2NH3 + SO3 + H2O → (NH4)2SO4
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- Reaction of ammonia, sulfur trioxide, and water
The reaction of ammonia, sulfur trioxide, and water yields ammonium sulfate (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 ammonia, sulfur trioxide, and water
General equation
- Reaction of base and acidic oxide
- BaseLewis base + Acidic oxideLewis acid + H2O ⟶ Oxoacid saltLewis conjugate + (H2O)
- Non hydroxide baseBrønsted base + Acidic oxideLewis acid + H2O ⟶ Oxoacid salt
Oxidation state of each atom
- Reaction of ammonia, sulfur trioxide, and water
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NH3 | Ammonia | 2 | Lewis base Brønsted base | Base Non hydroxide base |
SO3 | Sulfur trioxide | 1 | Lewis acid | Acidic oxide |
H2O | Water | 1 | – | Water |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
(NH4)2SO4 | Ammonium sulfate | 1 | Lewis conjugate – | Oxoacid salt |
Thermodynamic changes
Changes in standard condition
- Reaction of ammonia, sulfur trioxide, and water◆
ΔrG −257.89 kJ/mol K 1.51 × 1045 pK −45.18
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 | −361.76 | −257.89 | −348.5 | – |
per 1 mol of | −180.88 | −128.94 | −174.3 | – |
per 1 mol of | −361.76 | −257.89 | −348.5 | – |
per 1 mol of | −361.76 | −257.89 | −348.5 | – |
per 1 mol of | −361.76 | −257.89 | −348.5 | – |
Changes in aqueous solution
- Reaction of ammonia, sulfur trioxide, and water◆
ΔrG −238.80 kJ/mol K 6.85 × 1041 pK −41.84
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 | −273.36 | −238.80 | −116.3 | – |
per 1 mol of | −136.68 | −119.40 | −58.15 | – |
per 1 mol of | −273.36 | −238.80 | −116.3 | – |
per 1 mol of | −273.36 | −238.80 | −116.3 | – |
per 1 mol of | −273.36 | −238.80 | −116.3 | – |
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 |
---|---|---|---|---|
NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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] |
H2O (cr) | – | – | – | – |
H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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 |
---|---|---|---|---|
(NH4)2SO4 (cr) | -1180.85[1] | -901.67[1] | 220.1[1] | 187.49[1] |
(NH4)2SO4 (ai) | -1174.28[1] | -903.14[1] | 246.9[1] | -133.1[1] |
* (cr):Crystalline solid, (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°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 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°, -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
- ^ ΔfH°, -1180.85 kJ · mol−1
- ^ ΔfG°, -901.67 kJ · mol−1
- ^ S°, 220.1 J · K−1 · mol−1
- ^ Cp°, 187.49 J · K−1 · mol−1
- ^ ΔfH°, -1174.28 kJ · mol−1
- ^ ΔfG°, -903.14 kJ · mol−1
- ^ S°, 246.9 J · K−1 · mol−1
- ^ Cp°, -133.1 J · K−1 · mol−1