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When 2.56 g of sulphur was dissolved in ...

When 2.56 g of sulphur was dissolved in 100 g of `CS_(2)`, the freezing point lowered by 0.383 K. Calculate the formula of sulphur `(S_(x))`.
(`K_(f)` for `CS_(2)` = 3.83 K kg `mol^(-1)`, Atomic mass of sulphur = 32g `mol^(-1)`]

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AI Generated Solution

To solve the problem step by step, we will use the formula for freezing point depression and the information provided in the question. ### Step 1: Write down the formula for freezing point depression. The freezing point depression (\( \Delta T_f \)) is given by the formula: \[ \Delta T_f = K_f \times m \] where: ...
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