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2Na + 3NH4HCO3 → NaCN + NaHCO3 + (NH4)2CO3 + 3H2O

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Reaction of sodium and ammonium hydrogencarbonate
2NaSodium + 3NH4HCO3Ammonium hydrogencarbonate
⟶
NaCNSodium cyanide + NaHCO3Sodium hydrogencarbonate + (NH4)2CO3Ammonium carbonate + 3H2OWater

The reaction of sodium and ammonium hydrogencarbonate yields sodium cyanide, sodium hydrogencarbonate, ammonium carbonate, and water (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 sodium and ammonium hydrogencarbonate
2NaSodium + 3NH4HCO3Ammonium hydrogencarbonate
⟶
NaCNSodium cyanide + NaHCO3Sodium hydrogencarbonate + (NH4)2CO3Ammonium carbonate + 3H2OWater

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 sodium and ammonium hydrogencarbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium2
Reducing
Reducing
NH4HCO3Ammonium hydrogencarbonate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaCNSodium cyanide1
Redoxed product
–
NaHCO3Sodium hydrogencarbonate1
Oxidized
–
(NH4)2CO3Ammonium carbonate1
–
–
H2OWater3
–
–

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−337.8 kJ/mol
K1.51 × 1059
pK−59.18
2NaCrystalline solid + 3NH4HCO3Ionized aqueous solution
⟶
NaCNIonized aqueous solution + NaHCO3Ionized aqueous solution + (NH4)2CO3Ionized aqueous solution + 3H2OLiquid
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
−347.8−337.8−33.3–
per 1 mol of
−173.9−168.9−16.6–
−115.9−112.6−11.1–
per 1 mol of
−347.8−337.8−33.3–
−347.8−337.8−33.3–
per 1 mol of
−347.8−337.8−33.3–
per 1 mol of
−115.9−112.6−11.1–

Changes in aqueous solution (2)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−338.8 kJ/mol
K2.27 × 1059
pK−59.36
2NaCrystalline solid + 3NH4HCO3Ionized aqueous solution
⟶
NaCNIonized aqueous solution + NaHCO3Un-ionized aqueous solution + (NH4)2CO3Ionized aqueous solution + 3H2OLiquid
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
−359.5−338.8−69.7–
per 1 mol of
−179.8−169.4−34.9–
−119.8−112.9−23.2–
per 1 mol of
−359.5−338.8−69.7–
−359.5−338.8−69.7–
per 1 mol of
−359.5−338.8−69.7–
per 1 mol of
−119.8−112.9−23.2–

Changes in aqueous solution (3)

Reaction of sodium and ammonium hydrogencarbonate
2NaCrystalline solid + 3NH4HCO3Aqueous solution
⟶
NaCNIonized aqueous solution + NaHCO3Ionized aqueous solution + (NH4)2CO3Ionized aqueous solution + 3H2OLiquid
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
−356.2–––
per 1 mol of
−178.1–––
−118.7–––
per 1 mol of
−356.2–––
−356.2–––
per 1 mol of
−356.2–––
per 1 mol of
−118.7–––

Changes in aqueous solution (4)

Reaction of sodium and ammonium hydrogencarbonate
2NaCrystalline solid + 3NH4HCO3Aqueous solution
⟶
NaCNIonized aqueous solution + NaHCO3Un-ionized aqueous solution + (NH4)2CO3Ionized aqueous solution + 3H2OLiquid
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
−367.9–––
per 1 mol of
−183.9–––
−122.6–––
per 1 mol of
−367.9–––
−367.9–––
per 1 mol of
−367.9–––
per 1 mol of
−122.6–––

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]
NH4HCO3 (cr)-849.4[1]-665.9[1]120.9[1]–
NH4HCO3 (ai)-824.50[1]-666.07[1]204.6[1]–
NH4HCO3 (aq)-821.7[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (aq):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
NaCN (cr)
cubic
-87.49[1]-76.43[1]115.60[1]70.37[1]
NaCN (cr)
orthorhombic
-90.75[1]–––
NaCN (g)109[1]79.94[1]249.43[1]51.17[1]
NaCN (ai)-89.5[1]-89.5[1]153.1[1]–
NaCN (cr)
1/2 hydrate
-235.77[1]–––
NaCN (cr)
2 hydrate
-679.77[1]–––
NaHCO3 (cr)-950.81[1]-851.0[1]101.7[1]87.61[1]
NaHCO3 (ai)-932.11[1]-848.66[1]150.2[1]–
NaHCO3 (ao)-943.9[1]-849.7[1]113.8[1]–
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid

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)