Some metals can react directly with sulfur when heated. In one reaction, 32.0 g of sulfur (relative atomic mass of 32.0) combine completely with a metal, M (relative atomic mass of 40.0) to give a product with a mass of 52.0 g. Determine the empirical formula of the sulfide formed.

To determine the empirical formula of the sulfide formed, we need to find the ratio of the number of moles of the metal to the number of moles of sulfur in the product.

Step 1: Calculate the number of moles of sulfur and the metal.

• The number of moles of sulfur is given by the mass of sulfur divided by its relative atomic mass. So, the number of moles of sulfur is 32.0 g / 32.0 g/mol = 1.0 mol.
• The mass of the metal can be found by subtracting the mass of sulfur from the total mass of the product. So, the mass of the metal is 52.0 g - 32.0 g = 20.0 g.
• The number of moles of the metal is then given by the mass of the metal divided by its relative atomic mass. So, the number of moles of the metal is 20.0 g / 40.0 g/mol = 0.5 mol.

Step 2: Find the ratio of the number of moles of the metal to the number of moles of sulfur.

• The ratio is 0.5 mol : 1.0 mol, which simplifies to 1 : 2.

Therefore, the empirical formula of the sulfide formed is M2S.