as 1.5 E is relative to standard hydrogen electrode i don't know how im supposed to calculate it from this data
  76. precal

    Suppose the Cu electrode was replaced by an Al electrode. In order for this new cell to be a galvanic cell, which electrode would be the anode, Zinc or Aluminum?
  77. chemistry help

    Suppose the Cu electrode was replaced by an Al electrode. In order for this new cell to be a galvanic cell, which electrode would be the anode, Zinc or Aluminum?
  78. Chemistry PLEASE HELP

    how do i calculate a concentration ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+ given at 25 C and pH7 E(mV) as 100 and absorbance at 550nm as 1.5 E is relative to standard hydrogen electrode i don't know how im supposed to calculate it from this
  79. chem please help

    how do i calculate a concentration ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+ given at 25 C and pH7 E(mV) as 100 and absorbance at 550nm as 1.5 E is relative to standard hydrogen electrode i don't know how im supposed to calculate it from this
  80. chem HELP PLEASE

    how do i calculate a concentration ratio of oxidised to reduced cytochrome c Fe2+ to Fe3+ given at 25 C and pH7 E(mV) as 100 and absorbance at 550nm as 1.5 E is relative to standard hydrogen electrode i don't know how im supposed to calculate it from this
  81. Science

    When 25.0 ml of a solution containing both Fe2+and Fe3 +ions is titrated with 23.0 ml of 0.0200M KMnO4(in dilute sulphuric acid), all the Fe2+ are oxidised to Fe3+ ions. Next, the solution is treated with Zinc metal to convert all the Fe3+ ions to Fe2+
  82. 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
  83. chemistry

    Vanadium is an environmental pollutant originating from some types of steel, but also from the combustion of fossil fuels. The amount of V2+ in an unknown sample is determined by potentiometric titration by 7.62 mM permanganate ion, MnO4 - . 25.00 mL of
  84. 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,
  85. chemistry

    A pH glass/calomel electrode was found to develop a potential of -0.0390 V when used with buffer of pH 5.52. With an unknown solution, the potential was -0.360 V. Calculate the pH of the unknown solution
  86. 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?
  87. chemistry

    The measured potential of the following cell was 0.1776 volts. Pb|Pb2+ (?M )||Pb2+ (1.0M)|Pb Calculate the electrode potential of the unknown half-cell (anode).
  88. physics

    (a) Find the potential at a distance of 0.920 cm from a proton. (Note: Assume a reference level of potential V = 0 at r = ∞.) V (b) What is the potential difference between two points that are 0.920 cm and 2.00 cm from a proton? V (c) Repeat parts (a)
  89. Chemistry

    when 25.0 mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe2+ ions are oxidized to Fe3+ ions. Next, the solution is treated with Zn metal to convert all of
  90. College Physics

    Current passes through a solution of sodium chloride. In 1.00 second,2.68 x 10^16 Na+ ions arrive at the negative electrode and 3.92 10^16 Cl- ions arrive at the positive electrode. What is the current passing between the electrodes? mA What is the
  91. 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,
  92. Chemistry/Redox Reactions

    An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminium metal electrode immersed in a solution with [Al3+] = 1.0 M. Sodium hydroxide is added to the aluminium
  93. Electrochemistry

    Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a
  94. George School

    Ag2CrO4(s) + 2e- 2Ag(s) + CrO42-(aq) A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; which has a reduction potential of 0.242 V relative to the SHE) and a
  95. chemistry

    balance the net ionic equation for the overall reaction. Pt | Fe2+(aq), Fe3+(aq) || I-(aq) | AgI(s) | Ag(s) a) Fe3+(aq) + Ag(s) + I-(aq) → Fe2+(aq) + AgI(s) b) Fe2+(aq) + Ag(s) + I-(aq) → Fe3+(aq) + AgI(s) c) Fe3+(aq) + AgI(s) → Fe2+(aq) + Ag(s) +
  96. 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
  97. College Physics

    Current passes through a solution of sodium chloride. In 1.00 second, 2.68 x 10^16 Na+ ions arrive at the negative electrode and 3.92 x 10^16 Cl-ions arrive at the positive electrode. What is the current passing between the electrodes? Current = mA What is
  98. Chemistry

    If I am titrating KMnO4 against a sample of Fe2+, but there is also I- in the sample which of the iron and iodine will be oxidised first? Unless something is present in the sample to complex the iodide ion, KMnO4 may titrate both. How are you titatrating
  99. chemistry.

    a quantity of 25 ml of a solution containing both Fe2+ and Fe3+ ions is titrated with 23 ml of .02 M KMnO4 solution. as a result all the Fe2+ ions are oxidised to Fe3+ ions. Next the solution is treated with Zn metal to convert all Fe3+ ions to Fe2+ ions.
  100. General Chemestry

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

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