NH4+ → NH3 + H+
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Electrolytic dissociation of ammonium ion yields ammonia and hydrogen ion (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
General equation
- Electrolytic dissociation of ion
- Polyatomic ion ⟶ Cation/Electrically neutral + Anion/Electrically neutral
- Electrolytic dissociation of proton donating ion
- Proton donating ionBrønsted acid ⟶ H+ + Proton accepting/Proton accepting ionConjugate base
Oxidation state of each atom
- Electrolytic dissociation of ammonium ion
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4+ | Ammonium ion | 1 | – Brønsted acid | Polyatomic ion Proton donating ion |
Products
Thermodynamic changes
Changes in standard condition (1)
- Electrolytic dissociation of ammonium ion◆
ΔrG 62.86 kJ/mol K 0.97 × 10−11 pK 11.01
| 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 | 86.40 | 62.86 | 79.1 | −44.8 |
per 1 mol of Ammonium ion | 86.40 | 62.86 | 79.1 | −44.8 |
per 1 mol of | 86.40 | 62.86 | 79.1 | −44.8 |
per 1 mol of Hydrogen ion | 86.40 | 62.86 | 79.1 | −44.8 |
Changes in standard condition (2)
- Electrolytic dissociation of ammonium ion◆
ΔrG 52.81 kJ/mol K 0.56 × 10−9 pK 9.25
| 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 | 52.22 | 52.81 | −2.1 | – |
per 1 mol of Ammonium ion | 52.22 | 52.81 | −2.1 | – |
per 1 mol of | 52.22 | 52.81 | −2.1 | – |
per 1 mol of Hydrogen ion | 52.22 | 52.81 | −2.1 | – |
Thermodynamic data of reactants
| Chemical formula | Standard 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 |
|---|---|---|---|---|
| NH4+ (ao) | -132.51[1] | -79.31[1] | 113.4[1] | 79.9[1] |
* (ao):Un-ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard 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 |
|---|---|---|---|---|
| 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] | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -132.51 kJ · mol−1
- ^ ΔfG°, -79.31 kJ · mol−1
- ^ S°, 113.4 J · K−1 · mol−1
- ^ Cp°, 79.9 J · K−1 · mol−1
- ^ ΔfH°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1