Na2O + 2HClO4 → 2NaClO4 + H2O
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- Reaction of sodium oxide and perchloric acid
The reaction of sodium oxide and perchloric acid yields sodium perchlorate and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of sodium oxide and perchloric acid
General equation
- Reaction of basic oxide and acid
- Basic oxideBrønsted base + AcidBrønsted acid ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of strongly basic oxide and strong acid
- Strongly basic oxideBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acid and strong baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of sodium oxide and perchloric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2O | Sodium oxide | 1 | Brønsted base | Basic oxide Strongly basic oxide |
| HClO4 | Perchloric acid | 2 | Brønsted acid | Acid Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaClO4 | Sodium perchlorate | 2 | Conjugate base | Salt Salt of strong acid and strong base |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium oxide and perchloric acid
| 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 | −557.05 | – | – | – |
per 1 mol of | −557.05 | – | – | – |
per 1 mol of | −278.52 | – | – | – |
per 1 mol of | −278.52 | – | – | – |
per 1 mol of | −557.05 | – | – | – |
Changes in aqueous solution
- Reaction of sodium oxide and perchloric acid◆
ΔrG −385.45 kJ/mol K 3.37 × 1067 pK −67.53
| 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 | −351.85 | −385.45 | 112.9 | – |
per 1 mol of | −351.85 | −385.45 | 112.9 | – |
per 1 mol of | −175.93 | −192.72 | 56.45 | – |
per 1 mol of | −175.93 | −192.72 | 56.45 | – |
per 1 mol of | −351.85 | −385.45 | 112.9 | – |
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 |
|---|---|---|---|---|
| Na2O (cr) | -414.22[1] | -375.46[1] | 75.06[1] | 69.12[1] |
| Na2O (g) | -35.6[1] | -52.3[1] | 261.2[1] | 55.2[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, (g):Gas, (l):Liquid, (ai):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 |
|---|---|---|---|---|
| NaClO4 (cr) | -383.30[1] | -254.85[1] | 142.3[1] | – |
| NaClO4 (ai) | -369.45[1] | -270.41[1] | 241.0[1] | – |
| NaClO4 (cr) 1 hydrate | -677.77[1] | -494.29[1] | 190.8[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, (l):Liquid, (g):Gas
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°, -414.22 kJ · mol−1
- ^ ΔfG°, -375.46 kJ · mol−1
- ^ S°, 75.06 J · K−1 · mol−1
- ^ Cp°, 69.12 J · K−1 · mol−1
- ^ ΔfH°, -35.6 kJ · mol−1
- ^ ΔfG°, -52.3 kJ · mol−1
- ^ S°, 261.2 J · K−1 · mol−1
- ^ Cp°, 55.2 J · K−1 · 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°, -383.30 kJ · mol−1
- ^ ΔfG°, -254.85 kJ · mol−1
- ^ S°, 142.3 J · K−1 · mol−1
- ^ ΔfH°, -369.45 kJ · mol−1
- ^ ΔfG°, -270.41 kJ · mol−1
- ^ S°, 241.0 J · K−1 · mol−1
- ^ ΔfH°, -677.77 kJ · mol−1
- ^ ΔfG°, -494.29 kJ · mol−1
- ^ S°, 190.8 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