A current of `2A` is passed for `1.93 xx 10^(4)s ` through a molten tin salt depositing `23.8 g Sn (Aw` of `Sn=119)`. The oxidation state of `Sn` in the salt is `…………………………`.

Explanation

To find the oxidation state of tin (Sn) in the molten tin salt, we can follow these steps:

### Step 1: Calculate the total charge (Q) passed through the salt.
The charge can be calculated using the formula:
\[ Q = I \times t \]
Where:
- \( I \) = current in amperes (A)
- \( t \) = time in seconds (s)

Given:
- \( I = 2 \, \text{A} \)
- \( t = 1.93 \times 10^4 \, \text{s} \)

Calculating \( Q \):
\[ Q = 2 \, \text{A} \times 1.93 \times 10^4 \, \text{s} = 3.86 \times 10^4 \, \text{C} \]

### Step 2: Convert the charge to Faraday (F).
Using the conversion factor \( 1 \, \text{F} = 96500 \, \text{C} \):
\[ \text{Charge in Faraday} = \frac{Q}{96500} \]
Calculating:
\[ \text{Charge in Faraday} = \frac{3.86 \times 10^4}{96500} \approx 0.4 \, \text{F} \]

### Step 3: Relate the charge to the moles of electrons.
Using Faraday's laws of electrolysis, we know that:
- 1 mole of electrons corresponds to 1 Faraday.
- The number of moles of electrons (n) can be calculated as:
\[ n = \text{Charge in Faraday} = 0.4 \, \text{F} \]

### Step 4: Determine the moles of tin deposited.
The mass of tin deposited is given as \( 23.8 \, \text{g} \) and the atomic weight of tin (Sn) is \( 119 \, \text{g/mol} \). We can calculate the moles of tin (Sn) deposited:
\[ \text{Moles of Sn} = \frac{\text{mass}}{\text{molar mass}} = \frac{23.8 \, \text{g}}{119 \, \text{g/mol}} \approx 0.2 \, \text{mol} \]

### Step 5: Relate the moles of tin to the moles of electrons.
From the electrochemical reaction:
\[ \text{Sn}^{x+} + x \, e^- \rightarrow \text{Sn} \]
1 mole of Sn is produced by \( x \) moles of electrons. Therefore, for 0.2 moles of Sn, the moles of electrons required would be:
\[ \text{Moles of electrons} = 0.2 \, \text{mol Sn} \times x \]

### Step 6: Set up the equation to find x.
From the charge passed, we know:
\[ n = 0.4 = 0.2 \times x \]
Solving for \( x \):
\[ x = \frac{0.4}{0.2} = 2 \]

### Step 7: Determine the oxidation state of tin.
The oxidation state of tin in the salt is \( +2 \).

### Final Answer:
The oxidation state of Sn in the salt is \( +2 \).

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