2NaI + H2[PtCl6] → Na2[PtCl6] + 2HI↑
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The reaction of sodium iodide and hexachloridoplatinic(IV) acid yields sodium hexachloridoplatinate(IV) and hydrogen iodide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium iodide and hexachloridoplatinic(IV) acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of sodium iodide and hexachloridoplatinic(IV) acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaI | Sodium iodide | 2 | Brønsted base | Salt of volatile acid |
| H2[PtCl6] | Hexachloridoplatinic(IV) acid | 1 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2[PtCl6] | Sodium hexachloridoplatinate(IV) | 1 | Conjugate base | Salt of non volatile acid |
| HI | Hydrogen iodide | 2 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of sodium iodide and hexachloridoplatinic(IV) acid
- 2NaIIonized aqueous solution + H2[PtCl6]Ionized aqueous solutionNa2[PtCl6]Crystalline solid + 2HI↑Gas⟶
| 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 | 195.9 | – | – | – |
per 1 mol of | 97.95 | – | – | – |
per 1 mol of | 195.9 | – | – | – |
per 1 mol of | 195.9 | – | – | – |
per 1 mol of | 97.95 | – | – | – |
Changes in aqueous solution (2)
- Reaction of sodium iodide and hexachloridoplatinic(IV) acid
- 2NaIIonized aqueous solution + H2[PtCl6]Ionized aqueous solutionNa2[PtCl6]Crystalline solid + 2HI↑Ionized aqueous solution⟶
| 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 | 32.5 | – | – | – |
per 1 mol of | 16.3 | – | – | – |
per 1 mol of | 32.5 | – | – | – |
per 1 mol of | 32.5 | – | – | – |
per 1 mol of | 16.3 | – | – | – |
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 |
|---|---|---|---|---|
| NaI (cr) | -287.78[1] | -286.06[1] | 98.53[1] | 52.09[1] |
| NaI (g) | -79.5[1] | -121.0[1] | 248.978[1] | 36.65[1] |
| NaI (ai) | -295.31[1] | -313.47[1] | 170.3[1] | -95.8[1] |
| NaI (cr) 1 hydrate | -883.096[1] | -771.10[1] | 196.2[1] | – |
| H2[PtCl6] (ai) | -668.2[1] | -482.7[1] | 219.7[1] | – |
| H2[PtCl6] (cr) 6 hydrate | -2371.1[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):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 |
|---|---|---|---|---|
| Na2[PtCl6] (cr) | -1115.9[1] | – | – | – |
| Na2[PtCl6] (cr) 2 hydrate | -1723.8[1] | – | – | – |
| Na2[PtCl6] (cr) 6 hydrate | -2912.1[1] | – | – | – |
| HI (g) | 26.48[1] | 1.70[1] | 206.594[1] | 29.158[1] |
| HI (ai) | -55.19[1] | -51.57[1] | 111.3[1] | -142.3[1] |
* (cr):Crystalline solid, (g):Gas, (ai):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°, -287.78 kJ · mol−1
- ^ ΔfG°, -286.06 kJ · mol−1
- ^ S°, 98.53 J · K−1 · mol−1
- ^ Cp°, 52.09 J · K−1 · mol−1
- ^ ΔfH°, -79.5 kJ · mol−1
- ^ ΔfG°, -121.0 kJ · mol−1
- ^ S°, 248.978 J · K−1 · mol−1
- ^ Cp°, 36.65 J · K−1 · mol−1
- ^ ΔfH°, -295.31 kJ · mol−1
- ^ ΔfG°, -313.47 kJ · mol−1
- ^ S°, 170.3 J · K−1 · mol−1
- ^ Cp°, -95.8 J · K−1 · mol−1
- ^ ΔfH°, -883.096 kJ · mol−1
- ^ ΔfG°, -771.10 kJ · mol−1
- ^ S°, 196.2 J · K−1 · mol−1
- ^ ΔfH°, -668.2 kJ · mol−1
- ^ ΔfG°, -482.7 kJ · mol−1
- ^ S°, 219.7 J · K−1 · mol−1
- ^ ΔfH°, -2371.1 kJ · mol−1
- ^ ΔfH°, -1115.9 kJ · mol−1
- ^ ΔfH°, -1723.8 kJ · mol−1
- ^ ΔfH°, -2912.1 kJ · mol−1
- ^ ΔfH°, 26.48 kJ · mol−1
- ^ ΔfG°, 1.70 kJ · mol−1
- ^ S°, 206.594 J · K−1 · mol−1
- ^ Cp°, 29.158 J · K−1 · mol−1
- ^ ΔfH°, -55.19 kJ · mol−1
- ^ ΔfG°, -51.57 kJ · mol−1
- ^ S°, 111.3 J · K−1 · mol−1
- ^ Cp°, -142.3 J · K−1 · mol−1