We read your photo as:

Determine the empirical formula of iron(II) oxide and write a balanced equation for its formation.

Chemistry

ScanSolve AI Answer

Answer

a

Fe3O4\text{Fe}_3\text{O}_4

Step-by-step solution

6 steps

Here are the answers to your questions:

Part a· 6 steps

i) Determine the empirical formula of the oxide of iron.

  1. Calculate the mass of iron (Fe).

    Mass of iron = (Mass of empty dish + residue) - Mass of empty dish
    Mass of iron = 12.66 g−10.98 g=1.68 g12.66 \text{ g} - 10.98 \text{ g} = 1.68 \text{ g}

  2. Calculate the mass of the oxide of iron.

    Mass of oxide = (Mass of empty dish + oxide of iron) - Mass of empty dish
    Mass of oxide = 13.30 g−10.98 g=2.32 g13.30 \text{ g} - 10.98 \text{ g} = 2.32 \text{ g}

  3. Calculate the mass of oxygen (O).

    Mass of oxygen = Mass of oxide - Mass of iron
    Mass of oxygen = 2.32 g−1.68 g=0.64 g2.32 \text{ g} - 1.68 \text{ g} = 0.64 \text{ g}

  4. Convert masses to moles.

    Moles of Fe = Mass of FeMolar mass of Fe=1.68 g56.0 g/mol=0.03 mol\frac{\text{Mass of Fe}}{\text{Molar mass of Fe}} = \frac{1.68 \text{ g}}{56.0 \text{ g/mol}} = 0.03 \text{ mol}
    Moles of O = Mass of OMolar mass of O=0.64 g16.0 g/mol=0.04 mol\frac{\text{Mass of O}}{\text{Molar mass of O}} = \frac{0.64 \text{ g}}{16.0 \text{ g/mol}} = 0.04 \text{ mol}

  5. Find the simplest mole ratio.

    Divide by the smallest number of moles (0.03 mol):
    Ratio of Fe = 0.030.03=1\frac{0.03}{0.03} = 1
    Ratio of O = 0.040.03≈1.333\frac{0.04}{0.03} \approx 1.333

    To get whole numbers, multiply by 3:
    Fe ratio = 1×3=31 \times 3 = 3
    O ratio = 1.333×3=41.333 \times 3 = 4

  6. Write the empirical formula.

    The empirical formula is Fe3O4\boxed{\text{Fe}_3\text{O}_4}.

Part a(ii)

Write an equation for the reaction which took place in the combustion tube.

The reaction is the formation of iron(II,III) oxide from iron and oxygen.

3Fe(s)+2O2(g)→Fe3O4(s)3\text{Fe(s)} + 2\text{O}_2\text{(g)} \rightarrow \text{Fe}_3\text{O}_4\text{(s)}

Part b(i)

Two conditions necessary for rusting to occur

Corrosive is a destructive process in which iron is converted into hydrated iron (III) oxide.

  • Oxygen (or air)
  • Water (or moisture)

Part b(ii)

Two methods used to protect iron from rusting other than painting

  • Galvanizing (coating iron with a layer of zinc)
  • Oiling/Greasing (applying a layer of oil or grease to prevent contact with air and water)

Part c

Explain why it is not advisable to wash vehicles using seawater.

Seawater contains dissolved salts, which act as electrolytes. These electrolytes increase the electrical conductivity of the water, thereby accelerating the rate of rusting (corrosion) of the metal parts of the vehicle.

Was this helpful?

Try one yourself

A new problem that tests the same skill.

Still stuck on this one?

Ask a follow-up, and the answer starts from this question.

Got a different question?Ask your own question

More Chemistry Questions

QDetermine the molecular mass of iron III oxideQCalculate the mass of iron produced from 20 g of 50% pure Fe2O3 and 9 g of CO, given the reaction…QDetermine the limiting reactant, excess reactant, and the mass of iron(II) sulfide (FeS) produced…QDescribe how to prepare pure lead(II) carbonate from lead(II) oxide. Include chemical equations.QBalance the chemical equation for the reaction between copper (II) oxide and sulfuric acid and…
See all Chemistry questions →
Got a syllabus? Photograph it and I'll tell you what's due and what's worth the most.