C6H12 + 9O2 → 6CO2 + 6H2O
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Complete combustion of yields carbon dioxide and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
General equation
- Complete combustion of hydrocarbon
- HydrocarbonReducing agent + Oxidizing agent ⟶ CO2Oxidation product + H2OReduction product
Oxidation state of each atom
Reactants
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CO2 | Carbon dioxide | 6 | Redoxed product | Carbon dioxide |
| H2O | Water | 6 | Reduced | Water |
Thermodynamic changes
Changes in standard condition
| 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 | −4001.9 | −3872.5 | −439.4 | 226.9 |
| −4001.9 | −3872.5 | −439.4 | 226.9 | |
| −444.66 | −430.28 | −48.82 | 25.21 | |
per 1 mol of | −666.98 | −645.42 | −73.23 | 37.82 |
per 1 mol of | −666.98 | −645.42 | −73.23 | 37.82 |
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 |
|---|---|---|---|---|
| (l) | -74.1[1] | 83.6[1] | 295.1[1] | 183.3[1] |
| (g) | -43.5[1] | 84.45[1] | 384.6[1] | 132.3[1] |
| (g) | 0[2] | 0[2] | 205.138[2] | 29.355[2] |
| (ao) | -11.7[2] | 16.4[2] | 110.9[2] | – |
* (l):Liquid, (g):Gas, (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 |
|---|---|---|---|---|
| CO2 (g) | -393.509[2] | -394.359[2] | 213.74[2] | 37.11[2] |
| CO2 (ao) | -413.80[2] | -385.98[2] | 117.6[2] | – |
| H2O (cr) | – | – | – | – |
| H2O (l) | -285.830[2] | -237.129[2] | 69.91[2] | 75.291[2] |
| H2O (g) | -241.818[2] | -228.572[2] | 188.825[2] | 33.577[2] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (l):Liquid
References
List of references
- 1James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ ΔfH°, -74.1 kJ · mol−1 - p.969
- ^ ΔfG°, 83.6 kJ · mol−1 - p.969
- ^ S°, 295.1 J · K−1 · mol−1 - p.969
- ^ Cp°, 183.3 J · K−1 · mol−1 - p.969
- ^ ΔfH°, -43.5 kJ · mol−1 - p.969
- ^ ΔfG°, 84.45 kJ · mol−1 - p.969
- ^ S°, 384.6 J · K−1 · mol−1 - p.969
- ^ Cp°, 132.3 J · K−1 · mol−1 - p.969
- 2Janiel 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°, 205.138 J · K−1 · mol−1
- ^ Cp°, 29.355 J · K−1 · mol−1
- ^ ΔfH°, -11.7 kJ · mol−1
- ^ ΔfG°, 16.4 kJ · mol−1
- ^ S°, 110.9 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · 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