Ask Question
12 October, 09:45

A powder contains FeSO4 · 7 H2O (molar mass = 278.01 g/mol), among other components. A 3.055 g sample of the powder was dissolved in HNO, and heated to convert all iron to Fe3+. The addition of NH, precipitated Fe, Oz · xH, O, which was subsequently ignited to produce 0.294 g Fe2O3. What was the mass of FeSO4 · 7H2O in the 3.055 g sample?

+2
Answers (1)
  1. 12 October, 11:41
    0
    The mass of FeSO4*7H2O is 1.023 grams

    Explanation:

    Step 1: Data given

    Molar mass of FeSO4 * 7H2O = 278.01 g/mol

    Mass of Fe2O3 = 0.294 grams

    Mass of the sample = 3.055 grams

    Step 2: The balanced equation

    4 Fe + 3O2 → 2Fe2O3

    Step 3: Calculate moles Fe2O3

    Moles Fe2O3 = mass Fe2O3 / molar mass Fe2O3

    Moles Fe2O3 = 0.294 grams / 159.59 g/mol

    Moles Fe2O3 = 0.00184 moles

    Step 3: Calculate moles Fe

    In 2 moles Fe2O3 we have 4 moles Fe

    For 0.00184 moles we'll have 2*0.00184 = 0.00368 moles

    Step 4: The balanced equation

    Fe + H2SO4 + 7H2O → FeSO4*7H20 + H2

    Step 5: Calculate moles FeSO4 * 7H2O

    For 1 mol Fe we have 1 mol FeSO4*7H2O

    For 0.00368 moles Fe we have 0.00368 moles FeSO4*7H2O

    Step 6: Calculate the mass of FeSO4*7H2O

    Mass FeSO4*7H2O = moles * molar mass

    Mass FeSO4*7H2O = 0.00368 moles * 278.01 g/mol

    Mass FeSO4*7H2O = 1.023 grams

    The mass of FeSO4*7H2O is 1.023 grams
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A powder contains FeSO4 · 7 H2O (molar mass = 278.01 g/mol), among other components. A 3.055 g sample of the powder was dissolved in HNO, ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers