Cs2S + 2HClO4 → 2CsClO4 + H2S↑
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The reaction of caesium sulfide and perchloric acid yields caesium perchlorate and hydrogen sulfide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of caesium sulfide 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 caesium sulfide and perchloric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Cs2S | Caesium sulfide | 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 |
|---|---|---|---|---|
| CsClO4 | Caesium perchlorate | 2 | Conjugate base | Salt of strong acid Salt of non volatile acid |
| H2S | Hydrogen sulfide | 1 | Conjugate acid | Weak acid Volatile acid |
Thermodynamic changes
Changes in standard condition
- Reaction of caesium sulfide 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 | −465.9 | – | – | – |
per 1 mol of | −465.9 | – | – | – |
per 1 mol of | −232.9 | – | – | – |
per 1 mol of | −232.9 | – | – | – |
per 1 mol of | −465.9 | – | – | – |
Changes in aqueous solution (1)
- Reaction of caesium sulfide and perchloric acid◆
ΔrG −119.3 kJ/mol K 7.95 × 1020 pK −20.90
| 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 | −53.5 | −119.3 | 220.5 | – |
per 1 mol of | −53.5 | −119.3 | 220.5 | – |
per 1 mol of | −26.8 | −59.65 | 110.3 | – |
per 1 mol of | −26.8 | −59.65 | 110.3 | – |
per 1 mol of | −53.5 | −119.3 | 220.5 | – |
Changes in aqueous solution (2)
- Reaction of caesium sulfide and perchloric acid◆
ΔrG −113.6 kJ/mol K 7.98 × 1019 pK −19.90
| 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 | −72.6 | −113.6 | 136 | – |
per 1 mol of | −72.6 | −113.6 | 136 | – |
per 1 mol of | −36.3 | −56.80 | 68.0 | – |
per 1 mol of | −36.3 | −56.80 | 68.0 | – |
per 1 mol of | −72.6 | −113.6 | 136 | – |
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 |
|---|---|---|---|---|
| Cs2S (cr) | -359.8[1] | – | – | – |
| Cs2S (ai) | -483.7[1] | -498.3[1] | 251.5[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 |
|---|---|---|---|---|
| CsClO4 (cr) | -443.09[1] | -314.26[1] | 175.06[1] | 108.28[1] |
| CsClO4 (ai) | -387.61[1] | -300.54[1] | 315.1[1] | – |
| H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
| H2S (ao) | -39.7[1] | -27.83[1] | 121[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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°, -359.8 kJ · mol−1
- ^ ΔfH°, -483.7 kJ · mol−1
- ^ ΔfG°, -498.3 kJ · mol−1
- ^ S°, 251.5 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°, -443.09 kJ · mol−1
- ^ ΔfG°, -314.26 kJ · mol−1
- ^ S°, 175.06 J · K−1 · mol−1
- ^ Cp°, 108.28 J · K−1 · mol−1
- ^ ΔfH°, -387.61 kJ · mol−1
- ^ ΔfG°, -300.54 kJ · mol−1
- ^ S°, 315.1 J · K−1 · mol−1
- ^ ΔfH°, -20.63 kJ · mol−1
- ^ ΔfG°, -33.56 kJ · mol−1
- ^ S°, 205.79 J · K−1 · mol−1
- ^ Cp°, 34.23 J · K−1 · mol−1
- ^ ΔfH°, -39.7 kJ · mol−1
- ^ ΔfG°, -27.83 kJ · mol−1
- ^ S°, 121. J · K−1 · mol−1