NH4NO3 + RbOH → RbNO3 + NH3↑ + H2O
Last updated:
The reaction of ammonium nitrate and rubidium hydroxide yields rubidium nitrate, ammonia, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium nitrate and rubidium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
- Reaction of volatile acid and non volatile base
- Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base ⟶ Salt of non volatile baseConjugate acid + Volatile baseConjugate base + (H2O)
Oxidation state of each atom
- Reaction of ammonium nitrate and rubidium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NH4NO3 | Ammonium nitrate | 1 | Brønsted acid | Salt of weak base Salt of volatile base |
| RbOH | Rubidium hydroxide | 1 | Brønsted base | Strong base Nonvolatile base |
Products
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium nitrate and rubidium hydroxide
| 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 | −43.24 | – | – | – |
per 1 mol of | −43.24 | – | – | – |
per 1 mol of | −43.24 | – | – | – |
per 1 mol of | −43.24 | – | – | – |
per 1 mol of | −43.24 | – | – | – |
per 1 mol of | −43.24 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium nitrate and rubidium hydroxide◆
ΔrG −17.05 kJ/mol K 9.71 × 102 pK −2.99
| 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 | 30.57 | −17.05 | 159.6 | – |
per 1 mol of | 30.57 | −17.05 | 159.6 | – |
per 1 mol of | 30.57 | −17.05 | 159.6 | – |
per 1 mol of | 30.57 | −17.05 | 159.6 | – |
per 1 mol of | 30.57 | −17.05 | 159.6 | – |
per 1 mol of | 30.57 | −17.05 | 159.6 | – |
Changes in aqueous solution (2)
- Reaction of ammonium nitrate and rubidium hydroxide◆
ΔrG −27.10 kJ/mol K 5.59 × 104 pK −4.75
| 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 | −3.61 | −27.10 | 78.5 | – |
per 1 mol of | −3.61 | −27.10 | 78.5 | – |
per 1 mol of | −3.61 | −27.10 | 78.5 | – |
per 1 mol of | −3.61 | −27.10 | 78.5 | – |
per 1 mol of | −3.61 | −27.10 | 78.5 | – |
per 1 mol of | −3.61 | −27.10 | 78.5 | – |
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 |
|---|---|---|---|---|
| NH4NO3 (cr) | -365.56[1] | -183.87[1] | 151.08[1] | 139.3[1] |
| NH4NO3 (ai) | -339.87[1] | -190.56[1] | 259.8[1] | -6.7[1] |
| RbOH (cr) | -418.19[1] | – | – | – |
| RbOH (g) | -238[1] | – | – | – |
| RbOH (ai) | -481.16[1] | -441.21[1] | 110.75[1] | – |
| RbOH (cr) 1 hydrate | -748.85[1] | – | – | – |
| RbOH (cr) 2 hydrate | -1053.24[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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 |
|---|---|---|---|---|
| RbNO3 (cr) | -495.05[1] | -395.78[1] | 147.3[1] | 102.1[1] |
| RbNO3 (ai) | -458.52[1] | -395.24[1] | 267.8[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] | – |
| 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] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -365.56 kJ · mol−1
- ^ ΔfG°, -183.87 kJ · mol−1
- ^ S°, 151.08 J · K−1 · mol−1
- ^ Cp°, 139.3 J · K−1 · mol−1
- ^ ΔfH°, -339.87 kJ · mol−1
- ^ ΔfG°, -190.56 kJ · mol−1
- ^ S°, 259.8 J · K−1 · mol−1
- ^ Cp°, -6.7 J · K−1 · mol−1
- ^ ΔfH°, -418.19 kJ · mol−1
- ^ ΔfH°, -238. kJ · mol−1
- ^ ΔfH°, -481.16 kJ · mol−1
- ^ ΔfG°, -441.21 kJ · mol−1
- ^ S°, 110.75 J · K−1 · mol−1
- ^ ΔfH°, -748.85 kJ · mol−1
- ^ ΔfH°, -1053.24 kJ · mol−1
- ^ ΔfH°, -495.05 kJ · mol−1
- ^ ΔfG°, -395.78 kJ · mol−1
- ^ S°, 147.3 J · K−1 · mol−1
- ^ Cp°, 102.1 J · K−1 · mol−1
- ^ ΔfH°, -458.52 kJ · mol−1
- ^ ΔfG°, -395.24 kJ · mol−1
- ^ S°, 267.8 J · K−1 · mol−1
- ^ 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°, -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