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3Zn(SCN)2 + 50Fe2O3 → 3ZnSO4 + Fe2(SO4)3 + 2Fe(NO3)3 + 6FeCO3 + 90FeO

The reaction of zinc thiocyanate and iron(III) oxide yields zinc sulfate, iron(III) sulfate, iron(III) nitrate, iron(II) carbonate, and iron(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

General equation

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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Zn(SCN)2Zinc thiocyanate3
Reducing
Reducing
Fe2O3Iron(III) oxide50
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnSO4Zinc sulfate3
Oxidized
Fe2(SO4)3Iron(III) sulfate1
Oxidized
Fe(NO3)3Iron(III) nitrate2
Oxidized
FeCO3Iron(II) carbonate6
Reduced
FeOIron(II) oxide90
Reduced

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Un-ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Un-ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (3)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (4)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (5)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Un-ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Ionized aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

Changes in aqueous solution (6)

Reaction of zinc thiocyanate and iron(III) oxide
3Zn(SCN)2Un-ionized aqueous solution + 50Fe2O3Crystalline solid
3ZnSO4Un-ionized aqueous solution + Fe2(SO4)3Ionized aqueous solution + 2Fe(NO3)3Aqueous solution + 6FeCO3Crystalline solidsiderite + 90FeOCrystalline 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
per 1 mol of
per 1 mol of
per 1 mol of
per 1 mol of

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
Zn(SCN)2 (ao)33.1[1]
Fe2O3 (cr)-824.2[1]-742.2[1]87.40[1]103.85[1]
* (ao):Un-ionized aqueous solution, (cr):Crystalline solid

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
ZnSO4 (cr)-982.8[1]-871.5[1]110.5[1]99.2[1]
ZnSO4 (ai)-1063.15[1]-891.59[1]-92.0[1]-247[1]
ZnSO4 (ao)-1047.7[1]-904.9[1]5.0[1]
ZnSO4 (cr)
1 hydrate
-1304.49[1]-1131.99[1]138.5[1]
ZnSO4 (cr)
6 hydrate
-2777.46[1]-2324.44[1]363.6[1]357.69[1]
ZnSO4 (cr)
7 hydrate
-3077.75[1]-2562.67[1]388.7[1]383.42[1]
Fe2(SO4)3 (cr)-2581.5[1]
Fe2(SO4)3 (ai)-2825.0[1]-2242.8[1]-571.5[1]
Fe(NO3)3 (ai)-670.7[1]-338.3[1]123.4[1]
Fe(NO3)3 (aq)-674.9[1]
Fe(NO3)3 (cr)
9 hydrate
-3285.3[1]
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[1]
FeO (cr)-272.0[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):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)