4NiS + 2KMnO4 → 4NiO + 3S + 2MnO2 + K2S
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The reaction of nickel(II) sulfide and potassium permanganate yields nickel(II) oxide, , manganese(IV) oxide, and potassium sulfide (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 nickel(II) sulfide and potassium permanganate
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 nickel(II) sulfide and potassium permanganate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NiS | Nickel(II) sulfide | 4 | Reducing | Reducing |
KMnO4 | Potassium permanganate | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NiO | Nickel(II) oxide | 4 | – | – |
3 | Oxidized | – | ||
MnO2 | Manganese(IV) oxide | 2 | Reduced | – |
K2S | Potassium sulfide | 1 | – | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of nickel(II) sulfide and potassium permanganate◆
ΔrG −347.9 kJ/mol K 8.90 × 1060 pK −60.95
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 | −377.2 | −347.9 | −97 | – |
per 1 mol of | −94.30 | −86.97 | −24 | – |
per 1 mol of | −188.6 | −173.9 | −49 | – |
per 1 mol of | −94.30 | −86.97 | −24 | – |
−125.7 | −116.0 | −32 | – | |
per 1 mol of | −188.6 | −173.9 | −49 | – |
per 1 mol of | −377.2 | −347.9 | −97 | – |
Changes in standard condition (2)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −342.1 | – | – | – |
per 1 mol of | −85.53 | – | – | – |
per 1 mol of | −171.1 | – | – | – |
per 1 mol of | −85.53 | – | – | – |
−114.0 | – | – | – | |
per 1 mol of | −171.1 | – | – | – |
per 1 mol of | −342.1 | – | – | – |
Changes in standard condition (3)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −376.2 | – | – | – |
per 1 mol of | −94.05 | – | – | – |
per 1 mol of | −188.1 | – | – | – |
per 1 mol of | −94.05 | – | – | – |
−125.4 | – | – | – | |
per 1 mol of | −188.1 | – | – | – |
per 1 mol of | −376.2 | – | – | – |
Changes in standard condition (4)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −341.1 | – | – | – |
per 1 mol of | −85.28 | – | – | – |
per 1 mol of | −170.6 | – | – | – |
per 1 mol of | −85.28 | – | – | – |
−113.7 | – | – | – | |
per 1 mol of | −170.6 | – | – | – |
per 1 mol of | −341.1 | – | – | – |
Changes in standard condition (5)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −395.6 | – | – | – |
per 1 mol of | −98.90 | – | – | – |
per 1 mol of | −197.8 | – | – | – |
per 1 mol of | −98.90 | – | – | – |
−131.9 | – | – | – | |
per 1 mol of | −197.8 | – | – | – |
per 1 mol of | −395.6 | – | – | – |
Changes in standard condition (6)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −360.5 | – | – | – |
per 1 mol of | −90.13 | – | – | – |
per 1 mol of | −180.3 | – | – | – |
per 1 mol of | −90.13 | – | – | – |
−120.2 | – | – | – | |
per 1 mol of | −180.3 | – | – | – |
per 1 mol of | −360.5 | – | – | – |
Changes in standard condition (7)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −394.6 | – | – | – |
per 1 mol of | −98.65 | – | – | – |
per 1 mol of | −197.3 | – | – | – |
per 1 mol of | −98.65 | – | – | – |
−131.5 | – | – | – | |
per 1 mol of | −197.3 | – | – | – |
per 1 mol of | −394.6 | – | – | – |
Changes in standard condition (8)
- Reaction of nickel(II) sulfide and potassium permanganate
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 | −359.5 | – | – | – |
per 1 mol of | −89.88 | – | – | – |
per 1 mol of | −179.8 | – | – | – |
per 1 mol of | −89.88 | – | – | – |
−119.8 | – | – | – | |
per 1 mol of | −179.8 | – | – | – |
per 1 mol of | −359.5 | – | – | – |
Changes in aqueous solution
- Reaction of nickel(II) sulfide and potassium permanganate◆
ΔrG −478.8 kJ/mol K 7.62 × 1083 pK −83.88
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 | −554.8 | −478.8 | −255.4 | – |
per 1 mol of | −138.7 | −119.7 | −63.85 | – |
per 1 mol of | −277.4 | −239.4 | −127.7 | – |
per 1 mol of | −138.7 | −119.7 | −63.85 | – |
−184.9 | −159.6 | −85.13 | – | |
per 1 mol of | −277.4 | −239.4 | −127.7 | – |
per 1 mol of | −554.8 | −478.8 | −255.4 | – |
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 |
---|---|---|---|---|
NiS (cr) | -82.0[1] | -79.5[1] | 52.97[1] | 47.11[1] |
NiS (cr) precipitated | -77.4[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] |
* (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 |
---|---|---|---|---|
NiO (cr) | -239.7[1] | -211.7[1] | 37.99[1] | 44.31[1] |
NiO (g) | 314[1] | – | – | – |
(cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
(cr) monoclinic | 0.33[1] | – | – | – |
(g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
MnO2 (cr) | -520.03[1] | -465.14[1] | 53.05[1] | 54.14[1] |
MnO2 (am) precipitated | -502.5[1] | – | – | – |
K2S (cr) | -380.7[1] | -364.0[1] | 105[1] | – |
K2S (ai) | -471.5[1] | -480.7[1] | 190.4[1] | – |
K2S (cr) 2 hydrate | -975.3[1] | – | – | – |
K2S (cr) 5 hydrate | -1871.5[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (am):Amorphous solid, (ai):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°, -82.0 kJ · mol−1
- ^ ΔfG°, -79.5 kJ · mol−1
- ^ S°, 52.97 J · K−1 · mol−1
- ^ Cp°, 47.11 J · K−1 · mol−1
- ^ ΔfH°, -77.4 kJ · 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°, -239.7 kJ · mol−1
- ^ ΔfG°, -211.7 kJ · mol−1
- ^ S°, 37.99 J · K−1 · mol−1
- ^ Cp°, 44.31 J · K−1 · mol−1
- ^ ΔfH°, 314. kJ · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, -520.03 kJ · mol−1
- ^ ΔfG°, -465.14 kJ · mol−1
- ^ S°, 53.05 J · K−1 · mol−1
- ^ Cp°, 54.14 J · K−1 · mol−1
- ^ ΔfH°, -502.5 kJ · mol−1
- ^ ΔfH°, -380.7 kJ · mol−1
- ^ ΔfG°, -364.0 kJ · mol−1
- ^ S°, 105. J · K−1 · mol−1
- ^ ΔfH°, -471.5 kJ · mol−1
- ^ ΔfG°, -480.7 kJ · mol−1
- ^ S°, 190.4 J · K−1 · mol−1
- ^ ΔfH°, -975.3 kJ · mol−1
- ^ ΔfH°, -1871.5 kJ · mol−1