fes ra fe2o3

4FeS + 7O24SO2 + 2Fe2O3

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Word Equation

Iron(Ii) Sulfide + Dioxygen = Sulfur Dioxide + Hematite

FeS + O2 = SO2 + Fe2O3 is a Double Displacement (Metathesis) reaction where four moles of Iron(Ii) Sulfide [FeS] and seven moles of Dioxygen [O2] react to tát form four moles of Sulfur Dioxide [SO2] and two moles of Hematite [Fe2O3]

Reactants

  • Iron(Ii) Sulfide - FeS

    Iron(Ii) Sulphide Ferrous Sulfide Ferrous Sulphide

  • Dioxygen - O2

    Lox Liquid Oxygen Oxygen Gas Triplet Oxygen Diatomic Oxygen Molecular Oxygen Oxygen O₂

Products

  • Sulfur Dioxide - SO2

    Sulphur Dioxide R-764 Sulfurous Anhydride So2 Sulphur Dioxide , Sulfur Dioxide Sulfur Oxide Sulfurous Oxide Sulfurous Acid Anhydride

  • Hematite - Fe2O3

    Iron(3+);Oxygen(2-) Haematitis Of Pliny Raphisiderite Oligiste Blood Stone

Thermodynamics

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

No state of matter options are available for this reaction.

Is the Reaction Exothermic or Endothermic?

FeS (s pyrrhotite)4 mol-99.9976 kJ/mol399.9904 kJ
O2 (g)7 mol0 kJ/mol-0 kJ
SO2 (g)4 mol-296.829696 kJ/mol-1187.318784 kJ
Fe2O3 (s hematite)2 mol-824.248 kJ/mol-1648.496 kJ
ΣΔH°f(reactants)-399.9904 kJ
ΣΔH°f(products)-2835.814784 kJ
ΔH°rxn-2435.824384 kJ

ΣΔH°f(reactants) > ΣΔH°f(products), so sánh FeS + O2 = SO2 + Fe2O3 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.

FeS (s pyrrhotite)4 mol60.29144 J/(mol K)-241.16576 J/K
O2 (g)7 mol205.028552 J/(mol K)-1435.199864 J/K
SO2 (g)4 mol248.1112 J/(mol K)992.4448 J/K
Fe2O3 (s hematite)2 mol87.40376 J/(mol K)174.80752 J/K
ΣΔS°(reactants)1676.365624 J/K
ΣΔS°(products)1167.25232 J/K
ΔS°rxn-509.113304 J/K

ΣΔS°(reactants) > ΣΔS°(products), so sánh FeS + O2 = SO2 + Fe2O3 is exoentropic (decrease in entropy).

Is the Reaction Exergonic or Endergonic?

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

FeS (s pyrrhotite)4 mol-100.416 kJ/mol401.664 kJ
O2 (g)7 mol0 kJ/mol-0 kJ
SO2 (g)4 mol-300.193632 kJ/mol-1200.774528 kJ
Fe2O3 (s hematite)2 mol-742.2416 kJ/mol-1484.4832 kJ
ΣΔG°(reactants)-401.664 kJ
ΣΔG°(products)-2685.257728 kJ
ΔG°rxn-2283.593728 kJ

ΣΔG°(reactants) > ΣΔG°(products), so sánh FeS + O2 = SO2 + Fe2O3 is exergonic (releases energy).

Reaction Expressions

Kc or Q = ( [SO2]4 [Fe2O3]2 ) / ( [FeS]4 [O2]7 )

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

rate = -1/4 * (Δ[FeS] / Δt) = -1/7 * (Δ[O2] / Δt) = 1/4 * (Δ[SO2] / Δt) = một nửa * (Δ[Fe2O3] / Δt)

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

Instructions

To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. The balanced equation will appear above.

  • Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F.
  • Ionic charges are not yet supported and will be ignored.
  • Replace immutable groups in compounds to tát avoid ambiguity. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will.
  • Compound states [like (s) (aq) or (g)] are not required.
  • You can use parenthesis () or brackets [].

How to tát Balance Chemical Equations

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Balance FeS + O2 = SO2 + Fe2O3 Using the Algebraic Method

How To Balance FeS + O2 = SO2 + Fe2O3

To balance the equation FeS + O2 = SO2 + Fe2O3 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.

Step 1: Label Each Compound With a Variable

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

a FeS + b O2 = c SO2 + d Fe2O3

Step 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	+	0b	=	0c	+	2d
S:	1a	+	0b	=	1c	+	0d
O:	0a	+	2b	=	2c	+	3d

Step 3: Solve For All Variables

Use substitution, Gaussian elimination, or a calculator to tát solve for each variable.

  • 1a - 2d = 0
  • 1a - 1c = 0
  • 2b - 2c - 3d = 0

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

[ 1	 0	 0	-2	0]
[ 1	 0	-1	 0	0]
[ 0	 2	-2	-3	0]

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

Simplify the result to tát get the lowest, whole integer values.

  • a = 4 (FeS)
  • b = 7 (O2)
  • c = 4 (SO2)
  • d = 2 (Fe2O3)

Step 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.

4 FeS + 7 O2 = 4 SO2 + 2 Fe2O3

Reactants Products
Fe44✔️
S44✔️
O1414✔️

Since there is an equal number of each element in the reactants and products of 4FeS + 7O2 = 4SO2 + 2Fe2O3, the equation is balanced.

Balance FeS + O2 = SO2 + Fe2O3 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 FeS + O2 = SO2 + Fe2O3 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 to tát balance one element at a time until both sides are equal and the chemical equation is balanced.

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

Reactants (Left Hand Side)Products (Right Hand Side)
ReactantsProducts
FeSO2TotalSO2Fe2O3Total
Fe1122
S1111✔️
O22235

Step 2: Multiply coefficients for compounds to tát balance out each element

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

  1. Fe is not balanced. Add 1 molecule of FeS to tát the reactant (left-hand) side to tát balance Iron:
    2FeS + O2 = SO2 + Fe2O3

    ReactantsProducts
    Fe22✔️
    S21
    O25
  2. S is not balanced. Add 1 molecule of SO2 to tát the product (right-hand) side to tát balance Sulfur:
    2FeS + O2 = 2SO2 + Fe2O3

    ReactantsProducts
    Fe22✔️
    S22✔️
    O27
  3. O is not balanced. Add 6 molecules of O2 to tát the reactant (left-hand) side to tát try to tát balance Oxygen:
    2FeS + 7O2 = 2SO2 + Fe2O3

    ReactantsProducts
    Fe22✔️
    S22✔️
    O147
  4. O is not balanced. Add 2 molecules of SO2 to tát the product (right-hand) side to tát balance Oxygen:
    2FeS + 7O2 = 4SO2 + Fe2O3

    ReactantsProducts
    Fe22✔️
    S24
    O1411
  5. S is not balanced. Add 2 molecules of FeS to tát the reactant (left-hand) side to tát balance Sulfur:
    4FeS + 7O2 = 4SO2 + Fe2O3

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    ReactantsProducts
    Fe42
    S44✔️
    O1411
  6. Fe is not balanced. Add 1 molecule of Fe2O3 to tát the product (right-hand) side to tát balance Iron:
    4FeS + 7O2 = 4SO2 + 2Fe2O3

    ReactantsProducts
    Fe44✔️
    S44✔️
    O1414✔️

Step 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.

4FeS + 7O2 = 4SO2 + 2Fe2O3

Practice Balancing