13RbCl + 4KMnO4 + 17H+ 🔥→ 13Rb+ + 5HClO2 + 4MnCl2 + 4K+ + 6H2O
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- Reaction of rubidium chloride and potassium permanganate under acidic condition
- 13RbClRubidium chloride + 4KMnO4Potassium permanganate + 17H+Hydrogen ion13Rb+Rubidium ion + 5HClO2Chlorous acid + 4MnCl2Manganese(II) chloride + 4K+Potassium ion + 6H2OWater🔥⟶
The reaction of rubidium chloride, potassium permanganate, and hydrogen ion yields rubidium ion, chlorous acid, manganese(II) chloride, potassium ion, 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 rubidium chloride and potassium permanganate under acidic condition
- 13RbClRubidium chloride + 4KMnO4Potassium permanganate + 17H+Hydrogen ion13Rb+Rubidium ion + 5HClO2Chlorous acid + 4MnCl2Manganese(II) chloride + 4K+Potassium ion + 6H2OWater🔥⟶
General equation
- Reaction of hardly oxidizable species and oxidizing species under acidic condition
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of rubidium chloride and potassium permanganate under acidic condition
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
RbCl | Rubidium chloride | 13 | Reducing | Hardly oxidizable |
KMnO4 | Potassium permanganate | 4 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 17 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Rb+ | Rubidium ion | 13 | – | – |
HClO2 | Chlorous acid | 5 | Oxidized | – |
MnCl2 | Manganese(II) chloride | 4 | Reduced | – |
K+ | Potassium ion | 4 | – | – |
H2O | Water | 6 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of rubidium chloride and potassium permanganate under acidic condition◆
ΔrG 138.3 kJ/mol K 0.59 × 10−24 pK 24.23
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 | 144.0 | 138.3 | 17.4 | – |
per 1 mol of | 11.08 | 10.64 | 1.34 | – |
per 1 mol of | 36.00 | 34.58 | 4.35 | – |
per 1 mol of Hydrogen ion | 8.471 | 8.135 | 1.02 | – |
per 1 mol of Rubidium ion | 11.08 | 10.64 | 1.34 | – |
per 1 mol of | 28.80 | 27.66 | 3.48 | – |
per 1 mol of | 36.00 | 34.58 | 4.35 | – |
per 1 mol of Potassium ion | 36.00 | 34.58 | 4.35 | – |
per 1 mol of | 24.00 | 23.05 | 2.90 | – |
Changes in standard condition (2)
- Reaction of rubidium chloride and potassium permanganate under acidic condition◆
ΔrG 133.5 kJ/mol K 0.41 × 10−23 pK 23.39
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 | – | 133.5 | – | – |
per 1 mol of | – | 10.27 | – | – |
per 1 mol of | – | 33.38 | – | – |
per 1 mol of Hydrogen ion | – | 7.853 | – | – |
per 1 mol of Rubidium ion | – | 10.27 | – | – |
per 1 mol of | – | 26.70 | – | – |
per 1 mol of | – | 33.38 | – | – |
per 1 mol of Potassium ion | – | 33.38 | – | – |
per 1 mol of | – | 22.25 | – | – |
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 |
---|---|---|---|---|
RbCl (cr) | -435.35[1] | -407.80[1] | 95.90[1] | 52.38[1] |
