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8NaH + KMnO4 → 4Na2O + K + Mn + 4H2↑

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Reaction of sodium hydride and potassium permanganate
8NaHSodium hydride + KMnO4Potassium permanganate
⟶
4Na2OSodium oxide + KPotassium + MnManganese + 4H2↑Hydrogen

The reaction of sodium hydride and potassium permanganate yields sodium oxide, potassium, manganese, and hydrogen (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of sodium hydride and potassium permanganate
8NaHSodium hydride + KMnO4Potassium permanganate
⟶
4Na2OSodium oxide + KPotassium + MnManganese + 4H2↑Hydrogen

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 sodium hydride and potassium permanganate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaHSodium hydride8
Reducing
Reducing
KMnO4Potassium permanganate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide4
–
–
KPotassium1
Reduced
–
MnManganese1
Reduced
–
H2Hydrogen4
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium hydride and potassium permanganate
◆
ΔrG−496.6 kJ/mol
K1.00 × 1087
pK−87.00
8NaHCrystalline solid + KMnO4Crystalline solid
⟶
4Na2OCrystalline solid + KCrystalline solid + MnCrystalline solidα + 4H2↑Gas
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
−369.5−496.6427.3338.90
per 1 mol of
−46.19−62.0853.4164.862
−369.5−496.6427.3338.90
per 1 mol of
−92.38−124.2106.839.725
per 1 mol of
−369.5−496.6427.3338.90
per 1 mol of
−369.5−496.6427.3338.90
per 1 mol of
−92.38−124.2106.839.725

Changes in standard condition (2)

Reaction of sodium hydride and potassium permanganate
8NaHCrystalline solid + KMnO4Crystalline solid
⟶
4Na2OCrystalline solid + KCrystalline solid + MnCrystalline solidβ + 4H2↑Gas
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
––429.7139.11
per 1 mol of
––53.7144.889
––429.7139.11
per 1 mol of
––107.439.777
per 1 mol of
––429.7139.11
per 1 mol of
––429.7139.11
per 1 mol of
––107.439.777

Changes in standard condition (3)

Reaction of sodium hydride and potassium permanganate
◆
ΔrG−495.1 kJ/mol
K5.47 × 1086
pK−86.74
8NaHCrystalline solid + KMnO4Crystalline solid
⟶
4Na2OCrystalline solid + KCrystalline solid + MnCrystalline solidγ + 4H2↑Gas
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
−367.9−495.1427.7540.15
per 1 mol of
−45.99−61.8953.4695.019
−367.9−495.1427.7540.15
per 1 mol of
−91.97−123.8106.9410.04
per 1 mol of
−367.9−495.1427.7540.15
per 1 mol of
−367.9−495.1427.7540.15
per 1 mol of
−91.97−123.8106.9410.04

Changes in aqueous solution (1)

Reaction of sodium hydride and potassium permanganate
◆
ΔrG−503.7 kJ/mol
K1.76 × 1088
pK−88.24
8NaHCrystalline solid + KMnO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + KCrystalline solid + MnCrystalline solidα + 4H2↑Gas
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
−412.9−503.7305.3216.7
per 1 mol of
−51.61−62.9638.1627.09
−412.9−503.7305.3216.7
per 1 mol of
−103.2−125.976.3354.17
per 1 mol of
−412.9−503.7305.3216.7
per 1 mol of
−412.9−503.7305.3216.7
per 1 mol of
−103.2−125.976.3354.17

Changes in aqueous solution (2)

Reaction of sodium hydride and potassium permanganate
◆
ΔrG−433.3 kJ/mol
K8.14 × 1075
pK−75.91
8NaHCrystalline solid + KMnO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + KCrystalline solid + MnCrystalline solidα + 4H2↑Un-ionized aqueous solution
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
−429.7−433.32091–
per 1 mol of
−53.71−54.16261.4–
−429.7−433.32091–
per 1 mol of
−107.4−108.3522.8–
per 1 mol of
−429.7−433.32091–
per 1 mol of
−429.7−433.32091–
per 1 mol of
−107.4−108.3522.8–

Thermodynamic data of reactants

Chemical formulaStandard 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
NaH (cr)-56.275[1]-33.46[1]40.016[1]36.401[1]
NaH (g)130.25[1]108.85[1]188.377[1]30.29[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, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard 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
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[1]
K (cr)0[1]0[1]64.18[1]29.58[1]
K (g)89.24[1]60.59[1]160.336[1]20.786[1]
Mn (cr)
α
0[1]0[1]32.01[1]26.32[1]
Mn (cr)
β
––34.39[1]26.53[1]
Mn (cr)
γ
1.55[1]1.42[1]32.43[1]27.57[1]
Mn (g)280.7[1]238.5[1]173.70[1]20.79[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)