PbCrO4 🔥⚡→ PbO + Cr + O3↑
Last updated:
- Molten salt electrolysis of lead(II) chromate
Molten salt electrolysis of lead(II) chromate yields lead(II) oxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Molten salt electrolysis of lead(II) chromate
General equation
- Molten salt electrolysis
- SaltSelf redox agent🔥⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Molten salt electrolysis of lead(II) chromate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbCrO4 | Lead(II) chromate | 1 | Self redox agent | Salt |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO | Lead(II) oxide | 1 | – | – |
| 1 | Reduced | – | ||
| 1 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Molten salt electrolysis 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 | 856.3 | – | – | – |
per 1 mol of | 856.3 | – | – | – |
per 1 mol of | 856.3 | – | – | – |
| 856.3 | – | – | – | |
| 856.3 | – | – | – |
Changes in standard condition (2)
- Molten salt electrolysis 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 | 854.6 | – | – | – |
per 1 mol of | 854.6 | – | – | – |
per 1 mol of | 854.6 | – | – | – |
| 854.6 | – | – | – | |
| 854.6 | – | – | – |
Changes in aqueous solution (1)
- Molten salt electrolysis 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 | 856.3 | – | – | – |
per 1 mol of | 856.3 | – | – | – |
per 1 mol of | 856.3 | – | – | – |
| 856.3 | – | – | – | |
| 856.3 | – | – | – |
Changes in aqueous solution (2)
- Molten salt electrolysis 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 | 839.5 | – | – | – |
per 1 mol of | 839.5 | – | – | – |
per 1 mol of | 839.5 | – | – | – |
| 839.5 | – | – | – | |
| 839.5 | – | – | – |
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] | – | – | – |
* (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] | – | – |
| (cr) | 0[1] | 0[1] | 23.77[1] | 23.35[1] |
| (g) | 396.6[1] | 351.8[1] | 174.50[1] | 20.79[1] |
| (g) | 142.7[1] | 163.2[1] | 238.93[1] | 39.20[1] |
| (ao) | 125.9[1] | 174.1[1] | 146[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°, -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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 23.77 J · K−1 · mol−1
- ^ Cp°, 23.35 J · K−1 · mol−1
- ^ ΔfH°, 396.6 kJ · mol−1
- ^ ΔfG°, 351.8 kJ · mol−1
- ^ S°, 174.50 J · K−1 · mol−1
- ^ Cp°, 20.79 J · K−1 · mol−1
- ^ ΔfH°, 142.7 kJ · mol−1
- ^ ΔfG°, 163.2 kJ · mol−1
- ^ S°, 238.93 J · K−1 · mol−1
- ^ Cp°, 39.20 J · K−1 · mol−1
- ^ ΔfH°, 125.9 kJ · mol−1
- ^ ΔfG°, 174.1 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1