In a hydrogen - oxygen fuel cell, combustion of hydrogen occurs to :
- Produce high purity water
- Create potential difference between the two electrodes
- Generate heat
- Remove adsorbed oxygen from electrode surfaces
The Correct Option is B
Solution and Explanation
$2H_{2}\left(g\right)+4OH^{-}\left(aq\right) \rightarrow 4H_{2}O\left(l\right)+4e^{-}$
$\frac{O_{2}\left(g\right)+2H_{2}O\left(l\right)+4e^{-}\rightarrow4OH^{-}\left(aq\right)}{Overall reaction=2H_{2}\left(g\right)+O_{2}\left(g\right)\rightarrow2H_{2}O\left(l\right)}$
the net reaction is the same as burning (combustion) of hydrogen to form water.
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Reason :
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Concepts Used:
Dihydrogen as a Fuel
Dihydrogen emancipates a large quantity of heat when it gets combusted. We can compare the energy emancipated by the combustion of various fuels like methane, LPG, Dihydrogen, etc., in the terms of the same amounts in mole, mass, and volume. Dihydrogen emancipates more energy than petrol. As well as, the combustion of dihydrogen will lead the way to less pollution than petrol. As dinitrogen exists as an impurity with dihydrogen, the only pollutants will be the oxides of dinitrogen. Furthermore, we would have to transform dihydrogen gas into the liquid state by cooling it down to 20K. We would be needed expensive insulated tanks for this transformation. Tanks of metal alloys such as Ti-TiH2, NaNi5, Mg-MgH2, etc, are used for storing dihydrogen in small quantities. Hence, due to these disadvantages and limitations, we have developed alternate techniques to use dihydrogen effectively and efficiently.
Read More: Hydrogen