You-iggy
  1. Home
  2. Chemical reactions
  3. 4KSCN + 7O2 → 2K2CO3 + 4S + 4NO + 2CO2

4KSCN + 7O2 → 2K2CO3 + 4S + 4NO + 2CO2

Last updated:
Reaction of potassium thiocyanate and oxygen
4KSCNPotassium thiocyanate + 7O2Oxygen
⟶
2K2CO3Potassium carbonate + 4SSulfur + 4NONitrogen monoxide + 2CO2Carbon dioxide

The reaction of potassium thiocyanate and oxygen yields potassium carbonate, sulfur, nitrogen monoxide, and carbon dioxide (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

Reaction of potassium thiocyanate and oxygen
4KSCNPotassium thiocyanate + 7O2Oxygen
⟶
2K2CO3Potassium carbonate + 4SSulfur + 4NONitrogen monoxide + 2CO2Carbon dioxide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of potassium thiocyanate and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KSCNPotassium thiocyanate4
Reducing
Reducing
O2Oxygen7
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2CO3Potassium carbonate2
Reduced
–
SSulfur4
Oxidized
–
NONitrogen monoxide4
Redoxed product
–
CO2Carbon dioxide2
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium thiocyanate and oxygen
◆
ΔrG−1856.3 kJ/mol
K1.62 × 10325
pK−325.21
4KSCNCrystalline solid + 7O2Gas
⟶
2K2CO3Crystalline solid + 4SCrystalline solidrhombic + 4NOGas + 2CO2Gas
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
−1927.42−1856.3−224.24−46.59
−481.855−464.07−56.060−11.65
per 1 mol of
−275.346−265.19−32.034−6.656
−963.710−928.15−112.12−23.30
per 1 mol of
−481.855−464.07−56.060−11.65
per 1 mol of
−481.855−464.07−56.060−11.65
per 1 mol of
−963.710−928.15−112.12−23.30

Changes in standard condition (2)

Reaction of potassium thiocyanate and oxygen
4KSCNCrystalline solid + 7O2Gas
⟶
2K2CO3Crystalline solid + 4SCrystalline solidmonoclinic + 4NOGas + 2CO2Gas
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
−1926.10–––
−481.525–––
per 1 mol of
−275.157–––
−963.050–––
per 1 mol of
−481.525–––
per 1 mol of
−481.525–––
per 1 mol of
−963.050–––

Changes in aqueous solution (1)

Reaction of potassium thiocyanate and oxygen
◆
ΔrG−1983.8 kJ/mol
K3.52 × 10347
pK−347.55
4KSCNIonized aqueous solution + 7O2Un-ionized aqueous solution
⟶
2K2CO3Ionized aqueous solution + 4SCrystalline solidrhombic + 4NOGas + 2CO2Gas
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
−2004.2−1983.8−70.0–
−501.05−495.95−17.5–
per 1 mol of
−286.31−283.40−10.0–
−1002.1−991.90−35.0–
per 1 mol of
−501.05−495.95−17.5–
per 1 mol of
−501.05−495.95−17.5–
per 1 mol of
−1002.1−991.90−35.0–

Changes in aqueous solution (2)

Reaction of potassium thiocyanate and oxygen
◆
ΔrG−1967.0 kJ/mol
K4.01 × 10344
pK−344.60
4KSCNIonized aqueous solution + 7O2Un-ionized aqueous solution
⟶
2K2CO3Ionized aqueous solution + 4SCrystalline solidrhombic + 4NOGas + 2CO2Un-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
−2044.7−1967.0−262.3–
−511.18−491.75−65.58–
per 1 mol of
−292.10−281.00−37.47–
−1022.4−983.50−131.2–
per 1 mol of
−511.18−491.75−65.58–
per 1 mol of
−511.18−491.75−65.58–
per 1 mol of
−1022.4−983.50−131.2–

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
KSCN (cr)-200.16[1]-178.31[1]124.26[1]88.53[1]
KSCN (ai)-175.94[1]-190.56[1]246.9[1]-18.4[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, (ai):Ionized aqueous solution, (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
K2CO3 (cr)-1151.02[1]-1063.5[1]155.52[1]114.43[1]
K2CO3 (ai)-1181.90[1]-1094.36[1]148.1[1]–
K2CO3 (cr)
1.5 hydrate
-1609.2[1]-1432.5[1]203.3[1]–
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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)