In a hydrogen fuel cell, hydrogen gas and oxygen gas are combined to form water. write the balanced chemical equation describing this reaction using the lowest whole‑number coefficients.

The balanced chemical equation:

2H₂+ O₂ ----> 2H₂O

Fuel Cells use the principle of chemical reactions to produce electrical energy.

The fuel used is Hydrogen (H₂) and Oxygen (O₂) gas

There are several fuel cells that are usually distinguished based on the use of electrolytes such as Alkali fuel cells that use KOH or Molten Carbonate fuel Cell (MCFC) that uses Carbonate salts

The reaction between Hydrogen and Oxygen will produce electricity and water vapor (H₂O)

The reaction occurs at the electrode (cathode and anode)

Oxygen (O₂) will function as a cathode, while Hydrogen (H₂) will function as an anode

Reaction on the electrode:

Cathode: O₂ + 4H⁺ + 4e⁻ ---> 4H₂O

Anode: 2H₂ ----> 4H⁺ + 4e⁻

Reduction reactions occur at the cathode and oxidation reactions occur at the anode, as is generally with electrochemical cells

The reaction of the cathode and anode above if added together is the balanced chemical equation of the reaction of Hydrogen (H₂) and Oxygen (O₂)

2H₂ + O₂ ----> 2H₂O

Or we can also use the principle of atomic balance, then the reaction between H₂ and O₂ is based on the similarity of the number of atoms where the number of atoms = coefficient × index (subscript) between reactant and product, and use variables on the reaction coefficient

aH₂ + bO₂ ---> 1H₂O

the number of H left =2a, right =2 ---> 2a = 2---> a = 1

the number of O left = 2b, right 1 ---> 2b = 1 ---> b = 1/2

so the reaction becomes

we multiply 2 so that the coefficient becomes an integer (whole number)

2H₂ + O₂ ⇒ 2H₂O -> balance

the combustion of octane in gasoline

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hydrogen and excess oxygen

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