Rb2CO3 + 2HClO4 → 2RbClO4 + H2CO3
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The reaction of rubidium carbonate and perchloric acid yields rubidium perchlorate and carbonic acid (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 rubidium carbonate and perchloric acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of rubidium carbonate and perchloric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Rb2CO3 | Rubidium carbonate | 1 | Brønsted base | Salt of weak acid Salt of volatile acid |
| HClO4 | Perchloric acid | 2 | Brønsted acid | Strong acid Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| RbClO4 | Rubidium perchlorate | 2 | Conjugate base | Salt of strong acid Salt of non volatile acid |
| H2CO3 | Carbonic acid | 1 | Conjugate acid | Weak acid Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of rubidium carbonate and perchloric acid◆
ΔrG −95.28 kJ/mol K 4.92 × 1016 pK −16.69
| 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 | −22.50 | −95.28 | 243.8 | – |
per 1 mol of | −22.50 | −95.28 | 243.8 | – |
per 1 mol of | −11.25 | −47.64 | 121.9 | – |
per 1 mol of | −11.25 | −47.64 | 121.9 | – |
per 1 mol of | −22.50 | −95.28 | 243.8 | – |
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 |
|---|---|---|---|---|
| Rb2CO3 (cr) | -1136.0[1] | -1051.0[1] | 181.33[1] | 117.61[1] |
| Rb2CO3 (ai) | -1179.47[1] | -1095.78[1] | 186.2[1] | – |
| Rb2CO3 (cr) 1 hydrate | -1448.5[1] | – | – | – |
| Rb2CO3 (cr) 1.5 hydrate | -1604.5[1] | – | – | – |
| Rb2CO3 (cr) 3 hydrate | -2048.1[1] | – | – | – |
| HClO4 (l) | -40.58[1] | – | – | – |
| HClO4 (ai) | -129.33[1] | -8.52[1] | 182.0[1] | – |
| HClO4 (cr) 1 hydrate | -382.21[1] | – | – | – |
| HClO4 (l) 2 hydrate | -677.98[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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 |
|---|---|---|---|---|
| RbClO4 (cr) | -437.23[1] | -306.90[1] | 161.1[1] | – |
| RbClO4 (ai) | -380.49[1] | -292.51[1] | 303.3[1] | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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°, -1136.0 kJ · mol−1
- ^ ΔfG°, -1051.0 kJ · mol−1
- ^ S°, 181.33 J · K−1 · mol−1
- ^ Cp°, 117.61 J · K−1 · mol−1
- ^ ΔfH°, -1179.47 kJ · mol−1
- ^ ΔfG°, -1095.78 kJ · mol−1
- ^ S°, 186.2 J · K−1 · mol−1
- ^ ΔfH°, -1448.5 kJ · mol−1
- ^ ΔfH°, -1604.5 kJ · mol−1
- ^ ΔfH°, -2048.1 kJ · mol−1
- ^ ΔfH°, -40.58 kJ · mol−1
- ^ ΔfH°, -129.33 kJ · mol−1
- ^ ΔfG°, -8.52 kJ · mol−1
- ^ S°, 182.0 J · K−1 · mol−1
- ^ ΔfH°, -382.21 kJ · mol−1
- ^ ΔfH°, -677.98 kJ · mol−1
- ^ ΔfH°, -437.23 kJ · mol−1
- ^ ΔfG°, -306.90 kJ · mol−1
- ^ S°, 161.1 J · K−1 · mol−1
- ^ ΔfH°, -380.49 kJ · mol−1
- ^ ΔfG°, -292.51 kJ · mol−1
- ^ S°, 303.3 J · K−1 · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1