Sulphur forms two chlorides `S_(2) Cl_(2)` and `SCl_(2)`. The equivalent mass of sulphur in `SCl_(2)` is `16 g//`mole. The equivalent mass of sulphur in `S_(2) Cl_(2) `is -

Options

A. `8 g //` mole
B. `16 g //` mole
C. `48 g //` mole
D. `32 g //` mole

Answer

To determine the equivalent mass of sulfur in the compound \( S_2Cl_2 \), we can follow these steps:

### Step 1: Understand the concept of equivalent mass
The equivalent mass of an element in a compound is calculated using the formula:
\[ \text{Equivalent mass} = \frac{\text{Atomic mass}}{\text{Valency}} \]
Where:
- Atomic mass of sulfur (S) = 32 g/mol
- Valency is determined based on the oxidation state of sulfur in the compound.

### Step 2: Determine the oxidation state of sulfur in \( S_2Cl_2 \)
In the compound \( S_2Cl_2 \):
- Let the oxidation state of sulfur be \( x \).
- The oxidation state of chlorine (Cl) is -1.

The overall charge of the compound is neutral, so we can set up the equation:
\[ 2x + 2(-1) = 0 \]
This simplifies to:
\[ 2x - 2 = 0 \]
Solving for \( x \):
\[ 2x = 2 \implies x = 1 \]
Thus, the oxidation state of sulfur in \( S_2Cl_2 \) is +1.

### Step 3: Calculate the valency of sulfur in \( S_2Cl_2 \)
The valency of sulfur corresponds to its oxidation state, which we found to be +1. Therefore, the valency of sulfur in \( S_2Cl_2 \) is 1.

### Step 4: Calculate the equivalent mass of sulfur in \( S_2Cl_2 \)
Using the equivalent mass formula:
\[ \text{Equivalent mass of sulfur} = \frac{\text{Atomic mass of sulfur}}{\text{Valency}} = \frac{32 \text{ g/mol}}{1} = 32 \text{ g/equiv} \]

### Final Answer
The equivalent mass of sulfur in \( S_2Cl_2 \) is **32 g/equiv**.

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