2H2 + 3SiO2 🔥→ Si + 2H2SiO3
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- Reaction of and silicon dioxide
The reaction of and silicon dioxide yields and metasilicic acid (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 and silicon dioxide
General equation
- Reaction of reducing species and reducible species
- Reducing speciesReducing agent + Reducible speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of and silicon dioxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
2 | Reducing | Reducing | ||
SiO2 | Silicon dioxide | 3 | Oxidizing | Reducible |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
1 | Reduced | – | ||
H2SiO3 | Metasilicic acid | 2 | Oxidized | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and silicon dioxide◆
ΔrG 385.1 kJ/mol K 0.34 × 10−67 pK 67.47
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 | 355.4 | 385.1 | −100 | – |
177.7 | 192.6 | −50.0 | – | |
per 1 mol of | 118.5 | 128.4 | −33.3 | – |
355.4 | 385.1 | −100 | – | |
per 1 mol of | 177.7 | 192.6 | −50.0 | – |
Changes in standard condition (2)
- Reaction of and silicon dioxide
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 | 359.6 | – | – | – |
179.8 | – | – | – | |
per 1 mol of | 119.9 | – | – | – |
359.6 | – | – | – | |
per 1 mol of | 179.8 | – | – | – |
Changes in standard condition (3)
- Reaction of and silicon dioxide◆
ΔrG 381.5 kJ/mol K 0.15 × 10−66 pK 66.84
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 | 351.0 | 381.5 | −103 | – |
175.5 | 190.8 | −51.5 | – | |
per 1 mol of | 117.0 | 127.2 | −34.3 | – |
351.0 | 381.5 | −103 | – | |
per 1 mol of | 175.5 | 190.8 | −51.5 | – |
Changes in standard condition (4)
- Reaction of and silicon dioxide
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 | 355.2 | – | – | – |
177.6 | – | – | – | |
per 1 mol of | 118.4 | – | – | – |
355.2 | – | – | – | |
per 1 mol of | 177.6 | – | – | – |
Changes in standard condition (5)
- Reaction of and silicon dioxide◆
ΔrG 381.0 kJ/mol K 0.18 × 10−66 pK 66.75
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 | 349.8 | 381.0 | −105 | – |
174.9 | 190.5 | −52.5 | – | |
per 1 mol of | 116.6 | 127.0 | −35.0 | – |
349.8 | 381.0 | −105 | – | |
per 1 mol of | 174.9 | 190.5 | −52.5 | – |
Changes in standard condition (6)
- Reaction of and silicon dioxide
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 | 354.0 | – | – | – |
177.0 | – | – | – | |
per 1 mol of | 118.0 | – | – | – |
354.0 | – | – | – | |
per 1 mol of | 177.0 | – | – | – |
Changes in standard condition (7)
- Reaction of and silicon dioxide◆
ΔrG 367.3 kJ/mol K 0.45 × 10−64 pK 64.35
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 | 333.1 | 367.3 | −115 | – |
166.6 | 183.7 | −57.5 | – | |
per 1 mol of | 111.0 | 122.4 | −38.3 | – |
333.1 | 367.3 | −115 | – | |
per 1 mol of | 166.6 | 183.7 | −57.5 | – |
Changes in standard condition (8)
- Reaction of and silicon dioxide
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 | 337.3 | – | – | – |
168.7 | – | – | – | |
per 1 mol of | 112.4 | – | – | – |
337.3 | – | – | – | |
per 1 mol of | 168.7 | – | – | – |
Changes in aqueous solution
- Reaction of and silicon dioxide
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 | 333.8 | – | – | – |
166.9 | – | – | – | |
per 1 mol of | 111.3 | – | – | – |
333.8 | – | – | – | |
per 1 mol of | 166.9 | – | – | – |
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 |
---|---|---|---|---|
(g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
(ao) | -4.2[1] | 17.6[1] | 577[1] | – |
SiO2 (cr) α-quartz | -910.94[1] | -856.64[1] | 41.84[1] | 44.43[1] |
SiO2 (cr) α-cristobalite | -909.48[1] | -855.43[1] | 42.68[1] | 44.18[1] |
SiO2 (cr) α-tridymite | -909.06[1] | -855.26[1] | 43.5[1] | 44.60[1] |
SiO2 (am) | -903.49[1] | -850.70[1] | 46.9[1] | 44.4[1] |
SiO2 (g) | -322[1] | – | – | – |
SiO2 (ao) | -897.0[1] | – | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (am):Amorphous solid
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 |
---|---|---|---|---|
(cr) | 0[1] | 0[1] | 18.83[1] | 20.00[1] |
(am) | 4.2[1] | – | – | – |
(g) | 455.6[1] | 411.3[1] | 167.97[1] | 22.251[1] |
H2SiO3 (cr) | -1188.7[1] | -1092.4[1] | 134[1] | – |
H2SiO3 (ao) | -1182.8[1] | -1079.4[1] | 109[1] | – |
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1
- ^ ΔfH°, -910.94 kJ · mol−1
- ^ ΔfG°, -856.64 kJ · mol−1
- ^ S°, 41.84 J · K−1 · mol−1
- ^ Cp°, 44.43 J · K−1 · mol−1
- ^ ΔfH°, -909.48 kJ · mol−1
- ^ ΔfG°, -855.43 kJ · mol−1
- ^ S°, 42.68 J · K−1 · mol−1
- ^ Cp°, 44.18 J · K−1 · mol−1
- ^ ΔfH°, -909.06 kJ · mol−1
- ^ ΔfG°, -855.26 kJ · mol−1
- ^ S°, 43.5 J · K−1 · mol−1
- ^ Cp°, 44.60 J · K−1 · mol−1
- ^ ΔfH°, -903.49 kJ · mol−1
- ^ ΔfG°, -850.70 kJ · mol−1
- ^ S°, 46.9 J · K−1 · mol−1
- ^ Cp°, 44.4 J · K−1 · mol−1
- ^ ΔfH°, -322. kJ · mol−1
- ^ ΔfH°, -897.0 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 18.83 J · K−1 · mol−1
- ^ Cp°, 20.00 J · K−1 · mol−1
- ^ ΔfH°, 4.2 kJ · mol−1
- ^ ΔfH°, 455.6 kJ · mol−1
- ^ ΔfG°, 411.3 kJ · mol−1
- ^ S°, 167.97 J · K−1 · mol−1
- ^ Cp°, 22.251 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