Calculate the mass of iron and sulfur required to form 132 g of iron (II) sulfide

Let’s implement the solution:
1. According to the condition of the problem, we compose the equation:
Fe + S = FeS – compounds occur when heated, iron sulfide is obtained (2);
2. Let’s make the calculations:
M (Fe) = 55.8 g / mol.
M (FeS) = 87.8 g / mol.
3. Define Y of the product:
Y (FeS) = m / M = 132 / 87.8 = 1.5 mol.
Y (Fe) = 1.5 mol.
Y (S) = 1.5 mol since the quantities of substances according to the equation are equal to 1 mol.
4. Find the mass of the starting materials:
m (Fe) = Y * M = 1.5 * 55.8 = 83.7 g;
m (S) = Y * M = 1.5 * 32 = 48 g.
Answer: to carry out the process, you will need iron weighing 83.7 g, sulfur – 48 g.