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In sulphur estimation, 0.471 g of an organic compound gave 1.4439 g of barium sulphate. The percentage of sulphur in the compound is ______ (Nearest Integer) (Given: Atomic masses Ba: 137, S: 32 u, O:16 u)

1. 42
2. 42
3. 42
4. 42

Correct answer: 42

Solution

The mass of barium sulfate produced allows us to calculate the amount of sulfur in the original compound using stoichiometry. Since the molar mass of barium sulfate (BaSO4) is 233 g/mol, we can determine the mass of sulfur from the mass of barium sulfate, leading to the conclusion that the percentage of sulfur in the compound is approximately 42%.

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