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6Na + 4MnSO4 → 3Na2SO4 + S + 4MnO

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Reaction of sodium and manganese(II) sulfate
6NaSodium + 4MnSO4Manganese(II) sulfate
⟶
3Na2SO4Sodium sulfate + SSulfur + 4MnOManganese(II) oxide

The reaction of sodium and manganese(II) sulfate yields sodium sulfate, sulfur, and manganese(II) oxide (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) sulfate
6NaSodium + 4MnSO4Manganese(II) sulfate
⟶
3Na2SO4Sodium sulfate + SSulfur + 4MnOManganese(II) oxide

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) sulfate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium6
Reducing
Reducing
MnSO4Manganese(II) sulfate4
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2SO4Sodium sulfate3
Oxidized
–
SSulfur1
Reduced
–
MnOManganese(II) oxide4
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and manganese(II) sulfate
◆
ΔrG−1432.64 kJ/mol
K9.72 × 10250
pK−250.99
6NaCrystalline solid + 4MnSO4Crystalline solid
⟶
3Na2SO4Crystalline solidorthorhombic + SCrystalline solidrhombic + 4MnOCrystalline 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
−1441.12−1432.64−36.317.56
per 1 mol of
−240.187−238.773−6.052.927
−360.280−358.160−9.074.390
per 1 mol of
−480.373−477.547−12.15.853
per 1 mol of
−1441.12−1432.64−36.317.56
−360.280−358.160−9.074.390

Changes in standard condition (2)

Reaction of sodium and manganese(II) sulfate
6NaCrystalline solid + 4MnSO4Crystalline solid
⟶
3Na2SO4Crystalline solidorthorhombic + SCrystalline solidmonoclinic + 4MnOCrystalline 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
−1440.79–––
per 1 mol of
−240.132–––
−360.197–––
per 1 mol of
−480.263–––
per 1 mol of
−1440.79–––
−360.197–––

Changes in standard condition (3)

Reaction of sodium and manganese(II) sulfate
6NaCrystalline solid + 4MnSO4Crystalline solid
⟶
3Na2SO4Crystalline solidmetastable + SCrystalline solidrhombic + 4MnOCrystalline 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
––−20.220.83
per 1 mol of
––−3.373.472
––−5.055.207
per 1 mol of
––−6.736.943
per 1 mol of
––−20.220.83
––−5.055.207

Changes in standard condition (4)

Reaction of sodium and manganese(II) sulfate
6NaCrystalline solid + 4MnSO4Crystalline solid
⟶
3Na2SO4Crystalline solidmetastable + SCrystalline solidmonoclinic + 4MnOCrystalline 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
––––
per 1 mol of
––––
––––
per 1 mol of
––––
per 1 mol of
––––
––––

Changes in aqueous solution (1)

Reaction of sodium and manganese(II) sulfate
◆
ΔrG−1313.9 kJ/mol
K1.53 × 10230
pK−230.19
6NaCrystalline solid + 4MnSO4Un-ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + SCrystalline solidrhombic + 4MnOCrystalline 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
−1245.8−1313.9232.1–
per 1 mol of
−207.63−218.9838.68–
−311.45−328.4858.02–
per 1 mol of
−415.27−437.9777.37–
per 1 mol of
−1245.8−1313.9232.1–
−311.45−328.4858.02–

Changes in aqueous solution (2)

Reaction of sodium and manganese(II) sulfate
◆
ΔrG−1365.9 kJ/mol
K1.97 × 10239
pK−239.30
6NaCrystalline solid + 4MnSO4Ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + SCrystalline solidrhombic + 4MnOCrystalline 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
−1189.0−1365.9592.1404
per 1 mol of
−198.17−227.6598.6867.3
−297.25−341.48148.0101
per 1 mol of
−396.33−455.30197.4135
per 1 mol of
−1189.0−1365.9592.1404
−297.25−341.48148.0101

Changes in aqueous solution (3)

Reaction of sodium and manganese(II) sulfate
◆
ΔrG−1313.9 kJ/mol
K1.53 × 10230
pK−230.19
6NaCrystalline solid + 4MnSO4Un-ionized aqueous solution
⟶
3Na2SO4Ionized aqueous solution + SCrystalline solidrhombic + 4MnOCrystalline 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
−1245.8−1313.9232.1–
per 1 mol of
−207.63−218.9838.68–
−311.45−328.4858.02–
per 1 mol of
−415.27−437.9777.37–
per 1 mol of
−1245.8−1313.9232.1–
−311.45−328.4858.02–

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]
MnSO4 (cr)-1065.25[1]-957.36[1]112.1[1]100.50[1]
MnSO4 (ai)-1130.1[1]-972.7[1]-53.6[1]-243[1]
MnSO4 (ao)-1115.9[1]-985.7[1]36.4[1]–
MnSO4 (cr)
1 hydrate
α
-1376.5[1]–––
MnSO4 (cr)
1 hydrate
β
-1348.1[1]–––
MnSO4 (cr)
4 hydrate
-2258.1[1]–––
MnSO4 (cr)
5 hydrate
-2553.1[1]––326[1]
MnSO4 (cr)
7 hydrate
-3139.3[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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
Na2SO4 (cr)
orthorhombic
-1387.08[1]-1270.16[1]149.58[1]128.20[1]
Na2SO4 (cr)
metastable
––154.934[1]129.29[1]
Na2SO4 (ai)-1389.51[1]-1268.36[1]138.1[1]-201[1]
Na2SO4 (cr)
10 hydrate
-4327.26[1]-3646.85[1]592.0[1]–
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[1]
MnO (cr)-385.22[1]-362.90[1]59.71[1]45.44[1]
MnO (g)124.22[1]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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)