Post a New Question

Chemistry

posted by .

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 reduction potential E°(Pu4+/Pu3+), in volts? [Enter only a number.]

  • Chemistry -

    Pu+3 ==> Pu+4 + e Eo = ??
    Cl2 + 2e ==> 2Cl^- Eo 1.36
    ============================
    2Pu+3 + Cl2 ==> 2Pu+4 + 2Cl^- Ece.. = 0.35
    What is ?? + 1.36 = 0.35
    Solve for ?? which will be the oxidation potential (because that's the way the half cell is written above) so change the sign for the reduction problem (what the problem is asking).

  • Chemistry -

    Cl is gaining elections which means it is the reduction half reaction. Reduction is associated with the Cathode.

    E(cell) = E(cathode) - E(anode)

    0.35v = 1.36v - E(anode)
    solving for E(anode) gives you 1.01v

  • Chemistry -

    1.17 V

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. 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 …
  2. 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 …
  3. chemistry

    Give the cell diagram notation of the electrochemical cell that could be used to determine experimentally the dissociation constant (Kw) of water. The standard reduction potential for: O2 + 2H20 + 4e- ---------> 4 OH- 0.40 V
  4. 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 …
  5. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction …
  6. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction …
  7. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction …
  8. 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 reaction............................................................. …
  9. 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 …
  10. 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. …

More Similar Questions

Post a New Question