8PbCrO4 + 6e− → 8PbO + Cr2O3 + 3Cr2O72−
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- Reduction of lead(II) chromate
- 8PbCrO4Lead(II) chromate + 6e−Electron8PbOLead(II) oxide + Cr2O3Chromium(III) oxide + 3Cr2O72−Dichromate ion⟶
Reduction of lead(II) chromate yields lead(II) oxide, chromium(III) oxide, and dichromate 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 lead(II) chromate
- 8PbCrO4Lead(II) chromate + 6e−Electron8PbOLead(II) oxide + Cr2O3Chromium(III) oxide + 3Cr2O72−Dichromate ion⟶
General equation
- Reduction of reducible species
- ReactantOxidizing agent + e− ⟶ ProductReduction product
Oxidation state of each atom
- Reduction of lead(II) chromate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbCrO4 | Lead(II) chromate | 8 | Oxidizing | – |
| e− | Electron | 6 | – | Electron |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO | Lead(II) oxide | 8 | – | – |
| Cr2O3 | Chromium(III) oxide | 1 | Reduced | – |
| Cr2O72− | Dichromate ion | 3 | – | – |
Thermodynamic changes
Changes in standard condition
- Reduction of lead(II) chromate
| 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 | 98.0 | – | – | – |
per 1 mol of | 12.3 | – | – | – |
per 1 mol of Electron | 16.3 | – | – | – |
per 1 mol of | 12.3 | – | – | – |
per 1 mol of | 98.0 | – | – | – |
per 1 mol of Dichromate ion | 32.7 | – | – | – |
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 |
|---|---|---|---|---|
| PbCrO4 (cr) | -930.9[1] | – | – | – |
| e− | – | – | – | – |
* (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 |
|---|---|---|---|---|
| PbO (cr) massicot, yellow | -217.32[1] | -187.89[1] | 68.70[1] | 45.77[1] |
| PbO (cr) litharge, red | -218.99[1] | -188.93[1] | 66.5[1] | 45.81[1] |
| PbO (cr) 1/3 hydrate | – | -266.5[1] | – | – |
| Cr2O3 (cr) | -1139.7[1] | -1058.1[1] | 81.2[1] | 118.74[1] |
| Cr2O3 (cr) 1 hydrate | -1506[1] | – | – | – |
| Cr2O3 (cr) 2 hydrate | -1845[1] | – | – | – |
| Cr2O3 (cr) 3 hydrate | -2171[1] | – | – | – |
| Cr2O72− (ao) | -1490.3[1] | -1301.1[1] | 261.9[1] | – |
* (cr):Crystalline solid, (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°, -930.9 kJ · mol−1
- ^ ΔfH°, -217.32 kJ · mol−1
- ^ ΔfG°, -187.89 kJ · mol−1
- ^ S°, 68.70 J · K−1 · mol−1
- ^ Cp°, 45.77 J · K−1 · mol−1
- ^ ΔfH°, -218.99 kJ · mol−1
- ^ ΔfG°, -188.93 kJ · mol−1
- ^ S°, 66.5 J · K−1 · mol−1
- ^ Cp°, 45.81 J · K−1 · mol−1
- ^ ΔfG°, -266.5 kJ · mol−1
- ^ ΔfH°, -1139.7 kJ · mol−1
- ^ ΔfG°, -1058.1 kJ · mol−1
- ^ S°, 81.2 J · K−1 · mol−1
- ^ Cp°, 118.74 J · K−1 · mol−1
- ^ ΔfH°, -1506. kJ · mol−1
- ^ ΔfH°, -1845. kJ · mol−1
- ^ ΔfH°, -2171. kJ · mol−1
- ^ ΔfH°, -1490.3 kJ · mol−1
- ^ ΔfG°, -1301.1 kJ · mol−1
- ^ S°, 261.9 J · K−1 · mol−1