4FeS2 + 11O2 → 2Fe2O3 + 8SO2
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Word Equation
Pyrite + Dioxygen = Hematite + Sulfur Dioxide
FeS2 + O2 = Fe2O3 + SO2 is a Double Displacement (Metathesis) reaction where four moles of
Reactants
Pyrite - FeS2
Fool's Gold Iron Pyrite
Dioxygen - O2
Lox Liquid Oxygen Oxygen Gas Triplet Oxygen Diatomic Oxygen Molecular Oxygen Oxygen O₂
Products
Hematite - Fe2O3
Iron(3+);Oxygen(2-) Haematitis Of Pliny Raphisiderite Oligiste Blood Stone
Sulfur Dioxide - SO2
Sulphur Dioxide R-764 Sulfurous Anhydride So2 Sulphur Dioxide , Sulfur Dioxide Sulfur Oxide Sulfurous Oxide Sulfurous Acid Anhydride
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?
| FeS2 (s pyrite) | 4 mol | -178.2384 kJ/mol | 712.9536 kJ |
|---|---|---|---|
| O2 (g) | 11 mol | 0 kJ/mol | -0 kJ |
| Fe2O3 (s hematite) | 2 mol | -824.248 kJ/mol | -1648.496 kJ |
| SO2 (g) | 8 mol | -296.829696 kJ/mol | -2374.637568 kJ |
| ΣΔH°f(reactants) | -712.9536 kJ | ||
| ΣΔH°f(products) | -4023.133568 kJ | ||
| ΔH°rxn | -3310.179968 kJ | ||
ΣΔH°f(reactants) > ΣΔH°f(products), sánh FeS2 + O2 = Fe2O3 + SO2 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.
| FeS2 (s pyrite) | 4 mol | 52.9276 J/(mol K) | -211.7104 J/K |
|---|---|---|---|
| O2 (g) | 11 mol | 205.028552 J/(mol K) | -2255.314072 J/K |
| Fe2O3 (s hematite) | 2 mol | 87.40376 J/(mol K) | 174.80752 J/K |
| SO2 (g) | 8 mol | 248.1112 J/(mol K) | 1984.8896 J/K |
| ΣΔS°(reactants) | 2467.024472 J/K | ||
| ΣΔS°(products) | 2159.69712 J/K | ||
| ΔS°rxn | -307.327352 J/K | ||
ΣΔS°(reactants) > ΣΔS°(products), sánh FeS2 + O2 = Fe2O3 + SO2 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.
| FeS2 (s pyrite) | 4 mol | -166.9416 kJ/mol | 667.7664 kJ |
|---|---|---|---|
| O2 (g) | 11 mol | 0 kJ/mol | -0 kJ |
| Fe2O3 (s hematite) | 2 mol | -742.2416 kJ/mol | -1484.4832 kJ |
| SO2 (g) | 8 mol | -300.193632 kJ/mol | -2401.549056 kJ |
| ΣΔG°(reactants) | -667.7664 kJ | ||
| ΣΔG°(products) | -3886.032256 kJ | ||
| ΔG°rxn | -3218.265856 kJ | ||
ΣΔG°(reactants) > ΣΔG°(products), sánh FeS2 + O2 = Fe2O3 + SO2 is exergonic (releases energy).
Reaction Expressions
Kc or Q = ( [Fe2O3]2 [SO2]8 ) / ( [FeS2]4 [O2]11 )
(assuming all reactants and products are aqueous. substitutue 1 for any solids/liquids, and Psubstance for gases.)
rate = -1/4 * (Δ[FeS2] / Δt) = -1/11 * (Δ[O2] / Δt) = 50% * (Δ[Fe2O3] / Δt) = 1/8 * (Δ[SO2] / 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 lớn 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 [].
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Practice Balancing
Balance FeS2 + O2 = Fe2O3 + SO2 Using the Algebraic Method
To balance the equation FeS2 + O2 = Fe2O3 + SO2 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 lớn represent the unknown coefficients.
a FeS2 + b O2 = c Fe2O3 + d SO2
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 = 2c + 0d S: 2a + 0b = 0c + 1d O: 0a + 2b = 3c + 2d
Step 3: Solve For All Variables
Use substitution, Gaussian elimination, or a calculator to lớn solve for each variable.
