1.6 g of an organic compound containing sulphur,produces 0.233 g of `BaSO_(4)`. Calculate % of S in the organic compound . (Given : Atomic weight of Ba = 137 )

Answer

To calculate the percentage of sulfur (S) in the organic compound, we can follow these steps:

### Step 1: Calculate the molar mass of barium sulfate (BaSO₄)
The molar mass of BaSO₄ can be calculated using the atomic weights of its constituent elements:
- Atomic weight of Ba = 137 g/mol
- Atomic weight of S = 32 g/mol
- Atomic weight of O = 16 g/mol

The formula for BaSO₄ is:
\[ \text{Molar mass of BaSO}_4 = \text{Ba} + \text{S} + 4 \times \text{O} \]
\[ = 137 + 32 + 4 \times 16 \]
\[ = 137 + 32 + 64 \]
\[ = 233 \text{ g/mol} \]

### Step 2: Determine the mass of sulfur in the barium sulfate produced
We know that 0.233 g of BaSO₄ is produced. To find the mass of sulfur in this amount, we can set up a proportion based on the molar mass:
- The molar mass of BaSO₄ corresponds to 32 g of sulfur.

Using the proportion:
\[ \text{Mass of S} = \left( \frac{32 \text{ g}}{233 \text{ g}} \right) \times 0.233 \text{ g} \]

Calculating this gives:
\[ \text{Mass of S} = \frac{32}{233} \times 0.233 \]
\[ \approx 0.032 \text{ g} \]

### Step 3: Calculate the percentage of sulfur in the organic compound
Now that we have the mass of sulfur, we can find the percentage of sulfur in the original organic compound:
\[ \text{Percentage of S} = \left( \frac{\text{Mass of S}}{\text{Mass of organic compound}} \right) \times 100 \]
\[ = \left( \frac{0.032 \text{ g}}{1.6 \text{ g}} \right) \times 100 \]
\[ = 0.02 \times 100 \]
\[ = 2\% \]

### Final Answer
The percentage of sulfur in the organic compound is **2%**.

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