C + K2O 🔥→ 2K + CO↑
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- Reaction of and potassium oxide
The reaction of and potassium oxide yields and carbon monoxide (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 potassium oxide
General equation
- Reaction of reducing species and hardly reducible species
- Reducing speciesReducing agent + Hardly reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
- Reducing agent + OxideOxidizing agent🔥⟶ Elementary substance/OxideReduction product + Oxidation product
Oxidation state of each atom
- Reaction of and potassium oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing Reducing nonmetal | ||
| K2O | Potassium oxide | 1 | Oxidizing | Hardly reducible Oxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 2 | Reduced | – Elementary substance | ||
| CO | Carbon monoxide | 1 | Oxidized | – Oxide |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and potassium oxide◆
ΔrG 184.9 kJ/mol K 0.40 × 10−32 pK 32.39
| 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 | 251.0 | 184.9 | 226.2 | −3.9 |
| 251.0 | 184.9 | 226.2 | −3.9 | |
per 1 mol of | 251.0 | 184.9 | 226.2 | −3.9 |
| 125.5 | 92.45 | 113.1 | −1.9 | |
per 1 mol of | 251.0 | 184.9 | 226.2 | −3.9 |
Changes in standard condition (2)
- Reaction of and potassium oxide◆
ΔrG 182.0 kJ/mol K 0.13 × 10−31 pK 31.89
| 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 | 249.1 | 182.0 | 229.6 | −1.5 |
| 249.1 | 182.0 | 229.6 | −1.5 | |
per 1 mol of | 249.1 | 182.0 | 229.6 | −1.5 |
| 124.5 | 91.00 | 114.8 | −0.75 | |
per 1 mol of | 249.1 | 182.0 | 229.6 | −1.5 |
Changes in aqueous solution (1)
- Reaction of and potassium oxide◆
ΔrG 184.9 kJ/mol K 0.40 × 10−32 pK 32.39
| 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 | 251.0 | 184.9 | 226.2 | −3.9 |
| 251.0 | 184.9 | 226.2 | −3.9 | |
per 1 mol of | 251.0 | 184.9 | 226.2 | −3.9 |
| 125.5 | 92.45 | 113.1 | −1.9 | |
per 1 mol of | 251.0 | 184.9 | 226.2 | −3.9 |
Changes in aqueous solution (2)
- Reaction of and potassium oxide◆
ΔrG 202.2 kJ/mol K 0.38 × 10−35 pK 35.42
| 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 | 240.5 | 202.2 | 133.1 | – |
| 240.5 | 202.2 | 133.1 | – | |
per 1 mol of | 240.5 | 202.2 | 133.1 | – |
| 120.3 | 101.1 | 66.55 | – | |
per 1 mol of | 240.5 | 202.2 | 133.1 | – |
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) graphite | 0[1] | 0[1] | 5.740[1] | 8.527[1] |
| (cr) diamond | 1.895[1] | 2.900[1] | 2.377[1] | 6.113[1] |
| (g) | 716.682[1] | 671.257[1] | 158.096[1] | 20.838[1] |
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 64.18[1] | 29.58[1] |
| (g) | 89.24[1] | 60.59[1] | 160.336[1] | 20.786[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] | – |
* (cr):Crystalline solid, (g):Gas, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 5.740 J · K−1 · mol−1
- ^ Cp°, 8.527 J · K−1 · mol−1
- ^ ΔfH°, 1.895 kJ · mol−1
- ^ ΔfG°, 2.900 kJ · mol−1
- ^ S°, 2.377 J · K−1 · mol−1
- ^ Cp°, 6.113 J · K−1 · mol−1
- ^ ΔfH°, 716.682 kJ · mol−1
- ^ ΔfG°, 671.257 kJ · mol−1
- ^ S°, 158.096 J · K−1 · mol−1
- ^ Cp°, 20.838 J · K−1 · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 64.18 J · K−1 · mol−1
- ^ Cp°, 29.58 J · K−1 · mol−1
- ^ ΔfH°, 89.24 kJ · mol−1
- ^ ΔfG°, 60.59 kJ · mol−1
- ^ S°, 160.336 J · K−1 · mol−1
- ^ Cp°, 20.786 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
- 2James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfG°, -322.1 kJ · mol−1 - p.280
- ^ S°, 94.1 J · K−1 · mol−1 - p.280
- ^ Cp°, 83.7 J · K−1 · mol−1 - p.280