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H2 + 2KNO2 → 2NO + 2KOH

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Reaction of hydrogen and potassium nitrite
H2Hydrogen + 2KNO2Potassium nitrite
⟶
2NONitrogen monoxide + 2KOHPotassium hydroxide

The reaction of hydrogen and potassium nitrite yields nitrogen monoxide and potassium hydroxide (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 hydrogen and potassium nitrite
H2Hydrogen + 2KNO2Potassium nitrite
⟶
2NONitrogen monoxide + 2KOHPotassium hydroxide

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 hydrogen and potassium nitrite

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen1
Reducing
Reducing
KNO2Potassium nitrite2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NONitrogen monoxide2
Reduced
–
KOHPotassium hydroxide2
Oxidized
–

Thermodynamic changes

Changes in standard condition

Reaction of hydrogen and potassium nitrite
◆
ΔrG28.04 kJ/mol
K0.12 × 10−4
pK4.91
H2Gas + 2KNO2Crystalline solidrhombic
⟶
2NOGas + 2KOHCrystalline solid
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
70.6128.04144.5−54.1
per 1 mol of
70.6128.04144.5−54.1
per 1 mol of
35.3014.0272.25−27.1
per 1 mol of
35.3014.0272.25−27.1
35.3014.0272.25−27.1

Changes in aqueous solution

Reaction of hydrogen and potassium nitrite
◆
ΔrG−94.7 kJ/mol
K3.90 × 1016
pK−16.59
H2Un-ionized aqueous solution + 2KNO2Ionized aqueous solution
⟶
2NOGas + 2KOHIonized 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
−66.2−94.7−423–
per 1 mol of
−66.2−94.7−423–
per 1 mol of
−33.1−47.4−212–
per 1 mol of
−33.1−47.4−212–
−33.1−47.4−212–

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
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
KNO2 (cr)
rhombic
-369.82[1]-306.55[1]152.09[1]107.40[1]
KNO2 (ai)-356.9[1]-315.4[1]225.5[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
KOH (cr)-424.764[1]-379.08[1]78.9[1]64.9[1]
KOH (g)-231.0[1]-232.6[1]238.3[1]49.20[1]
KOH (ai)-482.37[1]-440.50[1]91.6[1]-126.8[1]
KOH (cr)
1 hydrate
-748.9[1]-645.1[1]117.2[1]–
KOH (cr)
2 hydrate
-1051.0[1]-887.3[1]150.6[1]–
* (g):Gas, (cr):Crystalline solid, (ai):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)