- 1a - 2c = 0
- 2a - 1d = 0
- 2b - 3c - 2d = 0
Use your graphing calculator's rref() function (or an online rref calculator) to lớn convert the following matrix into reduced row-echelon-form:
[ 1 0 -2 0 0] [ 2 0 0 -1 0] [ 0 2 -3 -2 0]
The resulting matrix can be used to lớn determine the coefficients. In the case of a single solution, the last column of the matrix will contain the coefficients.
Simplify the result to lớn get the lowest, whole integer values.
- a = 4 (FeS2)
- b = 11 (O2)
- c = 2 (Fe2O3)
- d = 8 (SO2)
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 FeS2 + 11 O2 = 2 Fe2O3 + 8 SO2
| Fe | 4 | 4 | ✔️ |
|---|---|---|---|
| S | 8 | 8 | ✔️ |
| O | 22 | 22 | ✔️ |
Since there is an equal number of each element in the reactants and products of 4FeS2 + 11O2 = 2Fe2O3 + 8SO2, the equation is balanced.
Balance FeS2 + O2 = Fe2O3 + SO2 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 kết thúc of a chemical reaction as at the beginning. To be balanced, every element in FeS2 + O2 = Fe2O3 + SO2 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 lớn 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) | ||||||
|---|---|---|---|---|---|---|---|
| Reactants | Products | ||||||
| FeS2 | O2 | Total | Fe2O3 | SO2 | Total | ||
| Fe | 1 | 1 | 2 | 2 | ❌ | ||
| S | 2 | 2 | 1 | 1 | ❌ | ||
| O | 2 | 2 | 3 | 2 | 5 | ❌ | |
Step 2: Multiply coefficients for compounds to lớn balance out each element
For each element that is not equal, try to lớn balance it by adding more of it to lớn the side with less. Sometimes there may be multiple compounds with that element on one side, sánh you'll need to lớn use your best judgement and be prepared to lớn go back and try the other options.
Fe is not balanced. Add 1 molecule of FeS2 to lớn the reactant (left-hand) side to lớn balance Iron:
2FeS2 + O2 = Fe2O3 + SO2Reactants Products Fe 2 2 ✔️ S 4 1 ❌ O 2 5 ❌ S is not balanced. Add 3 molecules of SO2 to lớn the product (right-hand) side to lớn balance Sulfur:
2FeS2 + O2 = Fe2O3 + 4SO2Reactants Products Fe 2 2 ✔️ S 4 4 ✔️ O 2 11 ❌ O is not balanced. Add 10 molecules of O2 to lớn the reactant (left-hand) side to lớn try to lớn balance Oxygen:
2FeS2 + 11O2 = Fe2O3 + 4SO2Reactants Products Fe 2 2 ✔️ S 4 4 ✔️ O 22 11 ❌ O is not balanced. Add 1 molecule of Fe2O3 to lớn the product (right-hand) side to lớn balance Oxygen:
2FeS2 + 11O2 = 2Fe2O3 + 4SO2Reactants Products Fe 2 4 ❌ S 4 4 ✔️ O 22 14 ❌ Fe is not balanced. Add 2 molecules of FeS2 to lớn the reactant (left-hand) side to lớn balance Iron:
4FeS2 + 11O2 = 2Fe2O3 + 4SO2Xem thêm: bài 8 địa lí 7 kết nối tri thức
Reactants Products Fe 4 4 ✔️ S 8 4 ❌ O 22 14 ❌ S is not balanced. Add 4 molecules of SO2 to lớn the product (right-hand) side to lớn balance Sulfur:
4FeS2 + 11O2 = 2Fe2O3 + 8SO2Reactants Products Fe 4 4 ✔️ S 8 8 ✔️ O 22 22 ✔️
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.
4FeS2 + 11O2 = 2Fe2O3 + 8SO2
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