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2NaHCO3 + 2NH3 🔥→ Na2CO3 + (NH4)2CO3

The reaction of sodium hydrogencarbonate and ammonia yields sodium carbonate and ammonium carbonate (Other reactions are here). This reaction is an acid-base 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 acid salt and base
Acid saltBrønsted acid + BaseBrønsted base
SaltConjugate base + (H2O)
Reaction of acid salt and non hydroxide base
Acid saltBrønsted acid + Non hydroxide baseBrønsted base
SaltConjugate acid base

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaHCO3Sodium hydrogencarbonate2
Brønsted acid
Acid salt
NH3Ammonia2
Brønsted base
Base
Non hydroxide base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2CO3Sodium carbonate1
Conjugate base
Conjugate acid base
Salt
(NH4)2CO3Ammonium carbonate1
Conjugate base
Conjugate acid base
Salt

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of sodium hydrogencarbonate and ammonia
ΔrG12.26 kJ/mol
K0.71 × 10−2
pK2.15
2NaHCO3Ionized aqueous solution + 2NH3Un-ionized aqueous solution
🔥
Na2CO3Ionized aqueous solution + (NH4)2CO3Ionized 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
−74.7312.26−292.0
−37.376.130−146.0
per 1 mol of
−37.376.130−146.0
per 1 mol of
−74.7312.26−292.0
per 1 mol of
−74.7312.26−292.0

Changes in aqueous solution (2)

Reaction of sodium hydrogencarbonate and ammonia
ΔrG14.3 kJ/mol
K0.31 × 10−2
pK2.51
2NaHCO3Un-ionized aqueous solution + 2NH3Un-ionized aqueous solution
🔥
Na2CO3Ionized aqueous solution + (NH4)2CO3Ionized 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
−51.214.3−219.2
−25.67.15−109.6
per 1 mol of
−25.67.15−109.6
per 1 mol of
−51.214.3−219.2
per 1 mol of
−51.214.3−219.2

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
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]
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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas

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]
(NH4)2CO3 (ai)-942.15[1]-686.42[1]169.9[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1