4(NH4)3AsO4 + 6HNO3 🔥→ 9NH4NO2 + 4H3AsO4 + 3H2↑
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- Reaction of ammonium arsenate and nitric acid
The reaction of ammonium arsenate and nitric acid yields ammonium nitrite, arsenic acid, and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium arsenate and nitric acid
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of ammonium arsenate and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| (NH4)3AsO4 | Ammonium arsenate | 4 | Reducing | Reducing |
| HNO3 | Nitric acid | 6 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO2 | Ammonium nitrite | 9 | Redoxed product | – |
| H3AsO4 | Arsenic acid | 4 | – | – |
| 3 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium arsenate and nitric acid
- 4(NH4)3AsO4Crystalline solid + 6HNO3Liquid9NH4NO2Crystalline solid + 4H3AsO4Crystalline solid + 3↑Gas🔥⟶
| 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 | 255.7 | – | – | – |
per 1 mol of | 63.92 | – | – | – |
per 1 mol of | 42.62 | – | – | – |
per 1 mol of | 28.41 | – | – | – |
per 1 mol of | 63.92 | – | – | – |
| 85.23 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium arsenate and nitric acid◆
ΔrG 144.4 kJ/mol K 0.50 × 10−25 pK 25.30 - 4(NH4)3AsO4Ionized aqueous solution + 6HNO3Ionized aqueous solution9NH4NO2Ionized aqueous solution + 4H3AsO4Un-ionized aqueous solution + 3↑Gas🔥⟶
| 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 | 642.0 | 144.4 | 1668 | – |
per 1 mol of | 160.5 | 36.10 | 417.0 | – |
per 1 mol of | 107.0 | 24.07 | 278.0 | – |
per 1 mol of | 71.33 | 16.04 | 185.3 | – |
per 1 mol of | 160.5 | 36.10 | 417.0 | – |
| 214.0 | 48.13 | 556.0 | – |
Changes in aqueous solution (2)
- Reaction of ammonium arsenate and nitric acid◆
ΔrG 197.2 kJ/mol K 0.28 × 10−34 pK 34.55 - 4(NH4)3AsO4Ionized aqueous solution + 6HNO3Ionized aqueous solution9NH4NO2Ionized aqueous solution + 4H3AsO4Un-ionized aqueous solution + 3↑Un-ionized 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 | 629.4 | 197.2 | 3007 | – |
per 1 mol of | 157.3 | 49.30 | 751.8 | – |
per 1 mol of | 104.9 | 32.87 | 501.2 | – |
per 1 mol of | 69.93 | 21.91 | 334.1 | – |
per 1 mol of | 157.3 | 49.30 | 751.8 | – |
| 209.8 | 65.73 | 1002 | – |
Changes in aqueous solution (3)
- Reaction of ammonium arsenate and nitric acid
- 4(NH4)3AsO4Ionized aqueous solution + 6HNO3Ionized aqueous solution9NH4NO2Ionized aqueous solution + 4H3AsO4Aqueous solution + 3↑Gas🔥⟶
| 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 | 633.6 | – | – | – |
per 1 mol of | 158.4 | – | – | – |
per 1 mol of | 105.6 | – | – | – |
per 1 mol of | 70.40 | – | – | – |
per 1 mol of | 158.4 | – | – | – |
| 211.2 | – | – | – |
Changes in aqueous solution (4)
- Reaction of ammonium arsenate and nitric acid
- 4(NH4)3AsO4Ionized aqueous solution + 6HNO3Ionized aqueous solution9NH4NO2Ionized aqueous solution + 4H3AsO4Aqueous solution + 3↑Un-ionized 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 | 621.0 | – | – | – |
per 1 mol of | 155.3 | – | – | – |
per 1 mol of | 103.5 | – | – | – |
per 1 mol of | 69.00 | – | – | – |
per 1 mol of | 155.3 | – | – | – |
| 207.0 | – | – | – |
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)3AsO4 (cr) | -1286.2[1] | – | – | – |
| (NH4)3AsO4 (ai) | -1285.66[1] | -886.32[1] | 177.4[1] | – |
| (NH4)3AsO4 (cr) 3 hydrate | -2166.9[1] | – | – | – |
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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 |
|---|---|---|---|---|
| NH4NO2 (cr) | -256.5[1] | – | – | – |
| NH4NO2 (ai) | -237.2[1] | -111.6[1] | 236.4[1] | -17.6[1] |
| H3AsO4 (cr) | -906.3[1] | – | – | – |
| H3AsO4 (ao) | -902.5[1] | -766.0[1] | 184[1] | – |
| H3AsO4 (aq) | -904.6[1] | – | – | – |
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):Aqueous solution, (g):Gas
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°, -1286.2 kJ · mol−1
- ^ ΔfH°, -1285.66 kJ · mol−1
- ^ ΔfG°, -886.32 kJ · mol−1
- ^ S°, 177.4 J · K−1 · mol−1
- ^ ΔfH°, -2166.9 kJ · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -256.5 kJ · mol−1
- ^ ΔfH°, -237.2 kJ · mol−1
- ^ ΔfG°, -111.6 kJ · mol−1
- ^ S°, 236.4 J · K−1 · mol−1
- ^ Cp°, -17.6 J · K−1 · mol−1
- ^ ΔfH°, -906.3 kJ · mol−1
- ^ ΔfH°, -902.5 kJ · mol−1
- ^ ΔfG°, -766.0 kJ · mol−1
- ^ S°, 184. J · K−1 · mol−1
- ^ ΔfH°, -904.6 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1