Sn + 2SO3 → SnO2 + 2SO2↑
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- Reaction of and sulfur trioxide
The reaction of and sulfur trioxide yields tin(IV) oxide and sulfur dioxide (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 sulfur trioxide
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 sulfur trioxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing | ||
| SO3 | Sulfur trioxide | 2 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| SnO2 | Tin(IV) oxide | 1 | Oxidized | – |
| SO2 | Sulfur dioxide | 2 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of and sulfur trioxide◆
ΔrG −372.5 kJ/mol K 1.82 × 1065 pK −65.26
| 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 | −292.3 | −372.5 | 269.6 | – |
| −292.3 | −372.5 | 269.6 | – | |
per 1 mol of | −146.2 | −186.3 | 134.8 | – |
per 1 mol of | −292.3 | −372.5 | 269.6 | – |
per 1 mol of | −146.2 | −186.3 | 134.8 | – |
Changes in standard condition (2)
- Reaction of and sulfur trioxide◆
ΔrG −372.6 kJ/mol K 1.89 × 1065 pK −65.28
| 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 | −290.2 | −372.6 | 277.0 | – |
| −290.2 | −372.6 | 277.0 | – | |
per 1 mol of | −145.1 | −186.3 | 138.5 | – |
per 1 mol of | −290.2 | −372.6 | 277.0 | – |
per 1 mol of | −145.1 | −186.3 | 138.5 | – |
Changes in aqueous solution (1)
- Reaction of and sulfur trioxide◆
ΔrG −371.6 kJ/mol K 1.26 × 1065 pK −65.10
| 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 | −265.3 | −371.6 | 355.8 | – |
| −265.3 | −371.6 | 355.8 | – | |
per 1 mol of | −132.7 | −185.8 | 177.9 | – |
per 1 mol of | −265.3 | −371.6 | 355.8 | – |
per 1 mol of | −132.7 | −185.8 | 177.9 | – |
Changes in aqueous solution (2)
- Reaction of and sulfur trioxide◆
ΔrG −372.5 kJ/mol K 1.82 × 1065 pK −65.26
| 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 | −317.6 | −372.5 | 183.2 | – |
| −317.6 | −372.5 | 183.2 | – | |
per 1 mol of | −158.8 | −186.3 | 91.60 | – |
per 1 mol of | −317.6 | −372.5 | 183.2 | – |
per 1 mol of | −158.8 | −186.3 | 91.60 | – |
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 |
|---|---|---|---|---|
| (cr) white | 0[1] | 0[1] | 51.55[1] | 26.99[1] |
| (cr) gray | -2.09[1] | 0.13[1] | 44.14[1] | 25.77[1] |
| (g) | 302.1[1] | 267.3[1] | 168.486[1] | 21.259[1] |
| SO3 (cr) β | -454.51[1] | -374.21[1] | 70.7[1] | – |
| SO3 (l) | -441.04[1] | -373.75[1] | 113.8[1] | – |
| SO3 (g) | -395.72[1] | -371.06[1] | 256.76[1] | 50.67[1] |
* (cr):Crystalline solid, (g):Gas, (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 |
|---|---|---|---|---|
| SnO2 (cr) | -580.7[1] | -519.6[1] | 52.3[1] | 52.59[1] |
| SO2 (l) | -320.5[1] | – | – | – |
| SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
| SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[1] | – |
* (cr):Crystalline solid, (l):Liquid, (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°, 51.55 J · K−1 · mol−1
- ^ Cp°, 26.99 J · K−1 · mol−1
- ^ ΔfH°, -2.09 kJ · mol−1
- ^ ΔfG°, 0.13 kJ · mol−1
- ^ S°, 44.14 J · K−1 · mol−1
- ^ Cp°, 25.77 J · K−1 · mol−1
- ^ ΔfH°, 302.1 kJ · mol−1
- ^ ΔfG°, 267.3 kJ · mol−1
- ^ S°, 168.486 J · K−1 · mol−1
- ^ Cp°, 21.259 J · K−1 · mol−1
- ^ ΔfH°, -454.51 kJ · mol−1
- ^ ΔfG°, -374.21 kJ · mol−1
- ^ S°, 70.7 J · K−1 · mol−1
- ^ ΔfH°, -441.04 kJ · mol−1
- ^ ΔfG°, -373.75 kJ · mol−1
- ^ S°, 113.8 J · K−1 · mol−1
- ^ ΔfH°, -395.72 kJ · mol−1
- ^ ΔfG°, -371.06 kJ · mol−1
- ^ S°, 256.76 J · K−1 · mol−1
- ^ Cp°, 50.67 J · K−1 · mol−1
- ^ ΔfH°, -580.7 kJ · mol−1
- ^ ΔfG°, -519.6 kJ · mol−1
- ^ S°, 52.3 J · K−1 · mol−1
- ^ Cp°, 52.59 J · K−1 · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 J · K−1 · mol−1