Question

If 0.250 mol of red phosphorus reacts with 0.375 mol of yellow sulfur, what is the empirical formula of the product?

Answer 1

Answer on Question #43599 - Chemistry - Organic Chemistry

Question:

If 0.250 mol of red phosphorus reacts with 0.375 mol of yellow sulfur, what is the empirical formula of the product?

Answer:

Generally, when phosphorus reacts with sulfur mixture of phosphorus sulfides $(P_{x}S_{y})$ is formed. The molar ratio

$$\frac{n_{P}}{n_{S}} = \frac{0.250}{0.375} = \frac{2}{3}$$

So, the empirical formula of the product is $P_{2}S_{3}$.

By the way, phosphorus sulfide always includes 4 P atoms. So the actual formula of the product is $P_{4}S_{6}$.

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