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Mg + Cl2 → MgCl2

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Reaction of magnesium and chlorine
MgMagnesium + Cl2Chlorine
⟶
MgCl2Magnesium chloride

The reaction of magnesium and chlorine yields magnesium chloride. This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

Reaction of magnesium and chlorine
MgMagnesium + Cl2Chlorine
⟶
MgCl2Magnesium chloride

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product
Reaction of metal and nonmetal
MetalReducing agent + NonmetalOxidizing agent
⟶
Binary compoundOxidation reduction product

Oxidation state of each atom

Reaction of magnesium and chlorine

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
MgMagnesium1
Reducing
Reducing
Metal
Cl2Chlorine1
Oxidizing
Oxidizing
Nonmetal

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgCl2Magnesium chloride1
Redoxed product
–
Binary compound

Thermodynamic changes

Changes in standard condition

Reaction of magnesium and chlorine
◆
ΔrG−591.79 kJ/mol
K4.75 × 10103
pK−103.68
MgCrystalline solid + Cl2Gas
⟶
MgCl2Crystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−641.32−591.79−166.1312.58
per 1 mol of
−641.32−591.79−166.1312.58
per 1 mol of
−641.32−591.79−166.1312.58
per 1 mol of
−641.32−591.79−166.1312.58

Changes in aqueous solution

Reaction of magnesium and chlorine
◆
ΔrG−724.0 kJ/mol
K6.91 × 10126
pK−126.84
MgCrystalline solid + Cl2Un-ionized aqueous solution
⟶
MgCl2Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1		Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1		Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1		Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−777.8−724.0−179–
per 1 mol of
−777.8−724.0−179–
per 1 mol of
−777.8−724.0−179–
per 1 mol of
−777.8−724.0−179–

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Mg (cr)0[1]0[1]32.68[1]24.89[1]
Mg (g)147.70[1]113.10[1]148.650[1]20.786[1]
Cl2 (g)0[1]0[1]223.066[1]33.907[1]
Cl2 (ao)-23.4[1]6.94[1]121[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1		Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1		Standard
molar entropy
S°
J · K−1 · mol−1		Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
MgCl2 (cr)-641.32[1]-591.79[1]89.62[1]71.38[1]
MgCl2 (g)-400.4[1]–––
MgCl2 (ai)-801.15[1]-717.1[1]-25.1[1]–
MgCl2 (cr)
1 hydrate
-966.63[1]-861.74[1]137.2[1]115.27[1]
MgCl2 (cr)
2 hydrate
-1279.72[1]-1118.00[1]179.9[1]159.20[1]
MgCl2 (cr)
4 hydrate
-1898.99[1]-1623.29[1]264.0[1]241.42[1]
MgCl2 (cr)
6 hydrate
-2499.02[1]-2114.64[1]366.1[1]315.06[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)