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4Na + 3NH4SCN → 2NaSCN + Na2S + 4NH3↑ + C

The reaction of sodium and ammonium thiocyanate yields sodium thiocyanate, sodium sulfide, ammonia, and carbon (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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium4
Reducing
Reducing
NH4SCNAmmonium thiocyanate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaSCNSodium thiocyanate2
Oxidized
Na2SSodium sulfide1
Oxidized
NH3Ammonia4
CCarbon1
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and ammonium thiocyanate
4NaCrystalline solid + 3NH4SCNCrystalline solid
2NaSCNCrystalline solid + Na2SCrystalline solid + 4NH3Gas + CCrystalline solidgraphite
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
−654.1
per 1 mol of
−163.5
−218.0
per 1 mol of
−327.1
per 1 mol of
−654.1
per 1 mol of
−163.5
per 1 mol of
−654.1

Changes in standard condition (2)

Reaction of sodium and ammonium thiocyanate
4NaCrystalline solid + 3NH4SCNCrystalline solid
2NaSCNCrystalline solid + Na2SCrystalline solid + 4NH3Gas + CCrystalline soliddiamond
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
−652.2
per 1 mol of
−163.1
−217.4
per 1 mol of
−326.1
per 1 mol of
−652.2
per 1 mol of
−163.1
per 1 mol of
−652.2

Changes in aqueous solution (1)

Reaction of sodium and ammonium thiocyanate
ΔrG−882.5 kJ/mol
K4.05 × 10154
pK−154.61
4NaCrystalline solid + 3NH4SCNIonized aqueous solution
2NaSCNIonized aqueous solution + Na2SIonized aqueous solution + 4NH3Gas + CCrystalline solidgraphite
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
−790.9−882.5307.5
per 1 mol of
−197.7−220.676.88
−263.6−294.2102.5
per 1 mol of
−395.4−441.3153.8
per 1 mol of
−790.9−882.5307.5
per 1 mol of
−197.7−220.676.88
per 1 mol of
−790.9−882.5307.5

Changes in aqueous solution (2)

Reaction of sodium and ammonium thiocyanate
ΔrG−922.7 kJ/mol
K4.47 × 10161
pK−161.65
4NaCrystalline solid + 3NH4SCNIonized aqueous solution
2NaSCNIonized aqueous solution + Na2SIonized aqueous solution + 4NH3Un-ionized aqueous solution + CCrystalline solidgraphite
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
−927.6−922.7−17.1
per 1 mol of
−231.9−230.7−4.28
−309.2−307.6−5.70
per 1 mol of
−463.8−461.4−8.55
per 1 mol of
−927.6−922.7−17.1
per 1 mol of
−231.9−230.7−4.28
per 1 mol of
−927.6−922.7−17.1

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[1]
NH4SCN (cr)-78.7[1]
NH4SCN (ai)-56.07[1]13.40[1]257.7[1]39.7[1]
* (cr):Crystalline solid, (g):Gas, (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
NaSCN (cr)-170.50[1]
NaSCN (ai)-163.68[1]-169.18[1]203.3[1]6.3[1]
Na2S (cr)-364.8[1]-349.8[1]83.7[1]
Na2S (ai)-447.3[1]-438.1[1]103.3[1]
Na2S (cr)
4.5 hydrate
-1725.9[1]
Na2S (cr)
5 hydrate
-1886.6[1]
Na2S (cr)
9 hydrate
-3074.0[1]
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[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]
* (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)