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

### Step 1: Convert Time to Seconds
First, we need to convert the time from minutes to seconds since the standard unit for time in electrochemistry is seconds.

\[ t = 30 \text{ minutes} \times 60 \text{ seconds/minute} = 1800 \text{ seconds} \]

### Step 2: Calculate Charge (Q)
Using the formula for charge, which is given by:

\[ Q = I \times t \]

where \(I\) is the current in amperes and \(t\) is the time in seconds:

\[ Q = 1 \text{ A} \times 1800 \text{ s} = 1800 \text{ coulombs} \]

### Step 3: Use Faraday's Law
According to Faraday's law, 1 Faraday (F) of charge (which is 96500 coulombs) will liberate a certain amount of substance. For chlorine (Cl₂), the equivalent weight is 35.5 g (for Cl) and since Cl₂ consists of 2 chlorine atoms, the equivalent weight for Cl₂ is:

\[ \text{Equivalent weight of Cl₂} = \frac{35.5 \text{ g}}{1} = 35.5 \text{ g} \]

### Step 4: Calculate the Mass of Cl₂ Produced
From the above, we can find out how much mass of Cl₂ is produced per coulomb:

\[ \text{Mass of Cl₂ per coulomb} = \frac{35.5 \text{ g}}{96500 \text{ C}} \]

Now, we can find the mass of Cl₂ produced by the total charge of 1800 coulombs:

\[ \text{Mass of Cl₂} = \left(\frac{35.5 \text{ g}}{96500 \text{ C}}\right) \times 1800 \text{ C} \]

Calculating this gives:

\[ \text{Mass of Cl₂} = \frac{35.5 \times 1800}{96500} \approx 0.66 \text{ g} \]

### Final Answer
The mass of Cl₂ produced when 1 A current is passed through NaCl solution for 30 minutes is approximately **0.66 grams**.

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