The mass of `Cl_(2)` produced when 1A current is passed through NaCl solution for 30 minute is

Options

A. 0.33g
B. 0.66g
C. 0.33 mol
D. 0.66 mol

Answer

To find the mass of Cl₂ produced when a current of 1 A is passed through an NaCl solution for 30 minutes, we can follow these steps:

### Step 1: Calculate the total charge (Q)
The total charge can be calculated using the formula:
\[ Q = I \times T \]
Where:
- \( I \) is the current in Amperes (A)
- \( T \) is the time in seconds (s)

Given:
- \( I = 1 \, A \)
- \( T = 30 \, \text{minutes} = 30 \times 60 \, \text{s} = 1800 \, \text{s} \)

Now, substituting the values:
\[ Q = 1 \, A \times 1800 \, s = 1800 \, C \]

### Step 2: Determine the number of Faradays
1 Faraday (F) is equivalent to 96500 coulombs. To find the number of Faradays (n) used, we can use the formula:
\[ n = \frac{Q}{F} \]

Substituting the values:
\[ n = \frac{1800 \, C}{96500 \, C/F} \approx 0.0186 \, F \]

### Step 3: Relate Faradays to moles of Cl₂
From electrochemistry, we know that 1 mole of Cl₂ is produced by 2 Faradays (since the reaction is:
\[ 2 \, Cl^- \rightarrow Cl_2 + 2e^- \])

Thus, the number of moles of Cl₂ produced can be calculated as:
\[ \text{moles of Cl₂} = \frac{n}{2} = \frac{0.0186}{2} \approx 0.0093 \, \text{moles} \]

### Step 4: Calculate the mass of Cl₂ produced
The molar mass of Cl₂ is approximately 71 g/mol (since Cl has a molar mass of about 35.5 g/mol).

Using the formula:
\[ \text{mass} = \text{moles} \times \text{molar mass} \]
Substituting the values:
\[ \text{mass} = 0.0093 \, \text{moles} \times 71 \, \text{g/mol} \approx 0.6613 \, g \]

### Step 5: Final result
Thus, the mass of Cl₂ produced is approximately 0.66 g.