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ZnCO3 + 2HI → ZnI2 + CO2 + H2O

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Reaction of zinc carbonate and hydrogen iodide
ZnCO3Zinc carbonate + 2HIHydrogen iodide
⟶
ZnI2Zinc iodide + CO2Carbon dioxide + H2OWater

The reaction of zinc carbonate and hydrogen iodide yields zinc iodide, carbon dioxide, and water (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of zinc carbonate and hydrogen iodide
ZnCO3Zinc carbonate + 2HIHydrogen iodide
⟶
ZnI2Zinc iodide + CO2Carbon dioxide + H2OWater

General equation

Reaction of salt of weak acid and strong acid with generating weak acidic oxide
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid

Oxidation state of each atom

Reaction of zinc carbonate and hydrogen iodide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnCO3Zinc carbonate1
Brønsted base
Salt of weak acid
HIHydrogen iodide2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
ZnI2Zinc iodide1
Conjugate base
Salt of strong acid
CO2Carbon dioxide1
–
Acidic oxide
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of zinc carbonate and hydrogen iodide
◆
ΔrG−112.32 kJ/mol
K4.76 × 1019
pK−19.68
ZnCO3Crystalline solid + 2HIGas
⟶
ZnI2Crystalline solid + CO2Gas + H2OLiquid
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
−127.55−112.32−50.8–
per 1 mol of
−127.55−112.32−50.8–
per 1 mol of
−63.775−56.160−25.4–
per 1 mol of
−127.55−112.32−50.8–
per 1 mol of
−127.55−112.32−50.8–
per 1 mol of
−127.55−112.32−50.8–

Changes in aqueous solution (1)

Reaction of zinc carbonate and hydrogen iodide
◆
ΔrG−47.03 kJ/mol
K1.74 × 108
pK−8.24
ZnCO3Crystalline solid + 2HIIonized aqueous solution
⟶
ZnI2Ionized aqueous solution + CO2Gas + H2OLiquid
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
−20.44−47.0389.279
per 1 mol of
−20.44−47.0389.279
per 1 mol of
−10.22−23.5244.640
per 1 mol of
−20.44−47.0389.279
per 1 mol of
−20.44−47.0389.279
per 1 mol of
−20.44−47.0389.279

Changes in aqueous solution (2)

Reaction of zinc carbonate and hydrogen iodide
◆
ΔrG−38.65 kJ/mol
K5.90 × 106
pK−6.77
ZnCO3Crystalline solid + 2HIIonized aqueous solution
⟶
ZnI2Ionized aqueous solution + CO2Un-ionized aqueous solution + H2OLiquid
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
−40.73−38.65−7.0–
per 1 mol of
−40.73−38.65−7.0–
per 1 mol of
−20.36−19.32−3.5–
per 1 mol of
−40.73−38.65−7.0–
per 1 mol of
−40.73−38.65−7.0–
per 1 mol of
−40.73−38.65−7.0–

Changes in aqueous solution (3)

Reaction of zinc carbonate and hydrogen iodide
◆
ΔrG−37.4 kJ/mol
K3.57 × 106
pK−6.55
ZnCO3Crystalline solid + 2HIIonized aqueous solution
⟶
ZnI2Un-ionized aqueous solution + CO2Gas + H2OLiquid
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
–−37.4––
per 1 mol of
–−37.4––
per 1 mol of
–−18.7––
per 1 mol of
–−37.4––
per 1 mol of
–−37.4––
per 1 mol of
–−37.4––

Changes in aqueous solution (4)

Reaction of zinc carbonate and hydrogen iodide
◆
ΔrG−29.0 kJ/mol
K1.20 × 105
pK−5.08
ZnCO3Crystalline solid + 2HIIonized aqueous solution
⟶
ZnI2Un-ionized aqueous solution + CO2Un-ionized aqueous solution + H2OLiquid
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
–−29.0––
per 1 mol of
–−29.0––
per 1 mol of
–−14.5––
per 1 mol of
–−29.0––
per 1 mol of
–−29.0––
per 1 mol of
–−29.0––

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
ZnCO3 (cr)-812.78[1]-731.52[1]82.4[1]79.71[1]
ZnCO3 (cr)
1 hydrate
–-970.6[1]––
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[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
ZnI2 (cr)-208.03[1]-208.95[1]161.1[1]–
ZnI2 (ai)-264.26[1]-250.20[1]110.5[1]-238[1]
ZnI2 (ao)–-240.6[1]––
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[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, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas, (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)