5H2S + 10RbNO3 → 5Rb2SO4 + 4N2 + 2HNO3 + 4H2O
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- Reaction of hydrogen sulfide and rubidium nitrate
The reaction of hydrogen sulfide and rubidium nitrate yields rubidium sulfate, , nitric acid, and water (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of hydrogen sulfide and rubidium nitrate
General equation
- Reaction of reducing species and oxidizing species
- Reducing speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of hydrogen sulfide and rubidium nitrate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
H2S | Hydrogen sulfide | 5 | Reducing | Reducing |
RbNO3 | Rubidium nitrate | 10 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Rb2SO4 | Rubidium sulfate | 5 | Oxidized | – |
4 | Reduced | – | ||
HNO3 | Nitric acid | 2 | – | – |
H2O | Water | 4 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of hydrogen sulfide and rubidium nitrate◆
ΔrG −3568.79 kJ/mol K 1.68 × 10625 pK −625.22
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 | −3615.92 | −3568.79 | −157.5 | 115.6 |
per 1 mol of | −723.184 | −713.758 | −31.50 | 23.12 |
per 1 mol of | −361.592 | −356.879 | −15.75 | 11.56 |
per 1 mol of | −723.184 | −713.758 | −31.50 | 23.12 |
−903.980 | −892.197 | −39.38 | 28.90 | |
per 1 mol of | −1807.96 | −1784.39 | −78.75 | 57.80 |
per 1 mol of | −903.980 | −892.197 | −39.38 | 28.90 |
Changes in aqueous solution
- Reaction of hydrogen sulfide and rubidium nitrate◆
ΔrG −3641.97 kJ/mol K 1.11 × 10638 pK −638.05
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 | −3832.3 | −3641.97 | −628 | – |
per 1 mol of | −766.46 | −728.394 | −126 | – |
per 1 mol of | −383.23 | −364.197 | −62.8 | – |
per 1 mol of | −766.46 | −728.394 | −126 | – |
−958.08 | −910.492 | −157 | – | |
per 1 mol of | −1916.2 | −1820.98 | −314 | – |
per 1 mol of | −958.08 | −910.492 | −157 | – |
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 |
---|---|---|---|---|
H2S (g) | -20.63[1] | -33.56[1] | 205.79[1] | 34.23[1] |
H2S (ao) | -39.7[1] | -27.83[1] | 121[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] | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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 |
---|---|---|---|---|
Rb2SO4 (cr) | -1435.61[1] | -1316.89[1] | 197.44[1] | 134.06[1] |
Rb2SO4 (g) | -1068.6[1] | – | – | – |
Rb2SO4 (ai) | -1411.60[1] | -1312.50[1] | 263.2[1] | – |
(g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[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, (g):Gas, (ai):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°, -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
- ^ 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°, -1435.61 kJ · mol−1
- ^ ΔfG°, -1316.89 kJ · mol−1
- ^ S°, 197.44 J · K−1 · mol−1
- ^ Cp°, 134.06 J · K−1 · mol−1
- ^ ΔfH°, -1068.6 kJ · mol−1
- ^ ΔfH°, -1411.60 kJ · mol−1
- ^ ΔfG°, -1312.50 kJ · mol−1
- ^ S°, 263.2 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 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