9Ba(CH3COO)2 + 16HNO3 → 9Ba(HCO3)2 + 8NH4CN + 10H2CO3
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The reaction of barium acetate and nitric acid yields barium hydrogencarbonate, ammonium cyanide, and carbonic acid (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 barium acetate 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 barium acetate and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ba(CH3COO)2 | Barium acetate | 9 | Reducing | Reducing |
| HNO3 | Nitric acid | 16 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ba(HCO3)2 | Barium hydrogencarbonate | 9 | Oxidized | – |
| NH4CN | Ammonium cyanide | 8 | Redoxed product | – |
| H2CO3 | Carbonic acid | 10 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of barium acetate and nitric acid◆
ΔrG −7621.0 kJ/mol K 1.38 × 101335 pK −1335.14 - 9Ba(CH3COO)2Ionized aqueous solution + 16HNO3Ionized aqueous solution9Ba(HCO3)2Ionized aqueous solution + 8NH4CNIonized aqueous solution + 10H2CO3Un-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 | −7242.4 | −7621.0 | 1274.4 | – |
per 1 mol of | −804.71 | −846.78 | 141.60 | – |
per 1 mol of | −452.65 | −476.31 | 79.650 | – |
per 1 mol of | −804.71 | −846.78 | 141.60 | – |
per 1 mol of | −905.30 | −952.63 | 159.30 | – |
per 1 mol of | −724.24 | −762.10 | 127.44 | – |
Changes in standard condition (2)
- Reaction of barium acetate and nitric acid
- 9Ba(CH3COO)2Ionized aqueous solution + 16HNO3Ionized aqueous solution9Ba(HCO3)2Ionized aqueous solution + 8NH4CNAqueous solution + 10H2CO3Un-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 | −7128.8 | – | – | – |
per 1 mol of | −792.09 | – | – | – |
per 1 mol of | −445.55 | – | – | – |
per 1 mol of | −792.09 | – | – | – |
per 1 mol of | −891.10 | – | – | – |
per 1 mol of | −712.88 | – | – | – |
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 |
|---|---|---|---|---|
| Ba(CH3COO)2 (cr) | -1484.5[1] | – | – | – |
| Ba(CH3COO)2 (ai) | -1509.67[1] | -1299.39[1] | 182.8[1] | – |
| Ba(CH3COO)2 (cr) 3 hydrate | -2369.0[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 |
|---|---|---|---|---|
| Ba(HCO3)2 (ai) | -1921.63[1] | -1734.30[1] | 192.0[1] | – |
| NH4CN (cr) | 0.42[1] | – | – | 134[1] |
| NH4CN (ai) | 18.0[1] | 93.0[1] | 207.5[1] | – |
| NH4CN (aq) | 32.2[1] | – | – | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (aq):Aqueous solution, (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°, -1484.5 kJ · mol−1
- ^ ΔfH°, -1509.67 kJ · mol−1
- ^ ΔfG°, -1299.39 kJ · mol−1
- ^ S°, 182.8 J · K−1 · mol−1
- ^ ΔfH°, -2369.0 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°, -1921.63 kJ · mol−1
- ^ ΔfG°, -1734.30 kJ · mol−1
- ^ S°, 192.0 J · K−1 · mol−1
- ^ ΔfH°, 0.42 kJ · mol−1
- ^ Cp°, 134. J · K−1 · mol−1
- ^ ΔfH°, 18.0 kJ · mol−1
- ^ ΔfG°, 93.0 kJ · mol−1
- ^ S°, 207.5 J · K−1 · mol−1
- ^ ΔfH°, 32.2 kJ · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1