How many moles of iron(II)sulfide are produced when 4.38g of Fe reacts with 2.88g of S to produce iron(II)sulfide?
This is a limiting reagent problem.
Write the equation and balance it.
16Fe + 3S8 ==> 8Fe2S3
Convert 4.38 g Fe to mols. mols = g/molar mass.
Convert 2.88 g S8 to mols S8.
a.Using the coefficients in the balanced equation, convert mols Fe to mols Fe2S3.
b. Same thing but convert mols S8 to mols Fe2S3.
c. The smaller number of mols of Fe2S3 is the correct one to choose and the reactant that produced that is the limiting reagent.
The number in c x molar mass = grams Fe2S3.
Post your work if you get stuck.
To determine the number of moles of iron(II) sulfide produced, we need to follow these steps:
1. Convert the mass of Fe and S to moles.
2. Determine the mole ratio between Fe and FeS.
3. Calculate the number of moles of FeS.
Step 1: Convert the mass of Fe and S to moles.
To do this, we need to divide the given mass by the molar mass of each element. The molar mass of Fe is 55.85 g/mol, and the molar mass of S is 32.07 g/mol.
For Fe:
Moles of Fe = Mass of Fe / Molar mass of Fe
Moles of Fe = 4.38 g / 55.85 g/mol
For S:
Moles of S = Mass of S / Molar mass of S
Moles of S = 2.88 g / 32.07 g/mol
Step 2: Determine the mole ratio between Fe and FeS.
The balanced chemical equation for the reaction between Fe and S is:
Fe + S → FeS
From the equation, we can see that the mole ratio between Fe and FeS is 1:1. This means that for every 1 mole of Fe, we produce 1 mole of FeS.
Step 3: Calculate the number of moles of FeS.
Since the mole ratio is 1:1, the number of moles of FeS produced is the same as the number of moles of Fe.
Moles of FeS = Moles of Fe
Now, we can substitute the values we calculated in step 1 into the equation:
Moles of FeS = 4.38 g / 55.85 g/mol
Calculating this value will give you the number of moles of FeS produced when 4.38 g of Fe reacts with 2.88 g of S.