Jumping straight into the example👊
I- Understand the principles of hydrogen-oxygen fuel cell
II- Write the half-equation for reaction occurring at each electrode and the overall equation for reaction in a
hydrogen-oxygen fuel cell
III- State the pros and cons of a hydrogen-oxygen fuel cell
Part I- Principle of a hydrogen-oxygen fuel cell
Here is a simplified diagram👇
In the cell, three components are separated from each other by two electrodes.
The fuel (hydrogen) is supplied into the negative electrode(anode) while the oxidant(oxygen) is supplied into the positive electrode(cathode).
Further Details:
The electrolyte in the central compartment is hot concentrated potassium hydroxide solution
Part II
Half-equation at the anode
H2(g) + 2OH-(aq) → 2H2O(l) + 2e-
Half-equation at the cathode
O2(g) + 2H2O(l) + 4e- → 40H-
Overall equation
2H2(g) + O2(g) → 2H2O
Part III
Pros👍
- Do not emit any air pollutants and only water is produced✔️
- High energy efficiency of about 70%✔️
- Can operate continuously if the flow of O2(g) and H2(g) can be maintained✔️
Cons👎
- Materials used to make the electrodes are expensive 💰 💰
- Manufacturing of the cells results in the production of toxic by-products 💀
- The fuel(hydrogen) needed can only be produced cheaply by fossil fuels
- Do not work well at low temperatures *if the temperature drops below 0˚C, the cell will freeze
- Safety concerns as high-pressure tanks are required to store the hydrogen ☠️
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