Na2Cr2O7 + 2HIO3 → 2NaIO3 + 2CrO3 + H2O
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- Reaction of sodium dichromate and iodic acid
The reaction of sodium dichromate and iodic acid yields sodium iodate, chromium(VI) oxide, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium dichromate and iodic acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of sodium dichromate and iodic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2Cr2O7 | Sodium dichromate | 1 | Brønsted base | Salt of weak acid |
| HIO3 | Iodic acid | 2 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaIO3 | Sodium iodate | 2 | Conjugate base | Salt of strong acid |
| CrO3 | Chromium(VI) oxide | 2 | – | Acidic oxide |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium dichromate and iodic acid
| 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 | 10.4 | – | – | – |
per 1 mol of | 10.4 | – | – | – |
per 1 mol of | 5.20 | – | – | – |
per 1 mol of | 5.20 | – | – | – |
per 1 mol of | 5.20 | – | – | – |
per 1 mol of | 10.4 | – | – | – |
Changes in aqueous solution
- Reaction of sodium dichromate and iodic acid
| 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 | 5.5 | – | – | – |
per 1 mol of | 5.5 | – | – | – |
per 1 mol of | 2.8 | – | – | – |
per 1 mol of | 2.8 | – | – | – |
per 1 mol of | 2.8 | – | – | – |
per 1 mol of | 5.5 | – | – | – |
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 |
|---|---|---|---|---|
| Na2Cr2O7 (cr) | -1978.6[1] | – | – | – |
| Na2Cr2O7 (ai) | -1970.7[1] | -1824.9[1] | 379.9[1] | – |
| Na2Cr2O7 (cr) 2 hydrate | -2574.8[1] | – | – | – |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
* (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| 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] | – | – | – |
| CrO3 (cr) | -589.5[1] | – | – | – |
| CrO3 (g) | -385.8[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, (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°, -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°, -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°, -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°, -589.5 kJ · mol−1
- ^ ΔfH°, -385.8 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