Ba(HCO3)2 + 2e− → BaOH+ + C2O42− + OH−
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- Reduction of barium hydrogencarbonate
- Ba(HCO3)2Barium hydrogencarbonate + 2e−ElectronBaOH+Barium hydroxide ion + C2O42−Oxalate ion + OH−Hydroxide ion⟶
Reduction of barium hydrogencarbonate yields barium hydroxide ion, oxalate ion, and hydroxide ion (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reduction of barium hydrogencarbonate
- Ba(HCO3)2Barium hydrogencarbonate + 2e−ElectronBaOH+Barium hydroxide ion + C2O42−Oxalate ion + OH−Hydroxide ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of barium hydrogencarbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ba(HCO3)2 | Barium hydrogencarbonate | 1 | Oxidizing | – |
| e− | Electron | 2 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaOH+ | Barium hydroxide ion | 1 | – | – |
| C2O42− | Oxalate ion | 1 | Reduced | – |
| OH− | Hydroxide ion | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of barium hydrogencarbonate◆
ΔrG 172.7 kJ/mol K 0.55 × 10−30 pK 30.26 - Ba(HCO3)2Ionized aqueous solution + 2e−BaOH+Un-ionized aqueous solution + C2O42−Un-ionized aqueous solution + OH−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 | – | 172.7 | – | – |
per 1 mol of | – | 172.7 | – | – |
per 1 mol of Electron | – | 86.35 | – | – |
per 1 mol of Barium hydroxide ion | – | 172.7 | – | – |
per 1 mol of Oxalate ion | – | 172.7 | – | – |
per 1 mol of Hydroxide ion | – | 172.7 | – | – |
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(HCO3)2 (ai) | -1921.63[1] | -1734.30[1] | 192.0[1] | – |
| e− | – | – | – | – |
* (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 |
|---|---|---|---|---|
| BaOH+ (ao) | – | -730.5[1] | – | – |
| C2O42− (ao) | -825.1[1] | -673.9[1] | 45.6[1] | – |
| OH− (g) | -143.5[1] | – | – | – |
| OH− (ao) | -229.994[1] | -157.244[1] | -10.75[1] | -148.5[1] |
* (ao):Un-ionized 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°, -1921.63 kJ · mol−1
- ^ ΔfG°, -1734.30 kJ · mol−1
- ^ S°, 192.0 J · K−1 · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ ΔfH°, -825.1 kJ · mol−1
- ^ ΔfG°, -673.9 kJ · mol−1
- ^ S°, 45.6 J · K−1 · mol−1
- ^ ΔfH°, -143.5 kJ · mol−1
- ^ ΔfH°, -229.994 kJ · mol−1
- ^ ΔfG°, -157.244 kJ · mol−1
- ^ S°, -10.75 J · K−1 · mol−1
- ^ Cp°, -148.5 J · K−1 · mol−1