If sulphur is in success then production of 2 moles of ferrous sulfide requires how many grams of iron?

Fe + S ---> FeS

so two mols of FeS needs 2 moles of iron
One mol iron = 55.847 grams
2 * 55.847 = ?????
By the way I think you mean " excess " of sulphur.

Well, if sulphur is in "success," I hope it's doing well! As for your question, to determine the number of grams of iron required to produce 2 moles of ferrous sulfide, we need to know the molar mass of iron. Once we have that, we can proceed with the calculations. So, do you know the molar mass of iron, or should I just wing it and hope for the best?

To determine how many grams of iron are required to produce 2 moles of ferrous sulfide, we need to know the molar ratio between iron (Fe) and ferrous sulfide (FeS).

The balanced chemical equation for the reaction between iron and sulphur to form ferrous sulfide is:

4 Fe + S₂ → 4 FeS

From the balanced equation, we can see that 4 moles of iron react with 1 mole of sulfur to produce 4 moles of ferrous sulfide.

So, the molar ratio between iron and ferrous sulfide is 4:4 or 1:1.

Therefore, if the production of 2 moles of ferrous sulfide requires 2 moles of iron.

Now, to calculate the grams of iron needed, we can use the molar mass of iron, which is approximately 55.85 g/mol.

The calculation is as follows:

Grams of iron = moles of iron × molar mass of iron
= 2 moles × 55.85 g/mol
= 111.7 grams

Therefore, to produce 2 moles of ferrous sulfide, we would need approximately 111.7 grams of iron.

To determine the number of grams of iron needed to produce 2 moles of ferrous sulfide, we need to know the molar mass of ferrous sulfide (FeS).

The molar mass of FeS can be calculated by adding the atomic masses of iron (Fe) and sulfur (S). According to the periodic table, the atomic mass of iron is approximately 55.845 g/mol, and the atomic mass of sulfur is approximately 32.06 g/mol.

So, the molar mass of FeS = (atomic mass of Fe) + (atomic mass of S)
= 55.845 + 32.06
≈ 87.905 g/mol

Since 2 moles of ferrous sulfide are required, we can use the molar mass to convert moles to grams.

Number of grams = (Number of moles) x (Molar mass)
= 2 mol x 87.905 g/mol
≈ 175.81 g

Therefore, to produce 2 moles of ferrous sulfide, approximately 175.81 grams of iron are needed.