RbCl (g) | -228.9[1] | -247.3[1] | 249.56[1] | 36.82[1] |
RbCl (ai) | -418.32[1] | -415.20[1] | 177.99[1] | – |
KMnO4 (cr) | -837.2[1] | -737.6[1] | 171.71[1] | 117.57[1] |
KMnO4 (ai) | -793.8[1] | -730.5[1] | 293.7[1] | -60.2[1] |
H+ (g) | 1536.202[1] | – | – | – |
H+ (ao) | 0[1] | 0[1] | 0[1] | 0[1] |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-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 |
---|---|---|---|---|
Rb+ (g) | 490.101[1] | – | – | – |
Rb+ (ao) | -251.17[1] | -283.98[1] | 121.50[1] | – |
HClO2 (ao) | -51.9[1] | 5.9[1] | 188.3[1] | – |
MnCl2 (cr) | -481.29[1] | -440.50[1] | 118.24[1] | 72.93[1] |
MnCl2 (g) | -263.6[1] | – | – | – |
MnCl2 (ai) | -555.05[1] | -490.8[1] | 38.9[1] | -222[1] |
MnCl2 (ao) | – | -492.0[1] | – | – |
MnCl2 (cr) 1 hydrate | -789.9[1] | -696.1[1] | 174.1[1] | – |
MnCl2 (cr) 2 hydrate | -1092.0[1] | -942.1[1] | 218.8[1] | – |
MnCl2 (cr) 4 hydrate | -1687.4[1] | -1423.6[1] | 303.3[1] | – |
K+ (g) | 514.26[1] | – | – | – |
K+ (ao) | -252.38[1] | -283.27[1] | 102.5[1] | 21.8[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] |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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°, -435.35 kJ · mol−1
- ^ ΔfG°, -407.80 kJ · mol−1
- ^ S°, 95.90 J · K−1 · mol−1
- ^ Cp°, 52.38 J · K−1 · mol−1
- ^ ΔfH°, -228.9 kJ · mol−1
- ^ ΔfG°, -247.3 kJ · mol−1
- ^ S°, 249.56 J · K−1 · mol−1
- ^ Cp°, 36.82 J · K−1 · mol−1
- ^ ΔfH°, -418.32 kJ · mol−1
- ^ ΔfG°, -415.20 kJ · mol−1
- ^ S°, 177.99 J · K−1 · mol−1
- ^ ΔfH°, -837.2 kJ · mol−1
- ^ ΔfG°, -737.6 kJ · mol−1
- ^ S°, 171.71 J · K−1 · mol−1
- ^ Cp°, 117.57 J · K−1 · mol−1
- ^ ΔfH°, -793.8 kJ · mol−1
- ^ ΔfG°, -730.5 kJ · mol−1
- ^ S°, 293.7 J · K−1 · mol−1
- ^ Cp°, -60.2 J · K−1 · mol−1
- ^ ΔfH°, 1536.202 kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 0 J · K−1 · mol−1
- ^ Cp°, 0 J · K−1 · mol−1
- ^ ΔfH°, 490.101 kJ · mol−1
- ^ ΔfH°, -251.17 kJ · mol−1
- ^ ΔfG°, -283.98 kJ · mol−1
- ^ S°, 121.50 J · K−1 · mol−1
- ^ ΔfH°, -51.9 kJ · mol−1
- ^ ΔfG°, 5.9 kJ · mol−1
- ^ S°, 188.3 J · K−1 · mol−1
- ^ ΔfH°, -481.29 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 118.24 J · K−1 · mol−1
- ^ Cp°, 72.93 J · K−1 · mol−1
- ^ ΔfH°, -263.6 kJ · mol−1
- ^ ΔfH°, -555.05 kJ · mol−1
- ^ ΔfG°, -490.8 kJ · mol−1
- ^ S°, 38.9 J · K−1 · mol−1
- ^ Cp°, -222. J · K−1 · mol−1
- ^ ΔfG°, -492.0 kJ · mol−1
- ^ ΔfH°, -789.9 kJ · mol−1
- ^ ΔfG°, -696.1 kJ · mol−1
- ^ S°, 174.1 J · K−1 · mol−1
- ^ ΔfH°, -1092.0 kJ · mol−1
- ^ ΔfG°, -942.1 kJ · mol−1
- ^ S°, 218.8 J · K−1 · mol−1
- ^ ΔfH°, -1687.4 kJ · mol−1
- ^ ΔfG°, -1423.6 kJ · mol−1
- ^ S°, 303.3 J · K−1 · mol−1
- ^ ΔfH°, 514.26 kJ · mol−1
- ^ ΔfH°, -252.38 kJ · mol−1
- ^ ΔfG°, -283.27 kJ · mol−1
- ^ S°, 102.5 J · K−1 · mol−1
- ^ Cp°, 21.8 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