4KI + Rb2CO3 🔥→ 2K2O + I2 + 2RbI + CO↑
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- Reaction of potassium iodide and rubidium carbonate
The reaction of potassium iodide and rubidium carbonate yields potassium oxide, , rubidium iodide, 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 potassium iodide and rubidium carbonate
General equation
- Reaction of oxidizable species and reducible species
- Oxidizable speciesReducing agent + Reducible speciesOxidizing agent🔥⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium iodide and rubidium carbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 4 | Reducing | Oxidizable |
| Rb2CO3 | Rubidium carbonate | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2O | Potassium oxide | 2 | – | – |
| 1 | Oxidized | – | ||
| RbI | Rubidium iodide | 2 | – | – |
| CO | Carbon monoxide | 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and rubidium carbonate◆
ΔrG 911.5 kJ/mol K 0.21 × 10−159 pK 159.69
| 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 | 946.5 | 911.5 | 132.2 | 28.0 |
per 1 mol of | 236.6 | 227.9 | 33.05 | 7.00 |
per 1 mol of | 946.5 | 911.5 | 132.2 | 28.0 |
per 1 mol of | 473.3 | 455.8 | 66.10 | 14.0 |
| 946.5 | 911.5 | 132.2 | 28.0 | |
per 1 mol of | 473.3 | 455.8 | 66.10 | 14.0 |
per 1 mol of | 946.5 | 911.5 | 132.2 | 28.0 |
Changes in aqueous solution (1)
- Reaction of potassium iodide and rubidium carbonate◆
ΔrG 999.1 kJ/mol K 0.92 × 10−175 pK 175.03
| 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 | 986.1 | 999.1 | −53.1 | – |
per 1 mol of | 246.5 | 249.8 | −13.3 | – |
per 1 mol of | 986.1 | 999.1 | −53.1 | – |
per 1 mol of | 493.1 | 499.6 | −26.6 | – |
| 986.1 | 999.1 | −53.1 | – | |
per 1 mol of | 493.1 | 499.6 | −26.6 | – |
per 1 mol of | 986.1 | 999.1 | −53.1 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and rubidium carbonate◆
ΔrG 1016.4 kJ/mol K 0.86 × 10−178 pK 178.07
| 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 | 975.7 | 1016.4 | −146.2 | – |
per 1 mol of | 243.9 | 254.10 | −36.55 | – |
per 1 mol of | 975.7 | 1016.4 | −146.2 | – |
per 1 mol of | 487.9 | 508.20 | −73.10 | – |
| 975.7 | 1016.4 | −146.2 | – | |
per 1 mol of | 487.9 | 508.20 | −73.10 | – |
per 1 mol of | 975.7 | 1016.4 | −146.2 | – |
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 |
|---|---|---|---|---|
| KI (cr) | -327.900[1] | -324.892[1] | 106.32[1] | 52.93[1] |
| KI (g) | -125.5[1] | -166.1[1] | 258.3[1] | 37.11[1] |
| KI (ai) | -307.57[1] | -334.85[1] | 213.8[1] | -120.5[1] |
| Rb2CO3 (cr) | -1136.0[1] | -1051.0[1] | 181.33[1] | 117.61[1] |
| Rb2CO3 (ai) | -1179.47[1] | -1095.78[1] | 186.2[1] | – |
| Rb2CO3 (cr) 1 hydrate | -1448.5[1] | – | – | – |
| Rb2CO3 (cr) 1.5 hydrate | -1604.5[1] | – | – | – |
| Rb2CO3 (cr) 3 hydrate | -2048.1[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution
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 |
|---|---|---|---|---|
| K2O (cr) | -361.5[1] | -322.1[2] | 94.1[2] | 83.7[2] |
| K2O (g) | -63[1] | – | – | – |
| (cr) | 0[1] | 0[1] | 116.135[1] | 54.438[1] |
| (g) | 62.438[1] | 19.327[1] | 260.69[1] | 36.90[1] |
| (ao) | 22.6[1] | 16.40[1] | 137.2[1] | – |
| RbI (cr) | -333.80[1] | -328.86[1] | 118.41[1] | 53.18[1] |
| RbI (g) | -134.3[1] | -174.1[1] | 268.81[1] | 37.36[1] |
| RbI (ai) | -306.35[1] | -335.56[1] | 232.6[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, (ai):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°, -327.900 kJ · mol−1
- ^ ΔfG°, -324.892 kJ · mol−1
- ^ S°, 106.32 J · K−1 · mol−1
- ^ Cp°, 52.93 J · K−1 · mol−1
- ^ ΔfH°, -125.5 kJ · mol−1
- ^ ΔfG°, -166.1 kJ · mol−1
- ^ S°, 258.3 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -307.57 kJ · mol−1
- ^ ΔfG°, -334.85 kJ · mol−1
- ^ S°, 213.8 J · K−1 · mol−1
- ^ Cp°, -120.5 J · K−1 · mol−1
- ^ ΔfH°, -1136.0 kJ · mol−1
- ^ ΔfG°, -1051.0 kJ · mol−1
- ^ S°, 181.33 J · K−1 · mol−1
- ^ Cp°, 117.61 J · K−1 · mol−1
- ^ ΔfH°, -1179.47 kJ · mol−1
- ^ ΔfG°, -1095.78 kJ · mol−1
- ^ S°, 186.2 J · K−1 · mol−1
- ^ ΔfH°, -1448.5 kJ · mol−1
- ^ ΔfH°, -1604.5 kJ · mol−1
- ^ ΔfH°, -2048.1 kJ · mol−1
- ^ ΔfH°, -361.5 kJ · mol−1
- ^ ΔfH°, -63. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 116.135 J · K−1 · mol−1
- ^ Cp°, 54.438 J · K−1 · mol−1
- ^ ΔfH°, 62.438 kJ · mol−1
- ^ ΔfG°, 19.327 kJ · mol−1
- ^ S°, 260.69 J · K−1 · mol−1
- ^ Cp°, 36.90 J · K−1 · mol−1
- ^ ΔfH°, 22.6 kJ · mol−1
- ^ ΔfG°, 16.40 kJ · mol−1
- ^ S°, 137.2 J · K−1 · mol−1
- ^ ΔfH°, -333.80 kJ · mol−1
- ^ ΔfG°, -328.86 kJ · mol−1
- ^ S°, 118.41 J · K−1 · mol−1
- ^ Cp°, 53.18 J · K−1 · mol−1
- ^ ΔfH°, -134.3 kJ · mol−1
- ^ ΔfG°, -174.1 kJ · mol−1
- ^ S°, 268.81 J · K−1 · mol−1
- ^ Cp°, 37.36 J · K−1 · mol−1
- ^ ΔfH°, -306.35 kJ · mol−1
- ^ ΔfG°, -335.56 kJ · mol−1
- ^ S°, 232.6 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