A weighed portion of 1.12 g of iron was completely “dissolved” in a solution of copper (II) sulfate.
| January 17, 2021 | education
A weighed portion of 1.12 g of iron was completely “dissolved” in a solution of copper (II) sulfate. Calculate the mass of the copper precipitate formed. What amount of iron (II) sulfate was obtained in this case?
Given:
m (Fe) = 1.12 g
To find:
n (FeSO4)
Decision:
CuSO4 + Fe = FeSO4 + Cu
n (Fe) = m / M = 1.12 g / 56 g / mol = 0.02 mol
n (Fe): n (FeSO4) = 1: 1
n (FeSO4) = 0.02 mol
Answer: 0.02 mol
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