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K2SiO3 🔥→ K2O + Si + O2

Decomposition of potassium metasilicate yields potassium oxide, silicon, and oxygen (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Thermal decomposition with redox
Thermally decomposable substanceSelf redox agent
🔥
ProductOxidation product + ProductReduction product
Thermal decomposition of oxoacid salt with redox
Oxoacid saltSelf redox agent
🔥
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Decomposition of potassium metasilicate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K2SiO3Potassium metasilicate1
Self redox agent
Thermally decomposable
Oxoacid salt

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide1
SiSilicon1
Reduced
O2Oxygen1
Oxidized

Thermodynamic changes

Changes in standard condition (1)

Decomposition of potassium metasilicate
K2SiO3Crystalline solid
🔥
K2OCrystalline solid + SiCrystalline solid + O2Gas
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
172.114.7
172.114.7
per 1 mol of
172.114.7
per 1 mol of
172.114.7
per 1 mol of
172.114.7

Changes in standard condition (2)

Decomposition of potassium metasilicate
K2SiO3Crystalline solid
🔥
K2OCrystalline solid + SiAmorphous solid + O2Gas
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
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (1)

Decomposition of potassium metasilicate
K2SiO3Crystalline solid
🔥
K2OCrystalline solid + SiCrystalline solid + O2Gas
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
172.114.7
172.114.7
per 1 mol of
172.114.7
per 1 mol of
172.114.7
per 1 mol of
172.114.7

Changes in aqueous solution (2)

Decomposition of potassium metasilicate
K2SiO3Crystalline solid
🔥
K2OCrystalline solid + SiCrystalline solid + O2Un-ionized 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
77.8
77.8
per 1 mol of
77.8
per 1 mol of
77.8
per 1 mol of
77.8

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
K2SiO3 (cr)146.0[1]118.4[1]
* (cr):Crystalline solid

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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]
Si (cr)0[1]0[1]18.83[1]20.00[1]
Si (am)4.2[1]
Si (g)455.6[1]411.3[1]167.97[1]22.251[1]
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
  2. 2
    James G. Speight (2017)
    Lange's Handbook of Chemistry, 17th edition
    McGraw Hill Education