Solution Found!
In a hydrogen fuel cell, the steps of the chemical
Chapter 5, Problem 4P(choose chapter or problem)
\(\begin{array}{l}\text{at - electrode: } \mathrm{H}_{2}+2 \mathrm{OH}^{-} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \text{;}\\ \text{at + electrode: } \frac{1}{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-} \text{.}\end{array}\)
Calculate the voltage of the cell. What is the minimum voltage required for electrolysis of water? Explain briefly.
Questions & Answers
QUESTION: In a hydrogen fuel cell, the steps of the chemical reaction are
\(\begin{array}{l}\text{at - electrode: } \mathrm{H}_{2}+2 \mathrm{OH}^{-} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \text{;}\\ \text{at + electrode: } \frac{1}{2} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-} \text{.}\end{array}\)
Calculate the voltage of the cell. What is the minimum voltage required for electrolysis of water? Explain briefly.
ANSWER:Step 1 of 4
In a hydrogen fuel cell, the steps of the chemical reaction are
The overall reaction is,
