KI + 2AgNO3 🔥→ KIO3 + 2NO↑ + Ag2O
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The reaction of potassium iodide and silver(I) nitrate yields potassium iodate, nitrogen monoxide, and silver(I) oxide (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 silver(I) nitrate
General equation
- Reaction of oxidizable species and oxidizing species
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of potassium iodide and silver(I) nitrate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 1 | Reducing | Oxidizable |
| AgNO3 | Silver(I) nitrate | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 1 | Oxidized | – |
| NO | Nitrogen monoxide | 2 | Reduced | – |
| Ag2O | Silver(I) oxide | 1 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium iodide and silver(I) nitrate◆
ΔrG 135.26 kJ/mol K 0.20 × 10−23 pK 23.70
| 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 | 224.76 | 135.26 | 306.1 | −7.00 |
per 1 mol of | 224.76 | 135.26 | 306.1 | −7.00 |
per 1 mol of | 112.38 | 67.630 | 153.1 | −3.50 |
per 1 mol of | 224.76 | 135.26 | 306.1 | −7.00 |
per 1 mol of | 112.38 | 67.630 | 153.1 | −3.50 |
per 1 mol of | 224.76 | 135.26 | 306.1 | −7.00 |
Changes in aqueous solution (1)
- Reaction of potassium iodide and silver(I) nitrate◆
ΔrG 153.9 kJ/mol K 0.11 × 10−26 pK 26.96
| 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 | 187.0 | 153.9 | 111.5 | – |
per 1 mol of | 187.0 | 153.9 | 111.5 | – |
per 1 mol of | 93.50 | 76.95 | 55.75 | – |
per 1 mol of | 187.0 | 153.9 | 111.5 | – |
per 1 mol of | 93.50 | 76.95 | 55.75 | – |
per 1 mol of | 187.0 | 153.9 | 111.5 | – |
Changes in aqueous solution (2)
- Reaction of potassium iodide and silver(I) nitrate◆
ΔrG 150.5 kJ/mol K 0.43 × 10−26 pK 26.37
| 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 | – | 150.5 | – | – |
per 1 mol of | – | 150.5 | – | – |
per 1 mol of | – | 75.25 | – | – |
per 1 mol of | – | 150.5 | – | – |
per 1 mol of | – | 75.25 | – | – |
per 1 mol of | – | 150.5 | – | – |
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 |
|---|---|---|---|---|
| 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] |
| AgNO3 (cr) | -124.39[1] | -33.41[1] | 140.92[1] | 93.05[1] |
| AgNO3 (ai) | -101.80[1] | -34.16[1] | 219.2[1] | -64.9[1] |
| AgNO3 (ao) | – | -32.49[1] | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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 |
|---|---|---|---|---|
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| Ag2O (cr) | -31.05[1] | -11.20[1] | 121.3[1] | 65.86[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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°, -124.39 kJ · mol−1
- ^ ΔfG°, -33.41 kJ · mol−1
- ^ S°, 140.92 J · K−1 · mol−1
- ^ Cp°, 93.05 J · K−1 · mol−1
- ^ ΔfH°, -101.80 kJ · mol−1
- ^ ΔfG°, -34.16 kJ · mol−1
- ^ S°, 219.2 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfG°, -32.49 kJ · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 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