4H2 + Co3O4 🔥→ 3Co + 4H2O
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- Reaction of and cobalt(II,III) oxide
The reaction of and cobalt(II,III) oxide yields 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 cobalt(II,III) oxide
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
- Reducing agent + OxideOxidizing agent🔥⟶ Elementary substance/OxideReduction product + Oxidation product
Oxidation state of each atom
- Reaction of and cobalt(II,III) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 4 | Reducing | Reducing Reducing nonmetal | ||
| Co3O4 | Cobalt(II,III) oxide | 1 | Oxidizing | Oxidizing Oxide |
Products
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and cobalt(II,III) oxide◆
ΔrG −175 kJ/mol K 4.56 × 1030 pK −30.66
| 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 | −252 | −175 | −255.5 | 136.9 |
| −63.0 | −43.8 | −63.88 | 34.23 | |
per 1 mol of | −252 | −175 | −255.5 | 136.9 |
| −84.0 | −58.3 | −85.17 | 45.63 | |
per 1 mol of | −63.0 | −43.8 | −63.88 | 34.23 |
Changes in standard condition (2)
- Reaction of and cobalt(II,III) oxide◆
ΔrG −174 kJ/mol K 3.04 × 1030 pK −30.48
| 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 | −251 | −174 | −253.5 | – |
| −62.8 | −43.5 | −63.38 | – | |
per 1 mol of | −251 | −174 | −253.5 | – |
| −83.7 | −58.0 | −84.50 | – | |
per 1 mol of | −62.8 | −43.5 | −63.38 | – |
Changes in aqueous solution
- Reaction of and cobalt(II,III) oxide◆
ΔrG −245 kJ/mol K 8.36 × 1042 pK −42.92
| 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 | −236 | −245 | −2041 | – |
| −59.0 | −61.3 | −510.3 | – | |
per 1 mol of | −236 | −245 | −2041 | – |
| −78.7 | −81.7 | −680.3 | – | |
per 1 mol of | −59.0 | −61.3 | −510.3 | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[1] | – |
| Co3O4 (cr) | -891[1] | -774[1] | 102.5[1] | 123.4[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid
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 |
|---|---|---|---|---|
| (cr) α, hexagonal | 0[1] | 0[1] | 30.04[1] | 24.81[1] |
| (cr) β, face centered cubic | 0.46[1] | 0.25[1] | 30.71[1] | – |
| (g) | 424.7[1] | 380.3[1] | 179.515[1] | 23.020[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, (g):Gas, (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°, 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
- ^ ΔfH°, -891. kJ · mol−1
- ^ ΔfG°, -774. kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 123.4 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 30.04 J · K−1 · mol−1
- ^ Cp°, 24.81 J · K−1 · mol−1
- ^ ΔfH°, 0.46 kJ · mol−1
- ^ ΔfG°, 0.25 kJ · mol−1
- ^ S°, 30.71 J · K−1 · mol−1
- ^ ΔfH°, 424.7 kJ · mol−1
- ^ ΔfG°, 380.3 kJ · mol−1
- ^ S°, 179.515 J · K−1 · mol−1
- ^ Cp°, 23.020 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