Read the following passage and answer the next five questions based on it:

Battery or cell converts chemical energy of the redox reaction to electrical energy. In fuel cell (a galvanic cell), the chemical energy of combustion of fuels like \(H_2\), ethanol, etc, are directly converted to electrical energy. In a fuel cell, \(H_2\) and \(O_2\) react to produce electricity, where \(H_2\) gas is oxidized at anode and oxygen is reduced at cathode and the reactions involved are:

Anode Reaction :\(H_2 + 2OH^- \longrightarrow 2H_2O + 2e^-\)

Cathode reaction: \(O_2 + 2H_2O + 4e^- \longrightarrow 4OH^-\)

\(67.2 L\) of \(H_2\) at STP reacts in \(15 \) minutes

The number of moles of hydrogen oxidized is:

3.0 moles

The correct answer is option 3. 3.0 moles.

To determine the number of moles of hydrogen (\(H_2\)) oxidized in the fuel cell, we need to use the given volume of \(H_2\) gas and the conditions provided.

The conditions specify that \(67.2 \, \text{L}\) of \(H_2\) gas reacts at standard temperature and pressure (STP). At STP, 1 mole of any ideal gas occupies \(22.4 \, \text{L}\).

Using this information, we can calculate the number of moles of \(H_2\) as follows:

\(\text{Number of moles of } H_2 = \frac{\text{Volume of } H_2}{\text{Volume of 1 mole at STP}} = \frac{67.2 \, \text{L}}{22.4 \, \text{L/mol}}\)

\(\text{Number of moles of } H_2 = 3.0 \, \text{moles}\)

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

The correct answer is: 3. 3.0 moles