Answer:

Calculation of Quantity of Electricity:
The balanced equation for the reduction of nitrobenzene to aniline is:

C6H5NO2 + 6H+ + 6e- → C6H5NH2 + 2H2O

From the equation, we can see that 6 electrons are required to reduce one molecule of nitrobenzene to aniline. The molecular weight of nitrobenzene is 123.11 g/mol. Therefore, the number of moles of nitrobenzene can be calculated as:

n = 12.3 g / 123.11 g/mol = 0.0999 mol

Since 6 electrons are required per molecule of nitrobenzene, the total number of electrons required can be calculated as:

N = 6 × 0.0999 mol × 6.022 × 10^23 mol^-1 = 3.596 × 10^23 electrons

The Faraday constant (F) is the charge on one mole of electrons, and it is equal to 96,485 C/mol. Therefore, the quantity of electricity required to reduce 12.3 g of nitrobenzene can be calculated as:

Q = (3.596 × 10^23 electrons) × (1 F/96,485 C) = 3.725 × 10^19 C

However, the current efficiency for the process is given as 50%, which means that only half of the electrons supplied will contribute to the reduction of nitrobenzene. Therefore, the actual quantity of electricity required can be calculated as:

Q_actual = Q / (current efficiency) = 3.725 × 10^19 C / 0.5 = 7.45 × 10^19 C

Therefore, the quantity of electricity required to reduce 12.3 g of nitrobenzene to aniline is 7.45 × 10^19 C.

Calculation of Number of Faradays:
One Faraday is equal to the amount of electricity required to deposit one mole of metal from its ion. In this case, we are not depositing any metal, but we are reducing nitrobenzene to aniline. However, we can still use the concept of Faraday to calculate the number of electrons required for complete conversion.

From the balanced equation, we know that 6 electrons are required per molecule of nitrobenzene. Therefore, the total number of electrons required for complete conversion can be calculated as:

N_total = 6 × 0.0999 mol × 6.022 × 10^23 mol^-1 = 3.596 × 10^23 electrons

The number of Faradays required for complete conversion can be calculated as:

F_total = N_total / (Avogadro's number × 1 mol) = 3.596 × 10^23 electrons / (6.022 × 10^23 electrons/mol) = 0.598 Faradays

Therefore, the number of Faradays required for complete conversion is 0.6 (rounded up to the first decimal place).