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4Na + MnCO3 → 2Na2O + MnO + C

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Reaction of sodium and manganese(II) carbonate
4NaSodium + MnCO3Manganese(II) carbonate
⟶
2Na2OSodium oxide + MnOManganese(II) oxide + CCarbon

The reaction of sodium and manganese(II) carbonate yields sodium oxide, manganese(II) oxide, and carbon (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 and manganese(II) carbonate
4NaSodium + MnCO3Manganese(II) carbonate
⟶
2Na2OSodium oxide + MnOManganese(II) oxide + CCarbon

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium and manganese(II) carbonate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium4
Reducing
Reducing
MnCO3Manganese(II) carbonate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide2
Oxidized
–
MnOManganese(II) oxide1
–
–
CCarbon1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and manganese(II) carbonate
◆
ΔrG−297.1 kJ/mol
K1.12 × 1052
pK−52.05
4NaCrystalline solid + MnCO3Crystalline solidnatural
⟶
2Na2OCrystalline solid + MnOCrystalline solid + CCrystalline solidgraphite
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
−319.6−297.1−75.1−2.25
per 1 mol of
−79.90−74.28−18.8−0.563
−319.6−297.1−75.1−2.25
per 1 mol of
−159.8−148.6−37.5−1.13
−319.6−297.1−75.1−2.25
per 1 mol of
−319.6−297.1−75.1−2.25

Changes in standard condition (2)

Reaction of sodium and manganese(II) carbonate
◆
ΔrG−294.2 kJ/mol
K3.48 × 1051
pK−51.54
4NaCrystalline solid + MnCO3Crystalline solidnatural
⟶
2Na2OCrystalline solid + MnOCrystalline solid + CCrystalline soliddiamond
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
−317.7−294.2−78.4−4.67
per 1 mol of
−79.42−73.55−19.6−1.17
−317.7−294.2−78.4−4.67
per 1 mol of
−158.8−147.1−39.2−2.33
−317.7−294.2−78.4−4.67
per 1 mol of
−317.7−294.2−78.4−4.67

Changes in standard condition (3)

Reaction of sodium and manganese(II) carbonate
4NaCrystalline solid + MnCO3Crystalline solidprecipitated
⟶
2Na2OCrystalline solid + MnOCrystalline solid + CCrystalline solidgraphite
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
−330.5–––
per 1 mol of
−82.63–––
−330.5–––
per 1 mol of
−165.3–––
−330.5–––
per 1 mol of
−330.5–––

Changes in standard condition (4)

Reaction of sodium and manganese(II) carbonate
4NaCrystalline solid + MnCO3Crystalline solidprecipitated
⟶
2Na2OCrystalline solid + MnOCrystalline solid + CCrystalline soliddiamond
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
−328.6–––
per 1 mol of
−82.15–––
−328.6–––
per 1 mol of
−164.3–––
−328.6–––
per 1 mol of
−328.6–––

Changes in aqueous solution

Reaction of sodium and manganese(II) carbonate
◆
ΔrG−297.1 kJ/mol
K1.12 × 1052
pK−52.05
4NaCrystalline solid + MnCO3Crystalline solidnatural
⟶
2Na2OCrystalline solid + MnOCrystalline solid + CCrystalline solidgraphite
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
−319.6−297.1−75.1−2.25
per 1 mol of
−79.90−74.28−18.8−0.563
−319.6−297.1−75.1−2.25
per 1 mol of
−159.8−148.6−37.5−1.13
−319.6−297.1−75.1−2.25
per 1 mol of
−319.6−297.1−75.1−2.25

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[1]
MnCO3 (cr)
natural
-894.1[1]-816.7[1]85.8[1]81.50[1]
MnCO3 (cr)
precipitated
-883.2[1]–––
* (cr):Crystalline solid, (g):Gas

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]
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]–––
C (cr)
graphite
0[1]0[1]5.740[1]8.527[1]
C (cr)
diamond
1.895[1]2.900[1]2.377[1]6.113[1]
C (g)716.682[1]671.257[1]158.096[1]20.838[1]
* (cr):Crystalline solid, (g):Gas

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)