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How does H(2)-O(2) fuel cell operate?...

How does `H_(2)-O_(2)` fuel cell operate?

Text Solution

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At anode: `2H_(2)(g)+4OH^(-)(aq)to4H_(2)O+4e^(-)`
At cathode: `underline(O_(2)(g)+2H_(2)O(e)+4e^(-)to4OH^(-)(aq))`
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Describe the construction of a H_(2)-O_(2) , fuel cell and the reactions H_(2)O taking place in it.

State two advantages of H_(2)-O_(2) fuel cell over ordinary cell.

Knowledge Check

  • EMF of an H_(2)-O_(2) fuel cell

    A
    Is indepenent of partial pressures of `H_(2)` and `O_(2)`
    B
    Decreases on increasing `P_(H_(2))` and `P_(O_(2))`
    C
    Increases on increasing `P_(H_(2))` and `P_(O_(2))`
    D
    Varies with the concentration of `OH^(-)` ions in the cathodic and anodic compartments.

  • Fuel cells : Fuel cells are galvanic cells in which the chemical energy of fuel cell is directly converted into electrical energy. A type of fuel cell is a hydrogen - oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst ( platinum, silver, or metal oxide ). The electrodes are placed in aqueous solution of NaOH . Oxygen and hydrogen are continuously fed into the cell. Hydrogen gets oxidized to H^(o+) which is neutralized by overset(c-)(O)H, i.e., anodic reaction. At cathode, O_(2) gets reduced to overset(c-)(O)H Hence, the net reaction is The overall reaction has DeltaH=-285.6 kJ mol^(-1) and DeltaG=-237.4 kJ mol^(-1) at 25^(@)C If the cell voltage is 1.23V for the H_(2)-O_(2) fuel cell and for the half cell :

    A
    `0.41V`
    B
    `0.83V`
    C
    `-0.41V`
    D
    `0.83V`

  • W.r.t. H_(2)-O_(2) fuel cell the correct statement is

    A
    electrolyte used is pure `H_(2)O`
    B
    heat of combustion is directly converted to electrical energy
    C
    `O_(2)` gas gets oxidised to `O_(3)` in cell
    D
    overall reaction in the cell is `H^(+)+OH^(-)rarrH_(2)O`

    • Similar Questions

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    How does fuel cell operate

    Draw a neat and labelled diagram for H_(2)-O_(2) fuel cell. Write the reaction which occurs at cathode of the cell.

    (a) What are fuel cells ? Explain the electrode reactions involved in the working of H_(2)-O_(2) fuel cell. (b) Represent the galvanic cell in which the reaction Zn(s) + Cu^(2)(aq) to Zn^(2+) (aq) + Cu(s) takes place.

    What are fuel cells ? Explain the electrode reactions involved in the working of H_(2) - O_(2) fuel cell.

    For a H_(2) - O_(2) fuel cell , the theoretical voltage has been found to be 1.23 V and Delta H to be -285 kJ mol^(-1) . The efficiency of the fuel cell is

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