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 hydrogen oxidized is:

The correct option is 3.0 moles.

Step-by-step Explanation:

According to the passage, the volume of hydrogen gas (H₂) reacting at Standard Temperature and Pressure (STP) is 67.2 L.

By definition, 1 mole of any ideal gas occupies a volume of 22.4 L at STP (Standard Temperature and Pressure). To find the number of moles of hydrogen gas oxidized, we can use the relation between the volume of a gas at STP and its number of moles:

$$\text{Number of moles of}{H}_2=\frac{\text{Given volume of gas at STP (L)}}{\text{Molar volume of gas at STP (L/mol)}}$$

Now, we substitute the given values into the equation:

$$\text{Number of moles of}{H}_2=\frac{67.2\text{L}}{22.4\text{L/mol}}$$

Solving the division gives:

$$\text{Number of moles of}{H}_2=3.0\text{moles}$$

Therefore, the number of moles of hydrogen oxidized is 3.0 moles.