2Na + Ba(HCO3)2 → Na2CO3 + BaO + CO↑ + H2O
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- Reaction of and barium hydrogencarbonate
The reaction of and barium hydrogencarbonate yields sodium carbonate, barium oxide, carbon monoxide, and water (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 and barium hydrogencarbonate
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 and barium hydrogencarbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reducing | Reducing | ||
| Ba(HCO3)2 | Barium hydrogencarbonate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2CO3 | Sodium carbonate | 1 | Oxidized | – |
| BaO | Barium oxide | 1 | – | – |
| CO | Carbon monoxide | 1 | Reduced | – |
| H2O | Water | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and barium hydrogencarbonate◆
ΔrG −216.7 kJ/mol K 9.21 × 1037 pK −37.96
| 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 | −185.6 | −216.7 | 104.7 | – |
| −92.80 | −108.3 | 52.35 | – | |
per 1 mol of | −185.6 | −216.7 | 104.7 | – |
per 1 mol of | −185.6 | −216.7 | 104.7 | – |
per 1 mol of | −185.6 | −216.7 | 104.7 | – |
per 1 mol of | −185.6 | −216.7 | 104.7 | – |
per 1 mol of | −185.6 | −216.7 | 104.7 | – |
Changes in standard condition (2)
- Reaction of and barium hydrogencarbonate◆
ΔrG −199.5 kJ/mol K 8.93 × 1034 pK −34.95
| 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 | −196.0 | −199.5 | 11.6 | – |
| −98.00 | −99.75 | 5.80 | – | |
per 1 mol of | −196.0 | −199.5 | 11.6 | – |
per 1 mol of | −196.0 | −199.5 | 11.6 | – |
per 1 mol of | −196.0 | −199.5 | 11.6 | – |
per 1 mol of | −196.0 | −199.5 | 11.6 | – |
per 1 mol of | −196.0 | −199.5 | 11.6 | – |
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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 51.21[1] | 28.24[1] |
| (g) | 107.32[1] | 76.761[1] | 153.712[1] | 20.786[1] |
| Ba(HCO3)2 (ai) | -1921.63[1] | -1734.30[1] | 192.0[1] | – |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
|---|---|---|---|---|
| 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] |
| BaO (cr) | -553.5[1] | -525.1[1] | 70.42[1] | 47.78[1] |
| BaO (g) | -117[1] | – | – | 33.1[1] |
| CO (g) | -110.525[1] | -137.168[1] | 197.674[1] | 29.142[1] |
| CO (ao) | -120.96[1] | -119.90[1] | 104.6[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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 51.21 J · K−1 · mol−1
- ^ Cp°, 28.24 J · K−1 · mol−1
- ^ ΔfH°, 107.32 kJ · mol−1
- ^ ΔfG°, 76.761 kJ · mol−1
- ^ S°, 153.712 J · K−1 · mol−1
- ^ Cp°, 20.786 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°, -1130.68 kJ · mol−1
- ^ ΔfG°, -1044.44 kJ · mol−1
- ^ S°, 134.98 J · K−1 · mol−1
- ^ Cp°, 112.30 J · K−1 · mol−1
- ^ ΔfH°, -1157.38 kJ · mol−1
- ^ ΔfG°, -1051.64 kJ · mol−1
- ^ S°, 61.1 J · K−1 · mol−1
- ^ ΔfH°, -1431.26 kJ · mol−1
- ^ ΔfG°, -1285.31 kJ · mol−1
- ^ S°, 168.11 J · K−1 · mol−1
- ^ Cp°, 145.60 J · K−1 · mol−1
- ^ ΔfH°, -3199.96 kJ · mol−1
- ^ ΔfG°, -2714.2 kJ · mol−1
- ^ S°, 422.2 J · K−1 · mol−1
- ^ ΔfH°, -4081.32 kJ · mol−1
- ^ ΔfG°, -3427.66 kJ · mol−1
- ^ S°, 562.7 J · K−1 · mol−1
- ^ Cp°, 550.32 J · K−1 · mol−1
- ^ ΔfH°, -553.5 kJ · mol−1
- ^ ΔfG°, -525.1 kJ · mol−1
- ^ S°, 70.42 J · K−1 · mol−1
- ^ Cp°, 47.78 J · K−1 · mol−1
- ^ ΔfH°, -117. kJ · mol−1
- ^ Cp°, 33.1 J · K−1 · mol−1
- ^ ΔfH°, -110.525 kJ · mol−1
- ^ ΔfG°, -137.168 kJ · mol−1
- ^ S°, 197.674 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -120.96 kJ · mol−1
- ^ ΔfG°, -119.90 kJ · mol−1
- ^ S°, 104.6 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1