You-iggy
  1. Home
  2. Chemical reactions
  3. 2CuSCN + 5O2 → Cu(NO3)2 + CuS + S + 2CO2

2CuSCN + 5O2 → Cu(NO3)2 + CuS + S + 2CO2

Last updated:
Reaction of copper(I) thiocyanate and oxygen
2CuSCNCopper(I) thiocyanate + 5O2Oxygen
⟶
Cu(NO3)2Copper(II) nitrate + CuSCopper(II) sulfide + SSulfur + 2CO2Carbon dioxide

The reaction of copper(I) thiocyanate and oxygen yields copper(II) nitrate, copper(II) sulfide, sulfur, 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 copper(I) thiocyanate and oxygen
2CuSCNCopper(I) thiocyanate + 5O2Oxygen
⟶
Cu(NO3)2Copper(II) nitrate + CuSCopper(II) sulfide + SSulfur + 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 copper(I) thiocyanate and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
CuSCNCopper(I) thiocyanate2
Reducing
Reducing
O2Oxygen5
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu(NO3)2Copper(II) nitrate1
Redoxed product
–
CuSCopper(II) sulfide1
Oxidized
–
SSulfur1
Oxidized
–
CO2Carbon dioxide2
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of copper(I) thiocyanate and oxygen
2CuSCNCrystalline solid + 5O2Gas
⟶
Cu(NO3)2Crystalline solid + CuSCrystalline solid + SCrystalline solidrhombic + 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
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––

Changes in standard condition (2)

Reaction of copper(I) thiocyanate and oxygen
2CuSCNCrystalline solid + 5O2Gas
⟶
Cu(NO3)2Crystalline solid + CuSCrystalline solid + SCrystalline solidmonoclinic + 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
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––

Changes in aqueous solution (1)

Reaction of copper(I) thiocyanate and oxygen
◆
ΔrG−1366.7 kJ/mol
K2.73 × 10239
pK−239.44
2CuSCNIonized aqueous solution + 5O2Un-ionized aqueous solution
⟶
Cu(NO3)2Ionized aqueous solution + CuSCrystalline solid + SCrystalline solidrhombic + 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
−1427.8−1366.7−205.2–
−713.90−683.35−102.6–
per 1 mol of
−285.56−273.34−41.04–
per 1 mol of
−1427.8−1366.7−205.2–
per 1 mol of
−1427.8−1366.7−205.2–
per 1 mol of
−1427.8−1366.7−205.2–
per 1 mol of
−713.90−683.35−102.6–

Changes in aqueous solution (2)

Reaction of copper(I) thiocyanate and oxygen
◆
ΔrG−1350.0 kJ/mol
K3.23 × 10236
pK−236.51
2CuSCNIonized aqueous solution + 5O2Un-ionized aqueous solution
⟶
Cu(NO3)2Ionized aqueous solution + CuSCrystalline solid + SCrystalline solidrhombic + 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
−1468.4−1350.0−397.5–
−734.20−675.00−198.8–
per 1 mol of
−293.68−270.00−79.50–
per 1 mol of
−1468.4−1350.0−397.5–
per 1 mol of
−1468.4−1350.0−397.5–
per 1 mol of
−1468.4−1350.0−397.5–
per 1 mol of
−734.20−675.00−198.8–

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
CuSCN (cr)–69.9[1]––
CuSCN (ai)148.11[1]142.69[1]184.9[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
Cu(NO3)2 (cr)-302.9[1]–––
Cu(NO3)2 (ai)-349.95[1]-157.02[1]193.3[1]–
Cu(NO3)2 (cr)
3 hydrate
-1217.1[1]–––
Cu(NO3)2 (cr)
6 hydrate
-2110.8[1]–––
CuS (cr)-53.1[1]-53.6[1]66.5[1]47.82[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]
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)