Read the following passage and answer the next five questions based on it.(32-36)

Battery or cell converts chemical energy of the redox reaction to electrical energy. In fuel cells (a galvanic cell), the chemical energy of combustion of fuels like H2, ethanol, etc., is directly converted to electrical energy. In a fuel cell, H2 and O2 react to produce electricity, where H2
gas is oxidized at the anode and oxygen is reduced at the cathode, and the reactions involved are:

Anode reaction:H₂ + 2OH⁻ → 2H₂O+2e⁻
Cathode reaction:O₂ + 2H₂O +4e⁻ → 4OH⁻

67.2 L of H2 at STP reacts in 15 minutes.

The number of moles of electrons produced in the oxidation of 67.2 L of H2 at STP is

The correct option is 6 moles.

Step-by-step Explanation:

Step 1: Calculate the number of moles of hydrogen gas (H₂) reacting at STP
At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies a volume of 22.4 liters.
Given volume of H₂ gas = 67.2 L
We can find the number of moles using the formula:
$$\text{Number of moles of}{H}_2=\frac{\text{Volume of gas at STP}}{\text{Molar volume at STP}}$$
Substituting the given values:
$$\text{Number of moles of}{H}_2=\frac{67.2\text{L}}{22.4\text{L/mol}}=3\text{moles}$$

Step 2: Determine the moles of electrons produced from the oxidation reaction
The oxidation half-reaction occurring at the anode of the fuel cell is:
H₂ + 2OH^- → 2H₂O + 2e^-
From this balanced chemical equation, we can see that:
1 mole of H₂ gas produces 2 moles of electrons (e^-) upon oxidation.

Step 3: Calculate the total moles of electrons produced by 3 moles of H₂
Since 1 mole of H₂ produces 2 moles of electrons:
$$\text{Total moles of electrons}=3\text{moles of}{H}_2\times 2\text{moles of}{e}^{-}\text{/mole of}{H}_2=6\text{moles}$$
Therefore, the oxidation of 67.2 L of H₂ at STP produces 6 moles of electrons.