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H2 + 2CuSCN → 2Cu + 2HSCN

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Reaction of hydrogen and copper(I) thiocyanate
H2Hydrogen + 2CuSCNCopper(I) thiocyanate
⟶
2CuCopper + 2HSCNThiocyanic acid

The reaction of hydrogen and copper(I) thiocyanate yields copper and thiocyanic acid (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 hydrogen and copper(I) thiocyanate
H2Hydrogen + 2CuSCNCopper(I) thiocyanate
⟶
2CuCopper + 2HSCNThiocyanic acid

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of hydrogen and copper(I) thiocyanate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen1
Reducing
Reducing
CuSCNCopper(I) thiocyanate2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
CuCopper2
Reduced
–
HSCNThiocyanic acid2
Oxidized
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of hydrogen and copper(I) thiocyanate
◆
ΔrG−107.9 kJ/mol
K8.00 × 1018
pK−18.90
H2Un-ionized aqueous solution + 2CuSCNIonized aqueous solution
⟶
2CuCrystalline solid + 2HSCNUn-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
–−107.9––
per 1 mol of
–−107.9––
–−53.95––
per 1 mol of
–−53.95––
per 1 mol of
–−53.95––

Changes in aqueous solution (2)

Reaction of hydrogen and copper(I) thiocyanate
◆
ΔrG−117.6 kJ/mol
K4.01 × 1020
pK−20.60
H2Un-ionized aqueous solution + 2CuSCNIonized aqueous solution
⟶
2CuCrystalline solid + 2HSCNIonized 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
−139.1−117.6−592–
per 1 mol of
−139.1−117.6−592–
−69.55−58.80−296–
per 1 mol of
−69.55−58.80−296–
per 1 mol of
−69.55−58.80−296–

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
CuSCN (cr)–69.9[1]––
CuSCN (ai)148.11[1]142.69[1]184.9[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (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
Cu (cr)0[1]0[1]33.150[1]24.435[1]
Cu (g)338.32[1]298.58[1]166.38[1]20.786[1]
HSCN (ai)76.44[1]92.71[1]144.3[1]-40.2[1]
HSCN (ao)–97.56[1]––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)