5FeBr2 + KMnO4 + 18H+ → 5Fe3+ + Mn2+ + 10HBr↑ + K+ + 4H2O
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- Reaction of iron(II) bromide and potassium permanganate under acidic condition
- 5FeBr2Iron(II) bromide + KMnO4Potassium permanganate + 18H+Hydrogen ion5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + 10HBr↑Hydrogen bromide + K+Potassium ion + 4H2OWater⟶
The reaction of iron(II) bromide, potassium permanganate, and hydrogen ion yields iron(III) ion, manganese(II) ion, hydrogen bromide, 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 iron(II) bromide and potassium permanganate under acidic condition
- 5FeBr2Iron(II) bromide + KMnO4Potassium permanganate + 18H+Hydrogen ion5Fe3+Iron(III) ion + Mn2+Manganese(II) ion + 10HBr↑Hydrogen bromide + K+Potassium ion + 4H2OWater⟶
General equation
- Reaction of oxidizable species and oxidizing species under acidic condition
- Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent ⟶ ProductOxidation product + ProductReduction product + H2ONon-redox product
Oxidation state of each atom
- Reaction of iron(II) bromide and potassium permanganate under acidic condition
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
FeBr2 | Iron(II) bromide | 5 | Reducing | Oxidizable |
KMnO4 | Potassium permanganate | 1 | Oxidizing | Oxidizing under acidic condition |
H+ | Hydrogen ion | 18 | – | Hydrogen ion |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Fe3+ | Iron(III) ion | 5 | Oxidized | – |
Mn2+ | Manganese(II) ion | 1 | Reduced | – |
HBr | Hydrogen bromide | 10 | – | – |
K+ | Potassium ion | 1 | – | – |
H2O | Water | 4 | – | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of iron(II) bromide and potassium permanganate under acidic condition◆
ΔrG 146.7 kJ/mol K 0.20 × 10−25 pK 25.70
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 | 231.9 | 146.7 | 286.3 | – |
per 1 mol of | 46.38 | 29.34 | 57.26 | – |
per 1 mol of | 231.9 | 146.7 | 286.3 | – |
per 1 mol of Hydrogen ion | 12.88 | 8.150 | 15.91 | – |
per 1 mol of Iron(III) ion | 46.38 | 29.34 | 57.26 | – |
per 1 mol of Manganese(II) ion | 231.9 | 146.7 | 286.3 | – |
per 1 mol of | 23.19 | 14.67 | 28.63 | – |
per 1 mol of Potassium ion | 231.9 | 146.7 | 286.3 | – |
per 1 mol of | 57.98 | 36.67 | 71.58 | – |
Changes in standard condition (2)
- Reaction of iron(II) bromide and potassium permanganate under acidic condition◆
ΔrG −358.4 kJ/mol K 6.15 × 1062 pK −62.79
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 | −619.7 | −358.4 | −876.7 | – |
per 1 mol of | −123.9 | −71.68 | −175.3 | – |
per 1 mol of | −619.7 | −358.4 | −876.7 | – |
per 1 mol of Hydrogen ion | −34.43 | −19.91 | −48.71 | – |
per 1 mol of Iron(III) ion | −123.9 | −71.68 | −175.3 | – |
per 1 mol of Manganese(II) ion | −619.7 | −358.4 | −876.7 | – |
per 1 mol of | −61.97 | −35.84 | −87.67 | – |
per 1 mol of Potassium ion | −619.7 | −358.4 | −876.7 | – |
per 1 mol of | −154.9 | −89.60 | −219.2 | – |
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 |
---|---|---|---|---|
FeBr2 (cr) | -249.8[1] | -238.1[1] | 140.6[1] | – |
FeBr2 (g) | -46[1] | – | – | – |
FeBr2 (ai) | -332.2[1] | -286.81[1] | 27.2[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 |
---|---|---|---|---|
Fe3+ (g) | 5712.8[1] | – | – | – |
Fe3+ (ao) | -48.5[1] | -4.7[1] | -315.9[1] | – |
Mn2+ (g) | 2519.69[1] | – | – | – |
Mn2+ (ao) | -220.75[1] | -228.1[1] | -73.6[1] | 50[1] |
HBr (g) | -36.40[1] | -53.45[1] | 198.695[1] | 29.142[1] |
HBr (ai) | -121.55[1] | -103.96[1] | 82.4[1] | -141.8[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, (ai):Ionized aqueous solution, (cr):Crystalline solid, (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°, -249.8 kJ · mol−1
- ^ ΔfG°, -238.1 kJ · mol−1
- ^ S°, 140.6 J · K−1 · mol−1
- ^ ΔfH°, -46. kJ · mol−1
- ^ ΔfH°, -332.2 kJ · mol−1
- ^ ΔfG°, -286.81 kJ · mol−1
- ^ S°, 27.2 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°, 5712.8 kJ · mol−1
- ^ ΔfH°, -48.5 kJ · mol−1
- ^ ΔfG°, -4.7 kJ · mol−1
- ^ S°, -315.9 J · K−1 · mol−1
- ^ ΔfH°, 2519.69 kJ · mol−1
- ^ ΔfH°, -220.75 kJ · mol−1
- ^ ΔfG°, -228.1 kJ · mol−1
- ^ S°, -73.6 J · K−1 · mol−1
- ^ Cp°, 50. J · K−1 · mol−1
- ^ ΔfH°, -36.40 kJ · mol−1
- ^ ΔfG°, -53.45 kJ · mol−1
- ^ S°, 198.695 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -121.55 kJ · mol−1
- ^ ΔfG°, -103.96 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, -141.8 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