6NaCl + 16Ag2CrO4 + 62H+ → 3Na2Cr2O7 + 6ClO2↑ + 10Cr3+ + 32Ag+ + 31H2O
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- Reaction of sodium chloride and silver(I) chromate under acidic condition
- 6NaClSodium chloride + 16Ag2CrO4Silver(I) chromate + 62H+Hydrogen ion3Na2Cr2O7Sodium dichromate + 6ClO2↑Chlorine dioxide + 10Cr3+Chromium(III) ion + 32Ag+Silver(I) ion + 31H2OWater⟶
The reaction of sodium chloride, silver(I) chromate, and hydrogen ion yields sodium dichromate, chlorine dioxide, chromium(III) ion, 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 sodium chloride and silver(I) chromate under acidic condition
- 6NaClSodium chloride + 16Ag2CrO4Silver(I) chromate + 62H+Hydrogen ion3Na2Cr2O7Sodium dichromate + 6ClO2↑Chlorine dioxide + 10Cr3+Chromium(III) ion + 32Ag+Silver(I) ion + 31H2OWater⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of sodium chloride and silver(I) chromate under acidic condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaCl | Sodium chloride | 6 | Reducing | Hardly oxidizable |
| Ag2CrO4 | Silver(I) chromate | 16 | Oxidizing | Oxidizing under acidic condition |
| H+ | Hydrogen ion | 62 | – | Hydrogen ion |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2Cr2O7 | Sodium dichromate | 3 | – | – |
| ClO2 | Chlorine dioxide | 6 | Oxidized | – |
| Cr3+ | Chromium(III) ion | 10 | Reduced | – |
| Ag+ | Silver(I) ion | 32 | – | – |
| H2O | Water | 31 | – | Water |
Thermodynamic changes
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 |
|---|---|---|---|---|
| NaCl (cr) | -411.153[1] | -384.138[1] | 72.13[1] | 50.50[1] |
| NaCl (g) | -176.65[1] | -196.66[1] | 229.81[1] | 35.77[1] |
| NaCl (ai) | -407.27[1] | -393.133[1] | 115.5[1] | -90.0[1] |
| Ag2CrO4 (cr) | -731.74[1] | -641.76[1] | 217.6[1] | 142.26[1] |
| Ag2CrO4 (ai) | -669.98[1] | -573.52[1] | 195.8[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 |
|---|---|---|---|---|
| Na2Cr2O7 (cr) | -1978.6[1] | – | – | – |
| Na2Cr2O7 (ai) | -1970.7[1] | -1824.9[1] | 379.9[1] | – |
| Na2Cr2O7 (cr) 2 hydrate | -2574.8[1] | – | – | – |
| ClO2 (g) | 102.5[1] | 120.5[1] | 256.84[1] | 41.97[1] |
| ClO2 (ao) | 74.9[1] | 120.1[1] | 164.8[1] | – |
| Cr3+ (g) | 5648.4[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, (g):Gas, (ao):Un-ionized aqueous solution, (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°, -411.153 kJ · mol−1
- ^ ΔfG°, -384.138 kJ · mol−1
- ^ S°, 72.13 J · K−1 · mol−1
- ^ Cp°, 50.50 J · K−1 · mol−1
- ^ ΔfH°, -176.65 kJ · mol−1
- ^ ΔfG°, -196.66 kJ · mol−1
- ^ S°, 229.81 J · K−1 · mol−1
- ^ Cp°, 35.77 J · K−1 · mol−1
- ^ ΔfH°, -407.27 kJ · mol−1
- ^ ΔfG°, -393.133 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ Cp°, -90.0 J · K−1 · mol−1
- ^ ΔfH°, -731.74 kJ · mol−1
- ^ ΔfG°, -641.76 kJ · mol−1
- ^ S°, 217.6 J · K−1 · mol−1
- ^ Cp°, 142.26 J · K−1 · mol−1
- ^ ΔfH°, -669.98 kJ · mol−1
- ^ ΔfG°, -573.52 kJ · mol−1
- ^ S°, 195.8 J · K−1 · 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°, -1978.6 kJ · mol−1
- ^ ΔfH°, -1970.7 kJ · mol−1
- ^ ΔfG°, -1824.9 kJ · mol−1
- ^ S°, 379.9 J · K−1 · mol−1
- ^ ΔfH°, -2574.8 kJ · mol−1
- ^ ΔfH°, 102.5 kJ · mol−1
- ^ ΔfG°, 120.5 kJ · mol−1
- ^ S°, 256.84 J · K−1 · mol−1
- ^ Cp°, 41.97 J · K−1 · mol−1
- ^ ΔfH°, 74.9 kJ · mol−1
- ^ ΔfG°, 120.1 kJ · mol−1
- ^ S°, 164.8 J · K−1 · mol−1
- ^ ΔfH°, 5648.4 kJ · 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