In the electrolysis of acidulated water, it is desired to obtain 1.12 cc of hydrogen per second under STP condition. The current to be passed is:

Options

A. `1.93A`
B. `9.65`
C. `19.3A`
D. `0.965`

Explanation

To solve the problem of determining the current required to obtain 1.12 cc of hydrogen per second during the electrolysis of acidulated water, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Reaction**:
In the electrolysis of water, hydrogen gas (H₂) is produced at the cathode. The half-reaction for the production of hydrogen is:
\[ 2H^+ + 2e^- \rightarrow H_2(g) \]
This means that 2 moles of electrons are required to produce 1 mole of hydrogen gas.

2. **Volume of Hydrogen at STP**:
At standard temperature and pressure (STP), 1 mole of any gas occupies 22,400 mL. Therefore, the volume of hydrogen produced from 1 mole of electrons can be calculated as follows:
\[ \text{Volume of } H_2 = \frac{22400 \text{ mL}}{2} = 11200 \text{ mL} \]
This means that 1 mole of electrons (1 Faraday) produces 11,200 mL of hydrogen.

3. **Calculate the Charge for 1.12 cc of Hydrogen**:
We need to find out how much charge is required to produce 1.12 cc (or 1.12 mL) of hydrogen. We can set up a proportion:
\[ \frac{11200 \text{ mL}}{96500 \text{ C}} = \frac{1.12 \text{ mL}}{Q} \]
Here, \( Q \) is the charge in coulombs required to produce 1.12 mL of hydrogen.

Rearranging gives:
\[ Q = \frac{1.12 \text{ mL} \times 96500 \text{ C}}{11200 \text{ mL}} \]
\[ Q = \frac{107072 \text{ C}}{11200} \approx 9.57 \text{ C} \]

4. **Calculate the Current**:
The current (I) can be calculated using the formula:
\[ Q = I \times t \]
Given that the time (t) is 1 second, we can rearrange the formula to find the current:
\[ I = \frac{Q}{t} = \frac{9.57 \text{ C}}{1 \text{ s}} \approx 9.57 \text{ A} \]

5. **Final Answer**:
Therefore, the current required to obtain 1.12 cc of hydrogen per second is approximately **9.57 A**.