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9H2 + Mn(NO3)2 → Mn + 2NH3 + 6H2O

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Reaction of hydrogen and manganese(II) nitrate
9H2Hydrogen + Mn(NO3)2Manganese(II) nitrate
⟶
MnManganese + 2NH3Ammonia + 6H2OWater

The reaction of hydrogen and manganese(II) nitrate yields manganese, ammonia, and water (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 manganese(II) nitrate
9H2Hydrogen + Mn(NO3)2Manganese(II) nitrate
⟶
MnManganese + 2NH3Ammonia + 6H2OWater

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 manganese(II) nitrate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H2Hydrogen9
Reducing
Reducing
Mn(NO3)2Manganese(II) nitrate1
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
MnManganese1
Reduced
–
NH3Ammonia2
Redoxed product
–
H2OWater6
Oxidized
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of hydrogen and manganese(II) nitrate
9H2Gas + Mn(NO3)2Crystalline solid
⟶
MnCrystalline solidα + 2NH3Gas + 6H2OLiquid
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
−1230.94–––
per 1 mol of
−136.771–––
−1230.94–––
per 1 mol of
−1230.94–––
per 1 mol of
−615.470–––
per 1 mol of
−205.157–––

Changes in standard condition (2)

Reaction of hydrogen and manganese(II) nitrate
9H2Gas + Mn(NO3)2Crystalline solid
⟶
MnCrystalline solidβ + 2NH3Gas + 6H2OLiquid
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
––––
per 1 mol of
––––
––––
per 1 mol of
––––
per 1 mol of
––––
per 1 mol of
––––

Changes in standard condition (3)

Reaction of hydrogen and manganese(II) nitrate
9H2Gas + Mn(NO3)2Crystalline solid
⟶
MnCrystalline solidγ + 2NH3Gas + 6H2OLiquid
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
−1229.39–––
per 1 mol of
−136.599–––
−1229.39–––
per 1 mol of
−1229.39–––
per 1 mol of
−614.695–––
per 1 mol of
−204.898–––

Changes in aqueous solution (1)

Reaction of hydrogen and manganese(II) nitrate
◆
ΔrG−1163.2 kJ/mol
K6.08 × 10203
pK−203.78
9H2Un-ionized aqueous solution + Mn(NO3)2Ionized aqueous solution
⟶
MnCrystalline solidα + 2NH3Gas + 6H2OLiquid
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
−1133.9−1163.2−4575–
per 1 mol of
−125.99−129.24−508.3–
−1133.9−1163.2−4575–
per 1 mol of
−1133.9−1163.2−4575–
per 1 mol of
−566.95−581.60−2288–
per 1 mol of
−188.98−193.87−762.5–

Changes in aqueous solution (2)

Reaction of hydrogen and manganese(II) nitrate
◆
ΔrG−1183.3 kJ/mol
K2.02 × 10207
pK−207.31
9H2Un-ionized aqueous solution + Mn(NO3)2Ionized aqueous solution
⟶
MnCrystalline solidα + 2NH3Un-ionized aqueous solution + 6H2OLiquid
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
−1202.3−1183.3−4737–
per 1 mol of
−133.59−131.48−526.3–
−1202.3−1183.3−4737–
per 1 mol of
−1202.3−1183.3−4737–
per 1 mol of
−601.15−591.65−2369–
per 1 mol of
−200.38−197.22−789.5–

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]–
Mn(NO3)2 (cr)-576.26[1]–––
Mn(NO3)2 (ai)-635.5[1]-450.9[1]218[1]-121[1]
Mn(NO3)2 (vit)
6 hydrate
-2371.9[1]–––
Mn(NO3)2 (l)
6 hydrate
-2331.62[1]–––
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (vit):Vitreous liquid, (l):Liquid

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
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]
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[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]
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution, (l):Liquid

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)