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4Na + 3NH4HCO3 → 2Na2CO3 + 3NH3↑ + 3H2O + C

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Reaction of sodium and ammonium hydrogencarbonate
4NaSodium + 3NH4HCO3Ammonium hydrogencarbonate
⟶
2Na2CO3Sodium carbonate + 3NH3↑Ammonia + 3H2OWater + CCarbon

The reaction of sodium and ammonium hydrogencarbonate yields sodium carbonate, ammonia, water, 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

Reaction of sodium and ammonium hydrogencarbonate
4NaSodium + 3NH4HCO3Ammonium hydrogencarbonate
⟶
2Na2CO3Sodium carbonate + 3NH3↑Ammonia + 3H2OWater + CCarbon

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
NaSodium4
Reducing
Reducing
NH4HCO3Ammonium hydrogencarbonate3
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2CO3Sodium carbonate2
Oxidized
–
NH3Ammonia3
–
–
H2OWater3
–
–
CCarbon1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−851.9 kJ/mol
K1.76 × 10149
pK−149.25
4NaCrystalline solid + 3NH4HCO3Crystalline solid
⟶
2Na2CO3Crystalline solid + 3NH3↑Gas + 3H2OLiquid + 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
−709.0−851.9495.2–
per 1 mol of
−177.3−213.0123.8–
−236.3−284.0165.1–
per 1 mol of
−354.5−425.9247.6–
per 1 mol of
−236.3−284.0165.1–
per 1 mol of
−236.3−284.0165.1–
per 1 mol of
−709.0−851.9495.2–

Changes in standard condition (2)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−849.0 kJ/mol
K5.47 × 10148
pK−148.74
4NaCrystalline solid + 3NH4HCO3Crystalline solid
⟶
2Na2CO3Crystalline solid + 3NH3↑Gas + 3H2OLiquid + 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
−707.1−849.0491.9–
per 1 mol of
−176.8−212.3123.0–
−235.7−283.0164.0–
per 1 mol of
−353.6−424.5245.9–
per 1 mol of
−235.7−283.0164.0–
per 1 mol of
−235.7−283.0164.0–
per 1 mol of
−707.1−849.0491.9–

Changes in aqueous solution (1)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−865.81 kJ/mol
K4.82 × 10151
pK−151.68
4NaCrystalline solid + 3NH4HCO3Ionized aqueous solution
⟶
2Na2CO3Ionized aqueous solution + 3NH3↑Gas + 3H2OLiquid + 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
−837.08−865.8196.4–
per 1 mol of
−209.27−216.4524.1–
−279.03−288.6032.1–
per 1 mol of
−418.54−432.9048.2–
per 1 mol of
−279.03−288.6032.1–
per 1 mol of
−279.03−288.6032.1–
per 1 mol of
−837.08−865.8196.4–

Changes in aqueous solution (2)

Reaction of sodium and ammonium hydrogencarbonate
◆
ΔrG−895.96 kJ/mol
K9.23 × 10156
pK−156.97
4NaCrystalline solid + 3NH4HCO3Ionized aqueous solution
⟶
2Na2CO3Ionized aqueous solution + 3NH3↑Un-ionized aqueous solution + 3H2OLiquid + 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
−939.62−895.96−147.1–
per 1 mol of
−234.91−223.99−36.77–
−313.21−298.65−49.03–
per 1 mol of
−469.81−447.98−73.55–
per 1 mol of
−313.21−298.65−49.03–
per 1 mol of
−313.21−298.65−49.03–
per 1 mol of
−939.62−895.96−147.1–

Changes in aqueous solution (3)

Reaction of sodium and ammonium hydrogencarbonate
4NaCrystalline solid + 3NH4HCO3Aqueous solution
⟶
2Na2CO3Ionized aqueous solution + 3NH3↑Gas + 3H2OLiquid + 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
−845.5–––
per 1 mol of
−211.4–––
−281.8–––
per 1 mol of
−422.8–––
per 1 mol of
−281.8–––
per 1 mol of
−281.8–––
per 1 mol of
−845.5–––

Changes in aqueous solution (4)

Reaction of sodium and ammonium hydrogencarbonate
4NaCrystalline solid + 3NH4HCO3Aqueous solution
⟶
2Na2CO3Ionized aqueous solution + 3NH3↑Un-ionized aqueous solution + 3H2OLiquid + 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
−948.0–––
per 1 mol of
−237.0–––
−316.0–––
per 1 mol of
−474.0–––
per 1 mol of
−316.0–––
per 1 mol of
−316.0–––
per 1 mol of
−948.0–––

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
Na2CO3 (cr)-1130.68[1]-1044.44[1]134.98[1]112.30[1]
Na2CO3 (ai)-1157.38[1]-1051.64[1]61.1[1]–
Na2CO3 (cr)
1 hydrate
-1431.26[1]-1285.31[1]168.11[1]145.60[1]
Na2CO3 (cr)
7 hydrate
-3199.96[1]-2714.2[1]422.2[1]–
Na2CO3 (cr)
10 hydrate
-4081.32[1]-3427.66[1]562.7[1]550.32[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]–
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]
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, (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)