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.

If the entire current produced is used for the electrodeposition of silver (atomic weight = 108 g/mol) from Silver (I) solution, the amount of silver deposited will be:

The correct option is 648 g.

Step-by-Step Explanation:

1. Calculate the number of moles of hydrogen gas (H₂) reacting:
We are given that 67.2 L of H₂ gas at STP (Standard Temperature and Pressure) reacts. Since 1 mole of any ideal gas occupies 22.4 L at STP, we can find the number of moles of H₂ using the formula:

$\text{Moles of}{\text{H}}_2=\frac{67.2\text{L}}{22.4\text{L/mol}}=3\text{moles}$

2. Determine the total moles of electrons produced at the anode:
According to the given anode half-reaction:
H₂ + 2OH^- → 2H₂O + 2e^-
Each mole of H₂ oxidized produces 2 moles of electrons. Therefore, 3 moles of H₂ will produce:

$\text{Moles of electrons}=3\times 2=6\text{moles of electrons}$

3. Relate the moles of electrons to the electrodeposition of silver:
The reduction of silver ions from a Silver (I) solution is given by the reaction:
Ag⁺ + e^- → Ag
This equation shows that 1 mole of electrons is required to deposit 1 mole of silver (Ag). Therefore, 6 moles of electrons will deposit 6 moles of silver.

4. Calculate the mass of silver deposited:
Using the atomic weight of silver (108 g/mol), the mass of silver deposited is calculated as:

$\text{Mass of Ag deposited}=6\text{moles}\times 108\text{g/mol}=648\text{g}$

Thus, the amount of silver deposited is 648 g.