what mass of iron is needed to react completely with 16 g of sulfur?
WTF!
Here is a site that is a lot of reading but it explains how to do stoichiometry problems. If you run into trouble, explain what you have done and what you don't understand.
http://www.shodor.org/UNChem/basic/stoic/
To determine the mass of iron needed to react completely with 16 g of sulfur, you need to use the balanced equation for the reaction between iron and sulfur.
The balanced equation is:
Fe + S → FeS
From the equation, we can see that 1 mole of iron (Fe) reacts with 1 mole of sulfur (S) to form 1 mole of iron sulfide (FeS).
First, we need to convert the given mass of sulfur (16 g) into moles. To do this, we use the molar mass of sulfur, which is approximately 32 g/mol.
Number of moles of sulfur = mass of sulfur / molar mass of sulfur
Number of moles of sulfur = 16 g / 32 g/mol
Number of moles of sulfur = 0.5 mol
According to the balanced equation, the mole ratio between sulfur and iron is 1:1. Therefore, 0.5 moles of sulfur will react with 0.5 moles of iron.
Now, we need to calculate the mass of iron required to react with 0.5 moles of sulfur. To do this, we need the molar mass of iron, which is approximately 56 g/mol.
Mass of iron = number of moles of iron x molar mass of iron
Mass of iron = 0.5 mol x 56 g/mol
Mass of iron = 28 g
Therefore, approximately 28 grams of iron is needed to react completely with 16 grams of sulfur.
To determine the mass of iron needed to react completely with 16 g of sulfur, we need to use the balanced chemical equation for the reaction between iron and sulfur.
The balanced chemical equation for the reaction is:
Fe + S ⟶ FeS
From the equation, we can see that one mole of iron (Fe) reacts with one mole of sulfur (S) to form one mole of iron sulfide (FeS).
First, let's calculate the number of moles of sulfur in 16 g of sulfur. To do this, we need to divide the given mass by the molar mass of sulfur (S), which is approximately 32.06 g/mol.
Number of moles of sulfur = mass of sulfur / molar mass of sulfur
= 16 g / 32.06 g/mol
≈ 0.499 mol
Since the reaction is 1:1 between iron and sulfur, we know that we also need 0.499 moles of iron to react completely with 0.499 moles of sulfur.
Now, we can calculate the mass of iron needed using the molar mass of iron (Fe), which is approximately 55.85 g/mol.
Mass of iron = number of moles of iron × molar mass of iron
= 0.499 mol × 55.85 g/mol
≈ 27.87 g
Therefore, approximately 27.87 grams of iron are needed to react completely with 16 grams of sulfur.