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  3. 2HSCN + 12H2O 💧⚡→ (NH4)2SO4 + H2SO4 + 2CO2↑ + 8H2↑

2HSCN + 12H2O 💧⚡→ (NH4)2SO4 + H2SO4 + 2CO2↑ + 8H2↑

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Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
2HSCNThiocyanic acid + 12H2OWater
💧⚡
⟶
(NH4)2SO4Ammonium sulfate + H2SO4Sulfuric acid + 2CO2↑Carbon dioxide + 8H2↑Hydrogen

Electrolysis of aqueous thiocyanic acid yields ammonium sulfate, sulfuric acid, carbon dioxide, 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 thiocyanic acid with water as oxidizing agent
2HSCNThiocyanic acid + 12H2OWater
💧⚡
⟶
(NH4)2SO4Ammonium sulfate + H2SO4Sulfuric acid + 2CO2↑Carbon dioxide + 8H2↑Hydrogen

General equation

Electrolysis of aqueous solution with water as oxidizing agent
Miscible with water/Very soluble in water/Soluble in waterReducing agent + H2OOxidizing agent
💧⚡
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
HSCNThiocyanic acid2
Reducing
Miscible with water
H2OWater12
Oxidizing
Water

Products

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SO4Ammonium sulfate1
Oxidized
–
H2SO4Sulfuric acid1
Oxidized
–
CO2Carbon dioxide2
–
–
H2Hydrogen8
Reduced
–

Thermodynamic changes

Changes in aqueous solution (1)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG223.74 kJ/mol
K0.63 × 10−39
pK39.20
2HSCNIonized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Gas + 8H2↑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
406.51223.74612.4−944
per 1 mol of
203.25111.87306.2−472
per 1 mol of
33.87618.64551.03−78.7
per 1 mol of
406.51223.74612.4−944
per 1 mol of
406.51223.74612.4−944
per 1 mol of
203.25111.87306.2−472
per 1 mol of
50.81427.96876.55−118

Changes in aqueous solution (2)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG364.5 kJ/mol
K0.14 × 10−63
pK63.86
2HSCNIonized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Gas + 8H2↑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
372.9364.54183–
per 1 mol of
186.4182.32092–
per 1 mol of
31.0730.38348.6–
per 1 mol of
372.9364.54183–
per 1 mol of
372.9364.54183–
per 1 mol of
186.4182.32092–
per 1 mol of
46.6145.56522.9–

Changes in aqueous solution (3)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG240.50 kJ/mol
K0.73 × 10−42
pK42.13
2HSCNIonized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Un-ionized aqueous solution + 8H2↑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
365.93240.50420.2–
per 1 mol of
182.97120.25210.1–
per 1 mol of
30.49420.04235.02–
per 1 mol of
365.93240.50420.2–
per 1 mol of
365.93240.50420.2–
per 1 mol of
182.97120.25210.1–
per 1 mol of
45.74130.06352.52–

Changes in aqueous solution (4)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG381.3 kJ/mol
K0.16 × 10−66
pK66.80
2HSCNIonized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Un-ionized aqueous solution + 8H2↑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
332.3381.33991–
per 1 mol of
166.2190.71996–
per 1 mol of
27.6931.78332.6–
per 1 mol of
332.3381.33991–
per 1 mol of
332.3381.33991–
per 1 mol of
166.2190.71996–
per 1 mol of
41.5447.66498.9–

Changes in aqueous solution (5)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG214.04 kJ/mol
K0.32 × 10−37
pK37.50
2HSCNUn-ionized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Gas + 8H2↑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
–214.04––
per 1 mol of
–107.02––
per 1 mol of
–17.837––
per 1 mol of
–214.04––
per 1 mol of
–214.04––
per 1 mol of
–107.02––
per 1 mol of
–26.755––

Changes in aqueous solution (6)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG354.8 kJ/mol
K0.69 × 10−62
pK62.16
2HSCNUn-ionized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Gas + 8H2↑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
–354.8––
per 1 mol of
–177.4––
per 1 mol of
–29.57––
per 1 mol of
–354.8––
per 1 mol of
–354.8––
per 1 mol of
–177.4––
per 1 mol of
–44.35––

Changes in aqueous solution (7)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG230.80 kJ/mol
K0.37 × 10−40
pK40.43
2HSCNUn-ionized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Un-ionized aqueous solution + 8H2↑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
–230.80––
per 1 mol of
–115.40––
per 1 mol of
–19.233––
per 1 mol of
–230.80––
per 1 mol of
–230.80––
per 1 mol of
–115.40––
per 1 mol of
–28.850––

Changes in aqueous solution (8)

Electrolysis of aqueous thiocyanic acid with water as oxidizing agent
◆
ΔrG371.6 kJ/mol
K0.79 × 10−65
pK65.10
2HSCNUn-ionized aqueous solution + 12H2OLiquid
💧⚡
⟶
(NH4)2SO4Ionized aqueous solution + H2SO4Ionized aqueous solution + 2CO2↑Un-ionized aqueous solution + 8H2↑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
–371.6––
per 1 mol of
–185.8––
per 1 mol of
–30.97––
per 1 mol of
–371.6––
per 1 mol of
–371.6––
per 1 mol of
–185.8––
per 1 mol of
–46.45––

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
HSCN (ai)76.44[1]92.71[1]144.3[1]-40.2[1]
HSCN (ao)–97.56[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]
* (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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)2SO4 (cr)-1180.85[1]-901.67[1]220.1[1]187.49[1]
(NH4)2SO4 (ai)-1174.28[1]-903.14[1]246.9[1]-133.1[1]
H2SO4 (cr)––––
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[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]–
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, (l):Liquid, (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)