How many moles of Fe2S3 are produced from a 0.4g piece of Fe?
.4g = .00716 moles
each mole of Fe2S3 requires 2 moles Fe, so we only get
.00358 moles Fe2S3
To determine the number of moles of Fe2S3 produced from a 0.4g piece of Fe, we need to follow these steps:
1. Find the molar mass of Fe:
The atomic mass of Fe is 55.845 g/mol.
2. Convert the mass of Fe to moles:
Divide the mass of Fe by its molar mass.
moles of Fe = mass of Fe / molar mass of Fe
moles of Fe = 0.4 g / 55.845 g/mol
3. Determine the stoichiometry between Fe and Fe2S3:
The balanced chemical equation for the reaction between Fe and Fe2S3 should be given.
Assuming the stoichiometry is 2Fe + 3S → Fe2S3, we can use the mole ratio here.
moles of Fe2S3 = moles of Fe × (moles of Fe2S3 / moles of Fe)
moles of Fe2S3 = moles of Fe × (1 mole of Fe2S3 / 2 moles of Fe)
4. Calculate the final result:
Plug in the value of moles of Fe calculated in step 2 into the equation calculated in step 3.
moles of Fe2S3 = 0.4 g / 55.845 g/mol × (1 mole of Fe2S3 / 2 moles of Fe)
Calculate the value to get the final answer.
To determine how many moles of Fe2S3 are produced from a 0.4g piece of Fe, we need to follow a few steps:
Step 1: Determine the molar mass of Fe (Iron).
The molar mass of Fe is the atomic mass of Iron, which can be found on the periodic table. The atomic mass of Fe is approximately 55.85 g/mol.
Step 2: Calculate the number of moles of Fe.
To calculate the number of moles, divide the mass of Fe (0.4g) by its molar mass (55.85 g/mol):
Number of moles of Fe = Mass of Fe / Molar mass of Fe
= 0.4g / 55.85 g/mol
≈ 0.00715 mol
Step 3: Determine the stoichiometry of the reaction.
The balanced chemical equation is needed to determine the stoichiometry of the reaction. If the equation is not provided, we cannot determine how many moles of Fe2S3 are produced.
However, assuming the reaction is balanced as follows:
8Fe + 3S → 4Fe2S3,
we can deduce that 8 moles of Fe react with 3 moles of sulfur to produce 4 moles of Fe2S3.
Step 4: Calculate the number of moles of Fe2S3 produced.
Using the stoichiometry of the reaction, we can determine the number of moles of Fe2S3 produced from the known number of moles of Fe:
Number of moles of Fe2S3 = (Number of moles of Fe / 8 moles) × 4 moles
= (0.00715 mol / 8 mol) × 4 mol
≈ 0.00358 mol
Therefore, approximately 0.00358 moles of Fe2S3 are produced from a 0.4g piece of Fe.