Na2SO3 + H2SiO3 → Na2SiO3 + H2SO3
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The reaction of sodium sulfite and metasilicic acid yields sodium metasilicate and sulfurous acid (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 sulfite and metasilicic 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 sulfite and metasilicic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2SO3 | Sodium sulfite | 1 | Brønsted base | Salt of volatile acid |
| H2SiO3 | Metasilicic acid | 1 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2SiO3 | Sodium metasilicate | 1 | Conjugate base | Salt of non volatile acid |
| H2SO3 | Sulfurous acid | 1 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium sulfite and metasilicic 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 | 103.7 | – | – | – |
per 1 mol of | 103.7 | – | – | – |
per 1 mol of | 103.7 | – | – | – |
per 1 mol of | 103.7 | – | – | – |
per 1 mol of | 103.7 | – | – | – |
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 |
|---|---|---|---|---|
| Na2SO3 (cr) | -1100.8[1] | -1012.5[1] | 145.94[1] | 120.25[1] |
| Na2SO3 (ai) | -1115.87[1] | -1010.39[1] | 87.9[1] | – |
| Na2SO3 (cr) 7 hydrate | -3162.3[1] | -2676.1[1] | 444[1] | – |
| H2SiO3 (cr) | -1188.7[1] | -1092.4[1] | 134[1] | – |
| H2SiO3 (ao) | -1182.8[1] | -1079.4[1] | 109[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 |
|---|---|---|---|---|
| Na2SiO3 (cr) | -1554.90[1] | -1462.80[1] | 113.85[1] | – |
| Na2SiO3 (vit) | -1540.1[1] | – | – | – |
| Na2SiO3 (aq) | -1586.2[1] | – | – | – |
| Na2SiO3 (cr) 5 hydrate | -3048.5[1] | – | – | – |
| Na2SiO3 (cr) 9 hydrate | -4228.8[1] | – | – | – |
| H2SO3 (ao) | -608.81[1] | -537.81[1] | 232.2[1] | – |
* (cr):Crystalline solid, (vit):Vitreous liquid, (aq):Aqueous solution, (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°, -1100.8 kJ · mol−1
- ^ ΔfG°, -1012.5 kJ · mol−1
- ^ S°, 145.94 J · K−1 · mol−1
- ^ Cp°, 120.25 J · K−1 · mol−1
- ^ ΔfH°, -1115.87 kJ · mol−1
- ^ ΔfG°, -1010.39 kJ · mol−1
- ^ S°, 87.9 J · K−1 · mol−1
- ^ ΔfH°, -3162.3 kJ · mol−1
- ^ ΔfG°, -2676.1 kJ · mol−1
- ^ S°, 444. J · K−1 · mol−1
- ^ ΔfH°, -1188.7 kJ · mol−1
- ^ ΔfG°, -1092.4 kJ · mol−1
- ^ S°, 134. J · K−1 · mol−1
- ^ ΔfH°, -1182.8 kJ · mol−1
- ^ ΔfG°, -1079.4 kJ · mol−1
- ^ S°, 109. J · K−1 · mol−1
- ^ ΔfH°, -1554.90 kJ · mol−1
- ^ ΔfG°, -1462.80 kJ · mol−1
- ^ S°, 113.85 J · K−1 · mol−1
- ^ ΔfH°, -1540.1 kJ · mol−1
- ^ ΔfH°, -1586.2 kJ · mol−1
- ^ ΔfH°, -3048.5 kJ · mol−1
- ^ ΔfH°, -4228.8 kJ · mol−1
- ^ ΔfH°, -608.81 kJ · mol−1
- ^ ΔfG°, -537.81 kJ · mol−1
- ^ S°, 232.2 J · K−1 · mol−1