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FeCO3 + 2CsOH → Cs2CO3 + Fe(OH)2

The reaction of iron(II) carbonate and caesium hydroxide yields caesium carbonate and iron(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
FeCO3Iron(II) carbonate1
Brønsted acid
Salt of weak base
CsOHCaesium hydroxide2
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cs2CO3Caesium carbonate1
Conjugate acid
Salt of strong base
Fe(OH)2Iron(II) hydroxide1
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition

Reaction of iron(II) carbonate and caesium hydroxide
FeCO3Crystalline solidsiderite + 2CsOHCrystalline solid
Cs2CO3Crystalline solid + Fe(OH)2Crystalline solidprecipitated
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
−133.7
per 1 mol of
−133.7
per 1 mol of
−66.85
per 1 mol of
−133.7
per 1 mol of
−133.7

Changes in aqueous solution

Reaction of iron(II) carbonate and caesium hydroxide
ΔrG−33.2 kJ/mol
K6.55 × 105
pK−5.82
FeCO3Crystalline solidsiderite + 2CsOHIonized aqueous solution
Cs2CO3Ionized aqueous solution + Fe(OH)2Crystalline solidprecipitated
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
−45.6−33.2−40
per 1 mol of
−45.6−33.2−40
per 1 mol of
−22.8−16.6−20
per 1 mol of
−45.6−33.2−40
per 1 mol of
−45.6−33.2−40

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
FeCO3 (cr)
siderite
-740.57[1]-666.67[1]92.9[1]82.13[1]
CsOH (cr)-417.23[1]
CsOH (g)-247[1]-247[1]254.83[1]49.71[1]
CsOH (ai)-488.27[1]-449.25[1]122.30[1]
CsOH (cr)
1 hydrate
-754.04[1]
* (cr):Crystalline solid, (g):Gas, (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
Cs2CO3 (cr)-1139.7[1]-1054.3[1]204.47[1]123.85[1]
Cs2CO3 (ai)-1193.70[1]-1111.85[1]209.2[1]
Cs2CO3 (cr)
3 hydrate
-2048.1[1]
Fe(OH)2 (cr)
precipitated
-569.0[1]-486.5[1]88[1]
Fe(OH)2 (g)-372[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

References

List of references

  1. 1