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NH4SCN + 3H2O 💧⚡→ (NH4)2SO3 + C + H2↑

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Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
NH4SCNAmmonium thiocyanate + 3H2OWater
💧⚡
⟶
(NH4)2SO3Ammonium sulfite + CCarbon + H2↑Hydrogen

Electrolysis of aqueous ammonium thiocyanate yields ammonium sulfite, carbon, and hydrogen (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

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
NH4SCNAmmonium thiocyanate + 3H2OWater
💧⚡
⟶
(NH4)2SO3Ammonium sulfite + CCarbon + H2↑Hydrogen

General equation

Electrolysis of aqueous solution with water as non redox agent
Miscible with water/Very soluble in water/Soluble in waterSelf redox agent + H2ONon-redox agent
💧⚡
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4SCNAmmonium thiocyanate1
Self redox agent
Very soluble in water
H2OWater3
–
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO3Ammonium sulfite1
Oxidized
–
CCarbon1
Reduced
–
H2Hydrogen1
–
–

Thermodynamic changes

Changes in standard condition (1)

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
NH4SCNCrystalline solid + 3H2OLiquid
💧⚡
⟶
(NH4)2SO3Crystalline solid + CCrystalline solidgraphite + H2↑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
50.9–––
50.9–––
per 1 mol of
17.0–––
per 1 mol of
50.9–––
per 1 mol of
50.9–––
per 1 mol of
50.9–––

Changes in standard condition (2)

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
NH4SCNCrystalline solid + 3H2OLiquid
💧⚡
⟶
(NH4)2SO3Crystalline solid + CCrystalline soliddiamond + H2↑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
52.8–––
52.8–––
per 1 mol of
17.6–––
per 1 mol of
52.8–––
per 1 mol of
52.8–––
per 1 mol of
52.8–––

Changes in aqueous solution (1)

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
◆
ΔrG53.0 kJ/mol
K0.52 × 10−9
pK9.29
NH4SCNIonized aqueous solution + 3H2OLiquid
💧⚡
⟶
(NH4)2SO3Ionized aqueous solution + CCrystalline solidgraphite + H2↑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
13.253.0−133.5–
13.253.0−133.5–
per 1 mol of
4.4017.7−44.50–
per 1 mol of
13.253.0−133.5–
per 1 mol of
13.253.0−133.5–
per 1 mol of
13.253.0−133.5–

Changes in aqueous solution (2)

Electrolysis of aqueous ammonium thiocyanate with water as non-redox agent
◆
ΔrG70.6 kJ/mol
K0.43 × 10−12
pK12.37
NH4SCNIonized aqueous solution + 3H2OLiquid
💧⚡
⟶
(NH4)2SO3Ionized aqueous solution + CCrystalline solidgraphite + H2↑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
9.070.6313–
9.070.6313–
per 1 mol of
3.023.5104–
per 1 mol of
9.070.6313–
per 1 mol of
9.070.6313–
per 1 mol of
9.070.6313–

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
NH4SCN (cr)-78.7[1]–––
NH4SCN (ai)-56.07[1]13.40[1]257.7[1]39.7[1]
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
(NH4)2SO3 (cr)-885.3[1]–––
(NH4)2SO3 (ai)-900.4[1]-645.0[1]197.5[1]–
(NH4)2SO3 (cr)
1 hydrate
-1187.4[1]–––
C (cr)
graphite
0[1]0[1]5.740[1]8.527[1]
C (cr)
diamond
1.895[1]2.900[1]2.377[1]6.113[1]
C (g)716.682[1]671.257[1]158.096[1]20.838[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[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)