Write the balanced half‑reaction that occurs at the anode in a hydrogen‑oxygen fuel cell in which an acidic electrolyte is used. A hydrogen fuel cell. H 2 flows into the cell at the negative electrode. O 2 flows into the cell at the positive electrode. Electrons travel through an external circuit from the negative to the positive electrode. Between the two electrodes is an electrolyte solution. Arrows in the electrolyte point from the negative electrode to the positive electrode. anode half-reaction: Write the balanced half‑reaction that occurs at the cathode in a hydrogen‑oxygen fuel cell in which an acidic electrolyte is used. cathode half-reaction: Write the balanced overall cell reaction. overall cell reaction:

A hydrogen-oxygen fuel cell is an alternative cell to rechargeable cells and batteries. In this cell, hydrogen and oxygen is used to produce voltage and water is the only byproduct.

At the cathode (positive electrode):

O2 + 4H+ +4e--------> 2H2O

At the anode (negative electrode);

2H2 -4e- ---------> 4H+

Adding the two half reactions we have:

2H2 + O2 + 4H+ + 4e- -----------> 2H2O + 4H + 4e-

The overall reaction after cancelling out the like terms in the reaction is:

2H2 (g) + O2 (g) --------> 2H2O (l)

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-11-20T08:00:42+01:00

The hydrogen fuel cell is an electrochemical cell in which hydrogen is oxidized and oxygen is reduced.

A fuel cell is an electrochemical cell in which oxygen enters into the positive cathode and hydrogen flows into the negative cathode. Hydrogen is oxidized and oxygen is reduced during the electrochemical reaction.

At the negative electrode;

2H2(g) -----> 4H^+(aq)+ 4e

At the positive electrode;

O2(g) + 4H^+(aq) + 4e -----> 2H2O(l)

The overall reaction is;

2H2(g) + O2(g) -----> 4H^+(aq) + 2H2O(l)

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