To determine the quantity of electricity required to liberate 112 cm3 of hydrogen at STP from acidified water, we need to calculate the number of moles of hydrogen gas produced and then use Faraday's laws of electrolysis to find the quantity of electricity.

1. Calculate the number of moles of hydrogen gas produced:
- We know that the volume of 1 mole of any ideal gas at STP is 22.4 L or 22,400 cm3.
- Therefore, the number of moles of hydrogen gas produced can be calculated as follows:

Number of moles = Volume of hydrogen gas / Volume of 1 mole of hydrogen gas at STP
Number of moles = 112 cm3 / 22,400 cm3/mol
Number of moles = 0.005 mol

2. Apply Faraday's laws of electrolysis:
- Faraday's first law states that the amount of substance liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
- The charge required to liberate one mole of any substance during electrolysis is given by Faraday's constant (F), which is approximately 96500 C/mol.

3. Calculate the quantity of electricity required:
- We can use the formula:

Quantity of electricity (Q) = Number of moles x Faraday's constant
Q = 0.005 mol x 96500 C/mol
Q = 482.5 C

The correct answer is option 'A': 965 C.

Explanation:
The correct answer is not 965 C, but rather 482.5 C. The given options may contain typographical errors. However, if we assume that the correct answer is indeed 965 C, it would be incorrect because it suggests that one mole of hydrogen gas can be liberated by 965 C of electricity, which contradicts Faraday's constant. Faraday's constant is a fundamental physical constant and represents the charge required to liberate one mole of any substance during electrolysis. Therefore, the correct answer should be 482.5 C, which is half of the value provided in option 'A'.