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  3. 12CH3COOK 🔥→ 6K2O + 15CO↑ + 9CH4↑ + O3↑

12CH3COOK 🔥→ 6K2O + 15CO↑ + 9CH4↑ + O3↑

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Decomposition of potassium acetate
12CH3COOKPotassium acetate
🔥
⟶
6K2OPotassium oxide + 15CO↑Carbon monoxide + 9CH4↑Methane + O3↑Ozone

Decomposition of potassium acetate yields potassium oxide, carbon monoxide, methane, and ozone (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

Decomposition of potassium acetate
12CH3COOKPotassium acetate
🔥
⟶
6K2OPotassium oxide + 15CO↑Carbon monoxide + 9CH4↑Methane + O3↑Ozone

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 acetate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CH3COOKPotassium acetate12
Self redox agent
Thermally decomposable
Oxoacid salt

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide6
–
–
COCarbon monoxide15
Redoxed product
–
CH4Methane9
Reduced
–
O3Ozone1
Oxidized
–

Thermodynamic changes

Changes in standard condition

Decomposition of potassium acetate
12CH3COOKCrystalline solid
🔥
⟶
6K2OCrystalline solid + 15CO↑Gas + 9CH4↑Gas + O3↑Gas
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
4318.5–––
per 1 mol of
359.88–––
per 1 mol of
719.75–––
per 1 mol of
287.90–––
per 1 mol of
479.83–––
per 1 mol of
4318.5–––

Changes in aqueous solution (1)

Decomposition of potassium acetate
◆
ΔrG3547.6 kJ/mol
K0.31 × 10−621
pK621.51
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Gas + 9CH4↑Gas + O3↑Gas
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
4503.23547.63175.81110.3
per 1 mol of
375.27295.63264.6592.525
per 1 mol of
750.53591.27529.30185.05
per 1 mol of
300.21236.51211.7274.020
per 1 mol of
500.36394.18352.87123.37
per 1 mol of
4503.23547.63175.81110.3

Changes in aqueous solution (2)

Decomposition of potassium acetate
◆
ΔrG3558.5 kJ/mol
K0.38 × 10−623
pK623.42
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Gas + 9CH4↑Gas + O3↑Un-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
4486.43558.53083–
per 1 mol of
373.87296.54256.9–
per 1 mol of
747.73593.08513.8–
per 1 mol of
299.09237.23205.5–
per 1 mol of
498.49395.39342.6–
per 1 mol of
4486.43558.53083–

Changes in aqueous solution (3)

Decomposition of potassium acetate
◆
ΔrG3695.1 kJ/mol
K0.44 × 10−647
pK647.35
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Gas + 9CH4↑Un-ionized aqueous solution + O3↑Gas
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
4375.13695.12252.7–
per 1 mol of
364.59307.93187.72–
per 1 mol of
729.18615.85375.45–
per 1 mol of
291.67246.34150.18–
per 1 mol of
486.12410.57250.30–
per 1 mol of
4375.13695.12252.7–

Changes in aqueous solution (4)

Decomposition of potassium acetate
◆
ΔrG3706.0 kJ/mol
K0.55 × 10−649
pK649.26
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Gas + 9CH4↑Un-ionized aqueous solution + O3↑Un-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
4358.33706.02160–
per 1 mol of
363.19308.83180.0–
per 1 mol of
726.38617.67360.0–
per 1 mol of
290.55247.07144.0–
per 1 mol of
484.26411.78240.0–
per 1 mol of
4358.33706.02160–

Changes in aqueous solution (5)

Decomposition of potassium acetate
◆
ΔrG3806.6 kJ/mol
K0.13 × 10−666
pK666.89
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Un-ionized aqueous solution + 9CH4↑Gas + O3↑Gas
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
4346.73806.61779.7–
per 1 mol of
362.22317.22148.31–
per 1 mol of
724.45634.43296.62–
per 1 mol of
289.78253.77118.65–
per 1 mol of
482.97422.96197.74–
per 1 mol of
4346.73806.61779.7–

Changes in aqueous solution (6)

Decomposition of potassium acetate
◆
ΔrG3817.5 kJ/mol
K0.16 × 10−668
pK668.80
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Un-ionized aqueous solution + 9CH4↑Gas + O3↑Un-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
4329.93817.51687–
per 1 mol of
360.82318.13140.6–
per 1 mol of
721.65636.25281.2–
per 1 mol of
288.66254.50112.5–
per 1 mol of
481.10424.17187.4–
per 1 mol of
4329.93817.51687–

Changes in aqueous solution (7)

Decomposition of potassium acetate
◆
ΔrG3954.1 kJ/mol
K0.19 × 10−692
pK692.73
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Un-ionized aqueous solution + 9CH4↑Un-ionized aqueous solution + O3↑Gas
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
4218.63954.1856.6–
per 1 mol of
351.55329.5171.38–
per 1 mol of
703.10659.02142.8–
per 1 mol of
281.24263.6157.11–
per 1 mol of
468.73439.3495.18–
per 1 mol of
4218.63954.1856.6–

Changes in aqueous solution (8)

Decomposition of potassium acetate
◆
ΔrG3965.0 kJ/mol
K0.23 × 10−694
pK694.64
12CH3COOKIonized aqueous solution
🔥
⟶
6K2OCrystalline solid + 15CO↑Un-ionized aqueous solution + 9CH4↑Un-ionized aqueous solution + O3↑Un-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
4201.83965.0764–
per 1 mol of
350.15330.4263.7–
per 1 mol of
700.30660.83127–
per 1 mol of
280.12264.3350.9–
per 1 mol of
466.87440.5684.9–
per 1 mol of
4201.83965.0764–

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
CH3COOK (cr)-723.0[1]–––
CH3COOK (ai)-738.39[1]-652.58[1]189.1[1]15.5[1]
* (cr):Crystalline solid, (ai):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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[1]–––
CO (g)-110.525[1]-137.168[1]197.674[1]29.142[1]
CO (ao)-120.96[1]-119.90[1]104.6[1]–
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]–
O3 (g)142.7[1]163.2[1]238.93[1]39.20[1]
O3 (ao)125.9[1]174.1[1]146[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education