10NaCl + 2NaIO3 + 6H2O 🔥→ 12NaOH + 5Cl2↑ + I2
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- Reaction of sodium chloride and sodium iodate under neutral condition
The reaction of sodium chloride, sodium iodate, and water yields sodium 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
- Reaction of sodium chloride and sodium iodate under neutral condition
General equation
- Reaction of hardly oxidizable species and oxidizing species under neutral condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H2ONon-redox agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of sodium chloride and sodium iodate under neutral condition
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaCl | Sodium chloride | 10 | Reducing | Hardly oxidizable |
| NaIO3 | Sodium iodate | 2 | Oxidizing | Oxidizing |
| H2O | Water | 6 | – | Water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaOH | Sodium hydroxide | 12 | – | – |
| 5 | Oxidized | – | ||
| 1 | Reduced | – |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium chloride and sodium iodate under neutral condition
| 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 | 1682.778 | – | – | −202.3 |
per 1 mol of | 168.2778 | – | – | −20.23 |
per 1 mol of | 841.3890 | – | – | −101.2 |
per 1 mol of | 280.4630 | – | – | −33.72 |
per 1 mol of | 140.2315 | – | – | −16.86 |
| 336.5556 | – | – | −40.46 | |
| 1682.778 | – | – | −202.3 |
Changes in aqueous solution (1)
- Reaction of sodium chloride and sodium iodate under neutral condition◆
ΔrG 1120.5 kJ/mol K 0.50 × 10−196 pK 196.30
| 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 | 1091.9 | 1120.5 | −99.5 | – |
per 1 mol of | 109.19 | 112.05 | −9.95 | – |
per 1 mol of | 545.95 | 560.25 | −49.8 | – |
per 1 mol of | 181.98 | 186.75 | −16.6 | – |
per 1 mol of | 90.992 | 93.375 | −8.29 | – |
| 218.38 | 224.10 | −19.9 | – | |
| 1091.9 | 1120.5 | −99.5 | – |
Changes in aqueous solution (2)
- Reaction of sodium chloride and sodium iodate under neutral condition◆
ΔrG 1155.2 kJ/mol K 0.41 × 10−202 pK 202.38
| 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 | 974.9 | 1155.2 | −610 | – |
per 1 mol of | 97.49 | 115.52 | −61.0 | – |
per 1 mol of | 487.4 | 577.60 | −305 | – |
per 1 mol of | 162.5 | 192.53 | −102 | – |
per 1 mol of | 81.24 | 96.267 | −50.8 | – |
| 195.0 | 231.04 | −122 | – | |
| 974.9 | 1155.2 | −610 | – |
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] |
| NaIO3 (cr) | -481.788[1] | – | – | 92.0[1] |
| NaIO3 (ai) | -461.5[1] | -389.9[1] | 177.4[1] | – |
| NaIO3 (cr) 1 hydrate | -779.48[1] | -634.03[1] | 162.3[1] | – |
| NaIO3 (cr) 5 hydrate | -1952.25[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| NaOH (cr) | -425.609[1] | -379.494[1] | 64.455[1] | 59.54[1] |
| NaOH (g) | -207.1[1] | -210.0[1] | 228.43[1] | 48.37[1] |
| NaOH (ai) | -470.114[1] | -419.150[1] | 48.1[1] | -102.1[1] |
| NaOH (cr) 1 hydrate | -734.543[1] | -629.338[1] | 99.50[1] | 90.17[1] |
| NaOH (l) 2 hydrate | -1019.076[1] | -873.091[1] | 195.979[1] | 239.41[1] |
| NaOH (l) 3.5 hydrate | -1459.798[1] | -1236.356[1] | 286.089[1] | 354.43[1] |
| NaOH (l) 4 hydrate | -1605.15[1] | -1356.64[1] | 318.70[1] | – |
| NaOH (l) 5 hydrate | -1894.31[1] | -1596.34[1] | 386.06[1] | – |
| NaOH (l) 7 hydrate | -2469.02[1] | -2073.80[1] | 526.31[1] | – |
| (g) | 0[1] | 0[1] | 223.066[1] | 33.907[1] |
| (ao) | -23.4[1] | 6.94[1] | 121[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] | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-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°, -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°, -481.788 kJ · mol−1
- ^ Cp°, 92.0 J · K−1 · mol−1
- ^ ΔfH°, -461.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 177.4 J · K−1 · mol−1
- ^ ΔfH°, -779.48 kJ · mol−1
- ^ ΔfG°, -634.03 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, -1952.25 kJ · 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
- ^ ΔfH°, -425.609 kJ · mol−1
- ^ ΔfG°, -379.494 kJ · mol−1
- ^ S°, 64.455 J · K−1 · mol−1
- ^ Cp°, 59.54 J · K−1 · mol−1
- ^ ΔfH°, -207.1 kJ · mol−1
- ^ ΔfG°, -210.0 kJ · mol−1
- ^ S°, 228.43 J · K−1 · mol−1
- ^ Cp°, 48.37 J · K−1 · mol−1
- ^ ΔfH°, -470.114 kJ · mol−1
- ^ ΔfG°, -419.150 kJ · mol−1
- ^ S°, 48.1 J · K−1 · mol−1
- ^ Cp°, -102.1 J · K−1 · mol−1
- ^ ΔfH°, -734.543 kJ · mol−1
- ^ ΔfG°, -629.338 kJ · mol−1
- ^ S°, 99.50 J · K−1 · mol−1
- ^ Cp°, 90.17 J · K−1 · mol−1
- ^ ΔfH°, -1019.076 kJ · mol−1
- ^ ΔfG°, -873.091 kJ · mol−1
- ^ S°, 195.979 J · K−1 · mol−1
- ^ Cp°, 239.41 J · K−1 · mol−1
- ^ ΔfH°, -1459.798 kJ · mol−1
- ^ ΔfG°, -1236.356 kJ · mol−1
- ^ S°, 286.089 J · K−1 · mol−1
- ^ Cp°, 354.43 J · K−1 · mol−1
- ^ ΔfH°, -1605.15 kJ · mol−1
- ^ ΔfG°, -1356.64 kJ · mol−1
- ^ S°, 318.70 J · K−1 · mol−1
- ^ ΔfH°, -1894.31 kJ · mol−1
- ^ ΔfG°, -1596.34 kJ · mol−1
- ^ S°, 386.06 J · K−1 · mol−1
- ^ ΔfH°, -2469.02 kJ · mol−1
- ^ ΔfG°, -2073.80 kJ · mol−1
- ^ S°, 526.31 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 223.066 J · K−1 · mol−1
- ^ Cp°, 33.907 J · K−1 · mol−1
- ^ ΔfH°, -23.4 kJ · mol−1
- ^ ΔfG°, 6.94 kJ · mol−1
- ^ S°, 121. J · K−1 · 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