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State two advantages of H(2)-O(2) fuel c...

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

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**Step-by-Step Solution:** 1. **Definition of Fuel Cell:** - A fuel cell is a device that generates electrical energy through an electrochemical reaction using fuel (in this case, hydrogen) and an oxidant (oxygen). 2. **Advantage 1 - Continuous Electricity Production:** - One significant advantage of hydrogen-oxygen fuel cells is their ability to produce electricity continuously as long as the fuel (H₂) and oxidant (O₂) are supplied. This means that they can operate for extended periods without the need for recharging, unlike ordinary cells which have a limited lifespan and require recharging after depletion. ...
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In H_(2)-O_(2) fuel cell, the reaction occurring at cathode is

In H_(2)-O_(2) fuel cell, the reaction occurring at cathode is

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 :

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 :

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