Fe + Fe_{2}(SO_{4})_{3} → 3FeSO_{4}

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### Word Equation

Iron + Ferric Sulfate = Iron(Ii) Sulfate

One mole of solid

and one mole of aqueous

combine đồ sộ size three moles of aqueous

### Reaction Type

Synthesis

- 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.

### Reactants

### Iron - Fe

### Ferric Sulfate - Fe

_{2}(SO_{4})_{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

### Products

### Iron(Ii) Sulfate - FeSO

_{4}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

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

#### Is the Reaction Exothermic or Endothermic?

Fe (s alpha) | 1 mol | 0 kJ/mol | -0 kJ |
---|---|---|---|

Fe_{2}(SO_{4})_{3} (s) | 1 mol | -2581.528 kJ/mol | 2581.528 kJ |

FeSO_{4} (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 = S_{products} - S_{reactants}. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.

Fe (s alpha) | 1 mol | 27.27968 J/(mol K) | -27.27968 J/K |
---|---|---|---|

Fe_{2}(SO_{4})_{3} (s) | 1 mol | 307.524 J/(mol K) | -307.524 J/K |

FeSO_{4} (s) | 3 mol | 120.9176 J/(mol K) | 362.7528 J/K |

ΣΔS°(reactants) | 334.80368 J/K | ||

ΣΔS°(products) | 362.7528 J/K | ||

ΔS°_{rxn} | 27.94912 J/K |

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

#### Is the Reaction Exergonic or Endergonic?

ΔG = G_{products} - G_{reactants}. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.

Fe (s alpha) | 1 mol | 0 kJ/mol | -0 kJ |
---|---|---|---|

Fe_{2}(SO_{4})_{3} (s) | 1 mol | -2263.1256 kJ/mol | 2263.1256 kJ |

FeSO_{4} (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

K_{c} or Q = ( [FeSO_{4}]^{3} ) / ( [Fe] [Fe_{2}(SO_{4})_{3}] )

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

rate = -(Δ[Fe] / Δt) = -(Δ[Fe_{2}(SO_{4})_{3}] / Δt) = 1/3 * (Δ[FeSO_{4}] / Δt)

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

## Instructions

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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 đồ sộ 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 Balance Equations

Read our article on how đồ sộ balance chemical equations or ask for help in our chat.

You can also ask for help in our chat or forums.

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

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.

### 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 Fe

_{2}(SO_{4})_{3}= c FeSO_{4}### 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### 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)

### 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 + Fe

_{2}(SO_{4})_{3}= 3 FeSO_{4}Reactants Products Fe 3 3 ✔️ S 3 3 ✔️ O 12 12 ✔️ 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) | |||||
---|---|---|---|---|---|---|

Reactants | Products | |||||

Fe | Fe_{2}(SO_{4})_{3} | Total | FeSO_{4} | Total | ||

Fe | 1 | 2 | 3 | 1 | 1 | ❌ |

S | 3 | 3 | 1 | 1 | ❌ | |

O | 12 | 12 | 4 | 4 | ❌ |

### 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.

**Fe**is not balanced. Add**2**molecules of**FeSO**đồ sộ the product (right-hand) side đồ sộ balance Iron:_{4}

Fe + Fe_{2}(SO_{4})_{3}= 3FeSO_{4}Reactants Products Fe 3 3 ✔️ S 3 3 ✔️ O 12 12 ✔️

### 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 + Fe_{2}(SO_{4})_{3} = 3FeSO_{4}

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