fe2so43 ra feso4

Fe + Fe2(SO4)33FeSO4

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Word Equation

Iron + Ferric Sulfate = Iron(Ii) Sulfate

One mole of solid

Iron [Fe]

and one mole of aqueous

Ferric Sulfate [Fe2(SO4)3]

combine đồ sộ size three moles of aqueous

Iron(Ii) Sulfate [FeSO4]

Reaction Type


  • Redox

Net Ionic Equation

Fe(s) + Fe2(SO4)3(aq) = 3FeSO4(aq) might be an ionic reaction. Calculate the net ionic equation for Fe(s) + Fe2(SO4)3(aq) = 3FeSO4(aq).

Redox (Oxidation-Reduction) Reaction

Fe + Fe2(SO4)3 = FeSO4 might be a redox reaction.


  • Iron - Fe

  • Ferric Sulfate - Fe2(SO4)3

    Ferric Sulfate Anhydrous Iron(Iii) Sulfate(Vi) Diiron Trisulfate Ferric Persulfate Ferric Sesquisulfate Ferric Tersulfate Iron Persulfate Iron Sesquisulfate Fe2(SO4)3 Molar Mass Fe2(SO4)3 Oxidation Number


  • Iron(Ii) Sulfate - FeSO4

    Ferrous Sulphate Iron(Ii) Sulphate (1:1) Iron(Ii) Sulphate Iron Sulphate (1:1) Ferrous Sulfate Anhydrous Fe(Ii)So4 Feso4 Iron(2+) Sulfate (Anh.) FeSO4 Molar Mass FeSO4 Oxidation Number


Thermodynamics of the reaction can be calculated using a lookup table.

Is the Reaction Exothermic or Endothermic?

Fe (s alpha)1 mol0 kJ/mol-0 kJ
Fe2(SO4)3 (s)1 mol-2581.528 kJ/mol2581.528 kJ
FeSO4 (s)3 mol-928.4296 kJ/mol-2785.2888 kJ
ΣΔH°f(reactants)-2581.528 kJ
ΣΔH°f(products)-2785.2888 kJ
ΔH°rxn-203.7608 kJ

ΣΔH°f(reactants) > ΣΔH°f(products), sánh Fe + Fe2(SO4)3 = FeSO4 is exothermic (releases heat).

Is the Reaction Exoentropic or Endoentropic?

ΔS = Sproducts - Sreactants. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.

Fe (s alpha)1 mol27.27968 J/(mol K)-27.27968 J/K
Fe2(SO4)3 (s)1 mol307.524 J/(mol K)-307.524 J/K
FeSO4 (s)3 mol120.9176 J/(mol K)362.7528 J/K
ΣΔS°(reactants)334.80368 J/K
ΣΔS°(products)362.7528 J/K
ΔS°rxn27.94912 J/K

ΣΔS°(products) > ΣΔS°(reactants), sánh Fe + Fe2(SO4)3 = FeSO4 is endoentropic (increase in entropy).

Is the Reaction Exergonic or Endergonic?

ΔG = Gproducts - Greactants. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.

Fe (s alpha)1 mol0 kJ/mol-0 kJ
Fe2(SO4)3 (s)1 mol-2263.1256 kJ/mol2263.1256 kJ
FeSO4 (s)3 mol-825.0848 kJ/mol-2475.2544 kJ
ΣΔG°(reactants)-2263.1256 kJ
ΣΔG°(products)-2475.2544 kJ
ΔG°rxn-212.1288 kJ

ΣΔG°(reactants) > ΣΔG°(products), sánh Fe + Fe2(SO4)3 = FeSO4 is exergonic (releases energy).

Reaction Expressions

Kc or Q = ( [FeSO4]3 ) / ( [Fe] [Fe2(SO4)3] )

(assuming all reactants and products are aqueous. substitutue 1 for any solids/liquids, and Psubstance for gases.)

rate = -(Δ[Fe] / Δt) = -(Δ[Fe2(SO4)3] / Δt) = 1/3 * (Δ[FeSO4] / Δt)

(assuming constant volume in a closed system and no accumulation of intermediates or side products)


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Balance Fe + Fe2(SO4)3 = FeSO4 Using the Algebraic Method

How To Balance Fe + Fe2(SO4)3 = FeSO4

To balance the equation Fe + Fe2(SO4)3 = FeSO4 using the algebraic method step-by-step, you must have experience solving systems of linear equations. The most common methods are substitution/elimination and linear algebra, but any similar method will work.

  1. Label Each Compound With a Variable

    Label each compound (reactant or product) in the equation with a variable đồ sộ represent the unknown coefficients.

    a Fe + b Fe2(SO4)3 = c FeSO4

  2. Create a System of Equations

    Create an equation for each element (Fe, S, O) where each term represents the number of atoms of the element in each reactant or product.

    Fe: 1a + 2b = 1c S: 0a + 3b = 1c O: 0a + 12b = 4c

  3. Solve For All Variables

    Use substitution, Gaussian elimination, or a calculator đồ sộ solve for each variable.

    • 1a + 2b - 1c = 0
    • 3b - 1c = 0
    • 12b - 4c = 0

    Use your graphing calculator's rref() function (or an online rref calculator) đồ sộ convert the following matrix into reduced row-echelon-form:

    [ 1 2 -1 0] [ 0 3 -1 0] [ 0 12 -4 0]

    The resulting matrix can be used đồ sộ determine the coefficients. In the case of a single solution, the last column of the matrix will contain the coefficients.

    Simplify the result đồ sộ get the lowest, whole integer values.

    • a = 1 (Fe)
    • b = 1 (Fe2(SO4)3)
    • c = 3 (FeSO4)
  4. Substitute Coefficients and Verify Result

    Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.

    Fe + Fe2(SO4)3 = 3 FeSO4

    Reactants Products

    Since there is an equal number of each element in the reactants and products of Fe + Fe2(SO4)3 = 3FeSO4, the equation is balanced.

Balance Fe + Fe2(SO4)3 = FeSO4 Using Inspection

The law of conservation of mass states that matter cannot be created or destroyed, which means there must be the same number atoms at the over of a chemical reaction as at the beginning. To be balanced, every element in Fe + Fe2(SO4)3 = FeSO4 must have the same number of atoms on each side of the equation. When using the inspection method (also known as the trial-and-error method), this principle is used đồ sộ balance one element at a time until both sides are equal and the chemical equation is balanced.

1. Count the number of each element on the left and right hand sides

Reactants (Left Hand Side)Products (Right Hand Side)

2. Multiply coefficients for compounds đồ sộ balance out each element

For each element that is not equal, try đồ sộ balance it by adding more of it đồ sộ the side with less. Sometimes there may be multiple compounds with that element on one side, sánh you'll need đồ sộ use your best judgement and be prepared đồ sộ go back and try the other options.

  1. Fe is not balanced. Add 2 molecules of FeSO4 đồ sộ the product (right-hand) side đồ sộ balance Iron:
    Fe + Fe2(SO4)3 = 3FeSO4


3. Verify that the equation is balanced

Since there are an equal number of atoms of each element on both sides, the equation is balanced.

Fe + Fe2(SO4)3 = 3FeSO4

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