You-iggy
  1. Home
  2. Chemical reactions
  3. 4KH + O2 → 2K2O + 2H2

4KH + O2 → 2K2O + 2H2

Last updated:
Reaction of potassium hydride and oxygen
4KHPotassium hydride + O2Oxygen
⟶
2K2OPotassium oxide + 2H2Hydrogen

The reaction of potassium hydride and oxygen yields potassium oxide 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 potassium hydride and oxygen
4KHPotassium hydride + O2Oxygen
⟶
2K2OPotassium oxide + 2H2Hydrogen

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 potassium hydride and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KHPotassium hydride4
Reducing
Reducing
O2Oxygen1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2OPotassium oxide2
Reduced
–
H2Hydrogen2
Oxidized
–

Thermodynamic changes

Changes in standard condition

Reaction of potassium hydride and oxygen
4KHCrystalline solid + O2Gas
⟶
2K2OCrystalline solid + 2H2Gas
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
−492.0–––
per 1 mol of
−123.0–––
per 1 mol of
−492.0–––
per 1 mol of
−246.0–––
per 1 mol of
−246.0–––

Changes in aqueous solution (1)

Reaction of potassium hydride and oxygen
4KHCrystalline solid + O2Un-ionized aqueous solution
⟶
2K2OCrystalline solid + 2H2Gas
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
−480.3–––
per 1 mol of
−120.1–––
per 1 mol of
−480.3–––
per 1 mol of
−240.2–––
per 1 mol of
−240.2–––

Changes in aqueous solution (2)

Reaction of potassium hydride and oxygen
4KHCrystalline solid + O2Un-ionized aqueous solution
⟶
2K2OCrystalline solid + 2H2Un-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
−488.7–––
per 1 mol of
−122.2–––
per 1 mol of
−488.7–––
per 1 mol of
−244.3–––
per 1 mol of
−244.3–––

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
KH (cr)-57.74[1]–––
KH (g)130[1]113[1]192.41[1]31.049[1]
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-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
K2O (cr)-361.5[1]-322.1[2]94.1[2]83.7[2]
K2O (g)-63[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)
    • 2
      James G. Speight (2017)
      Lange's Handbook of Chemistry, 17th edition
      McGraw Hill Education