If 0.250 mol of red phosphorus reacts with 0.625 mol of yellow sulfur,what is the empirical formula of the product?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction between red phosphorus and yellow sulfur is as follows:

4P4 + 15S8 → 8P2S5

Therefore, 0.250 mol of red phosphorus reacts with (0.625 mol ÷ 15 mol) × 4 mol = 0.167 mol of sulfur.

To find the empirical formula of the product, we need to determine the ratio of phosphorus atoms to sulfur atoms in the product. From the balanced chemical equation, we can see that there are 2 phosphorus atoms for every 5 sulfur atoms in the product.

Thus, the empirical formula of the product is P2S5, which corresponds to choice B.

If 0250 Mol of Red Phosphorus Reacts with 0