Answer:
When 5.00 g of FeCl₃·xH₂O is heated, 2.00 g of H₂O are driven off. This means that the 2.00 g of water that was lost came from the hydrate. To find the molar ratio of water to the iron chloride in the hydrate, we can calculate the moles of each component.
Moles of H₂O lost:
Moles of H₂O = Mass (g) / Molar mass of H₂O
Moles of H₂O = 2.00 g / 18.015 g/mol (molar mass of H₂O)
Moles of H₂O ≈ 0.111 mol
Moles of FeCl₃ (iron chloride) in the hydrate:
Moles of FeCl₃ = Moles of H₂O (since they have a 1:1 molar ratio based on the balanced chemical formula of the hydrate)
Now, let's check which of the provided options matches this information:
a) FeCl₂: This is not relevant to the given information.
b) FeCl₃ x 2H₂O (Iron(III) chloride dihydrate): This option doesn't match the molar ratio of 1:1 for water and iron chloride based on the information we calculated.
c) FeCl₄ x H₂O (Iron(IV) chloride monohydrate): This option doesn't match the molar ratio either.
d) FeCl₃ x 4H₂O (Iron(III) chloride tetrahydrate): This option doesn't match the molar ratio; it has a 4:1 ratio of water to iron chloride.
None of the provided options match the molar ratio of 1:1 for water and iron chloride based on the given information. It appears that the correct chemical formula and name of the hydrate were not among the options provided.
Step-by-step explanation: