2KI + 8AgNO3 + 8H+ 🔥→ 2KNO3 + 2HIO3 + 3N2O3↑ + 8Ag+ + 3H2O
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- Reaction of potassium iodide and silver(I) nitrate under acidic condition
- 2KIPotassium iodide + 8AgNO3Silver(I) nitrate + 8H+Hydrogen ion2KNO3Potassium nitrate + 2HIO3Iodic acid + 3N2O3↑Dinitrogen trioxide + 8Ag+Silver(I) ion + 3H2OWater🔥⟶
The reaction of potassium iodide, silver(I) nitrate, and hydrogen ion yields potassium nitrate, iodic acid, dinitrogen trioxide, silver(I) ion, and water (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 under acidic condition
- 2KIPotassium iodide + 8AgNO3Silver(I) nitrate + 8H+Hydrogen ion2KNO3Potassium nitrate + 2HIO3Iodic acid + 3N2O3↑Dinitrogen trioxide + 8Ag+Silver(I) ion + 3H2OWater🔥⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of potassium iodide and silver(I) nitrate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KI | Potassium iodide | 2 | Reducing | Oxidizable |
| AgNO3 | Silver(I) nitrate | 8 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 8 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 2 | – | – |
| HIO3 | Iodic acid | 2 | Oxidized | – |
| N2O3 | Dinitrogen trioxide | 3 | Reduced | – |
| Ag+ | Silver(I) ion | 8 | – | – |
| H2O | Water | 3 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of potassium iodide and silver(I) nitrate under acidic condition◆
ΔrG 212.6 kJ/mol K 0.57 × 10−37 pK 37.25
| 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 | 325.8 | 212.6 | 378.4 | – |
per 1 mol of | 162.9 | 106.3 | 189.2 | – |
per 1 mol of | 40.73 | 26.57 | 47.30 | – |
per 1 mol of Hydrogen ion | 40.73 | 26.57 | 47.30 | – |
per 1 mol of | 162.9 | 106.3 | 189.2 | – |
per 1 mol of | 162.9 | 106.3 | 189.2 | – |
per 1 mol of | 108.6 | 70.87 | 126.1 | – |
per 1 mol of Silver(I) ion | 40.73 | 26.57 | 47.30 | – |
per 1 mol of | 108.6 | 70.87 | 126.1 | – |
Changes in standard condition (2)
- Reaction of potassium iodide and silver(I) nitrate under acidic condition◆
ΔrG 199.2 kJ/mol K 0.13 × 10−34 pK 34.90
| 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 | – | 199.2 | – | – |
per 1 mol of | – | 99.60 | – | – |
per 1 mol of | – | 24.90 | – | – |
per 1 mol of Hydrogen ion | – | 24.90 | – | – |
per 1 mol of | – | 99.60 | – | – |
per 1 mol of | – | 99.60 | – | – |
per 1 mol of | – | 66.40 | – | – |
per 1 mol of Silver(I) ion | – | 24.90 | – | – |
per 1 mol of | – | 66.40 | – | – |
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] | – | – |
| H+ (g) | 1536.202[1] | – | – | – |
| H+ (ao) | 0[1] | 0[1] | 0[1] | 0[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 |
|---|---|---|---|---|
| KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
| KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[1] |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
| N2O3 (l) | 50.29[1] | – | – | – |
| N2O3 (g) | 83.72[1] | 139.46[1] | 312.28[1] | 65.61[1] |
| Ag+ (g) | 1021.73[1] | – | – | – |
| Ag+ (ao) | 105.579[1] | 77.107[1] | 72.68[1] | 21.8[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, (ao):Un-ionized aqueous solution, (l):Liquid, (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°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfH°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 J · K−1 · mol−1
- ^ ΔfH°, 50.29 kJ · mol−1
- ^ ΔfH°, 83.72 kJ · mol−1
- ^ ΔfG°, 139.46 kJ · mol−1
- ^ S°, 312.28 J · K−1 · mol−1
- ^ Cp°, 65.61 J · K−1 · mol−1
- ^ ΔfH°, 1021.73 kJ · mol−1
- ^ ΔfH°, 105.579 kJ · mol−1
- ^ ΔfG°, 77.107 kJ · mol−1
- ^ S°, 72.68 J · K−1 · mol−1
- ^ Cp°, 21.8 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