C + Ag2O 🔥→ 2Ag + CO↑
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- Reaction of and silver(I) oxide
The reaction of and silver(I) oxide yields and carbon monoxide. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and silver(I) oxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + 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 silver(I) oxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing Reducing nonmetal | ||
| Ag2O | Silver(I) oxide | 1 | Oxidizing | 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 silver(I) oxide◆
ΔrG −125.97 kJ/mol K 1.17 × 1022 pK −22.07
| 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 | −79.48 | −125.97 | 155.7 | 5.46 |
| −79.48 | −125.97 | 155.7 | 5.46 | |
per 1 mol of | −79.48 | −125.97 | 155.7 | 5.46 |
| −39.74 | −62.985 | 77.85 | 2.73 | |
per 1 mol of | −79.48 | −125.97 | 155.7 | 5.46 |
Changes in standard condition (2)
- Reaction of and silver(I) oxide◆
ΔrG −128.87 kJ/mol K 3.78 × 1022 pK −22.58
| 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 | −81.37 | −128.87 | 159.1 | 7.87 |
| −81.37 | −128.87 | 159.1 | 7.87 | |
per 1 mol of | −81.37 | −128.87 | 159.1 | 7.87 |
| −40.69 | −64.435 | 79.55 | 3.94 | |
per 1 mol of | −81.37 | −128.87 | 159.1 | 7.87 |
Changes in aqueous solution (1)
- Reaction of and silver(I) oxide◆
ΔrG −125.97 kJ/mol K 1.17 × 1022 pK −22.07
| 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 | −79.48 | −125.97 | 155.7 | 5.46 |
| −79.48 | −125.97 | 155.7 | 5.46 | |
per 1 mol of | −79.48 | −125.97 | 155.7 | 5.46 |
| −39.74 | −62.985 | 77.85 | 2.73 | |
per 1 mol of | −79.48 | −125.97 | 155.7 | 5.46 |
Changes in aqueous solution (2)
- Reaction of and silver(I) oxide◆
ΔrG −108.70 kJ/mol K 1.11 × 1019 pK −19.04
| 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 | −89.91 | −108.70 | 62.7 | – |
| −89.91 | −108.70 | 62.7 | – | |
per 1 mol of | −89.91 | −108.70 | 62.7 | – |
| −44.95 | −54.350 | 31.4 | – | |
per 1 mol of | −89.91 | −108.70 | 62.7 | – |
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 |
|---|---|---|---|---|
| (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] |
| Ag2O (cr) | -31.05[1] | -11.20[1] | 121.3[1] | 65.86[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] | 42.55[1] | 25.351[1] |
| (g) | 284.55[1] | 245.65[1] | 172.997[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°, -31.05 kJ · mol−1
- ^ ΔfG°, -11.20 kJ · mol−1
- ^ S°, 121.3 J · K−1 · mol−1
- ^ Cp°, 65.86 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 42.55 J · K−1 · mol−1
- ^ Cp°, 25.351 J · K−1 · mol−1
- ^ ΔfH°, 284.55 kJ · mol−1
- ^ ΔfG°, 245.65 kJ · mol−1
- ^ S°, 172.997 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