CoSO4 + 4H2O 💧⚡→ Co(OH)2 + S + 3H2O2
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- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
Electrolysis of aqueous cobalt(II) sulfate yields cobalt(II) hydroxide, , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
General equation
- Electrolysis of aqueous solution with water as reducing agent
- Miscible with water/Very soluble in water/Soluble in waterOxidizing agent + H2OReducing agent💧⚡⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CoSO4 | Cobalt(II) sulfate | 1 | Oxidizing | Very soluble in water |
| H2O | Water | 4 | Reducing | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co(OH)2 | Cobalt(II) hydroxide | 1 | – | – |
| 1 | Reduced | – | ||
| 3 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 919.7 kJ/mol K 0.75 × 10−161 pK 161.12
| 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 | – | 919.7 | – | – |
per 1 mol of | – | 919.7 | – | – |
per 1 mol of | – | 229.9 | – | – |
per 1 mol of | – | 919.7 | – | – |
| – | 919.7 | – | – | |
| – | 306.6 | – | – |
Changes in standard condition (2)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
| – | – | – | – |
Changes in standard condition (3)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 915.5 kJ/mol K 0.41 × 10−160 pK 160.39
| 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 | 928.6 | 915.5 | 42 | – |
per 1 mol of | 928.6 | 915.5 | 42 | – |
per 1 mol of | 232.2 | 228.9 | 11 | – |
per 1 mol of | 928.6 | 915.5 | 42 | – |
| 928.6 | 915.5 | 42 | – | |
| 309.5 | 305.2 | 14 | – |
Changes in standard condition (4)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
| 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 | 928.9 | – | – | – |
per 1 mol of | 928.9 | – | – | – |
per 1 mol of | 232.2 | – | – | – |
per 1 mol of | 928.9 | – | – | – |
| 928.9 | – | – | – | |
| 309.6 | – | – | – |
Changes in standard condition (5)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 911.7 kJ/mol K 0.19 × 10−159 pK 159.72
| 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 | – | 911.7 | – | – |
per 1 mol of | – | 911.7 | – | – |
per 1 mol of | – | 227.9 | – | – |
per 1 mol of | – | 911.7 | – | – |
| – | 911.7 | – | – | |
| – | 303.9 | – | – |
Changes in standard condition (6)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
| – | – | – | – | |
| – | – | – | – |
Changes in aqueous solution (1)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 907.0 kJ/mol K 0.13 × 10−158 pK 158.90
| 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 | – | 907.0 | – | – |
per 1 mol of | – | 907.0 | – | – |
per 1 mol of | – | 226.8 | – | – |
per 1 mol of | – | 907.0 | – | – |
| – | 907.0 | – | – | |
| – | 302.3 | – | – |
Changes in aqueous solution (2)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 878.6 kJ/mol K 0.12 × 10−153 pK 153.92
| 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 | – | 878.6 | – | – |
per 1 mol of | – | 878.6 | – | – |
per 1 mol of | – | 219.7 | – | – |
per 1 mol of | – | 878.6 | – | – |
| – | 878.6 | – | – | |
| – | 292.9 | – | – |
Changes in aqueous solution (3)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 874.4 kJ/mol K 0.65 × 10−153 pK 153.19
| 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 | 918.4 | 874.4 | 145 | – |
per 1 mol of | 918.4 | 874.4 | 145 | – |
per 1 mol of | 229.6 | 218.6 | 36.3 | – |
per 1 mol of | 918.4 | 874.4 | 145 | – |
| 918.4 | 874.4 | 145 | – | |
| 306.1 | 291.5 | 48.3 | – |
Changes in aqueous solution (4)
- Electrolysis of aqueous cobalt(II) sulfate with water as reducing agent◆
ΔrG 870.6 kJ/mol K 0.30 × 10−152 pK 152.52
| 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 | – | 870.6 | – | – |
per 1 mol of | – | 870.6 | – | – |
per 1 mol of | – | 217.7 | – | – |
per 1 mol of | – | 870.6 | – | – |
| – | 870.6 | – | – | |
| – | 290.2 | – | – |
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 |
|---|---|---|---|---|
| CoSO4 (cr) | -888.3[1] | -782.3[1] | 118.0[1] | – |
| CoSO4 (ai) | -967.3[1] | -799.1[1] | -92[1] | – |
| CoSO4 (cr) 6 hydrate | -2683.6[1] | -2235.36[1] | 367.61[1] | 353.38[1] |
| CoSO4 (cr) 7 hydrate | -2979.93[1] | -2473.42[1] | 406.06[1] | 390.49[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, (ai):Ionized aqueous solution, (l):Liquid, (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 |
|---|---|---|---|---|
| Co(OH)2 (cr) blue, precipitated | – | -450.1[1] | – | – |
| Co(OH)2 (cr) pink, precipitated | -539.7[1] | -454.3[1] | 79[1] | – |
| Co(OH)2 (cr) pink, precipitated, aged | – | -458.1[1] | – | – |
| Co(OH)2 (ai) | -518.0[1] | -369.0[1] | -134[1] | – |
| Co(OH)2 (ao) | – | -421.7[1] | – | – |
| (cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
| (cr) monoclinic | 0.33[1] | – | – | – |
| (g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
| (l) | -187.78[1] | -120.35[1] | 109.6[1] | 89.1[1] |
| (g) | -136.31[1] | -105.57[1] | 232.7[1] | 43.1[1] |
| (ao) | -191.17[1] | -134.03[1] | 143.9[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (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°, -888.3 kJ · mol−1
- ^ ΔfG°, -782.3 kJ · mol−1
- ^ S°, 118.0 J · K−1 · mol−1
- ^ ΔfH°, -967.3 kJ · mol−1
- ^ ΔfG°, -799.1 kJ · mol−1
- ^ S°, -92. J · K−1 · mol−1
- ^ ΔfH°, -2683.6 kJ · mol−1
- ^ ΔfG°, -2235.36 kJ · mol−1
- ^ S°, 367.61 J · K−1 · mol−1
- ^ Cp°, 353.38 J · K−1 · mol−1
- ^ ΔfH°, -2979.93 kJ · mol−1
- ^ ΔfG°, -2473.42 kJ · mol−1
- ^ S°, 406.06 J · K−1 · mol−1
- ^ Cp°, 390.49 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
- ^ ΔfG°, -450.1 kJ · mol−1
- ^ ΔfH°, -539.7 kJ · mol−1
- ^ ΔfG°, -454.3 kJ · mol−1
- ^ S°, 79. J · K−1 · mol−1
- ^ ΔfG°, -458.1 kJ · mol−1
- ^ ΔfH°, -518.0 kJ · mol−1
- ^ ΔfG°, -369.0 kJ · mol−1
- ^ S°, -134. J · K−1 · mol−1
- ^ ΔfG°, -421.7 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -187.78 kJ · mol−1
- ^ ΔfG°, -120.35 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ Cp°, 89.1 J · K−1 · mol−1
- ^ ΔfH°, -136.31 kJ · mol−1
- ^ ΔfG°, -105.57 kJ · mol−1
- ^ S°, 232.7 J · K−1 · mol−1
- ^ Cp°, 43.1 J · K−1 · mol−1
- ^ ΔfH°, -191.17 kJ · mol−1
- ^ ΔfG°, -134.03 kJ · mol−1
- ^ S°, 143.9 J · K−1 · mol−1