If 1.888 g of bismuth metal reacts with sulfur to give 2.323 g of bismuth sulfide,what is the empirical formula of the product?

Question

Quizplus · Accepted Answer

To find the empirical formula, calculate the moles of Bi and S. The mass of S is 2.323 g - 1.888 g = 0.435 g. Moles of Bi = 1.888 g / 208.98 g/mol = 0.00903 mol. Moles of S = 0.435 g / 32.07 g/mol = 0.01357 mol. The mole ratio of Bi:S is approximately 2:3, leading to the empirical formula Bi₂S₃.

If 1888 G of Bismuth Metal Reacts with Sulfur to Give