Sulphur forms the chlorides `S_(2)Cl_(2)` and `SCl_(2)`. The equivalent mass of sulphur in `SCl_(2)` is

Options

A. 8g/mol
B. 16g/mol
C. 64.8g/mol
D. 3g/mol

Answer

To find the equivalent mass of sulfur in the compound \( SCl_2 \), we will 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:
\[ \text{Equivalent mass} = \frac{\text{Molecular mass}}{\text{Valency factor}} \]
Where the molecular mass is the mass of the compound and the valency factor is determined by the number of moles of electrons transferred or the change in oxidation state.

### Step 2: Determine the molecular mass of \( SCl_2 \)
First, we need to calculate the molecular mass of \( SCl_2 \):
- The atomic mass of sulfur (S) is approximately 32 g/mol.
- The atomic mass of chlorine (Cl) is approximately 35.5 g/mol.
- Since there are 2 chlorine atoms in \( SCl_2 \), the molecular mass is calculated as follows:
\[ \text{Molecular mass of } SCl_2 = \text{Atomic mass of S} + 2 \times \text{Atomic mass of Cl} = 32 + 2 \times 35.5 = 32 + 71 = 103 \text{ g/mol} \]

### Step 3: Determine the valency factor of sulfur in \( SCl_2 \)
Next, we need to find the valency factor for sulfur in \( SCl_2 \). The oxidation state of chlorine is -1. Since there are two chlorine atoms, the total contribution from chlorine is -2. For the compound to be neutral:
\[ \text{Oxidation state of S} + 2 \times (-1) = 0 \]
Let the oxidation state of sulfur be \( x \):
\[ x - 2 = 0 \implies x = +2 \]
Thus, the valency factor of sulfur in \( SCl_2 \) is 2.

### Step 4: Calculate the equivalent mass of sulfur
Now we can calculate the equivalent mass of sulfur using the formula:
\[ \text{Equivalent mass} = \frac{\text{Molecular mass of S}}{\text{Valency factor}} = \frac{32 \text{ g/mol}}{2} = 16 \text{ g/mol} \]

### Conclusion
The equivalent mass of sulfur in \( SCl_2 \) is \( 16 \text{ g/mol} \).

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