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  3. 10ZnI2 + 2HNO3 + 20H^+ → 10Zn^2+ + 9I2 + 2NH4I + 6H2O + H2↑

10ZnI2 + 2HNO3 + 20H+ → 10Zn2+ + 9I2 + 2NH4I + 6H2O + H2↑

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Reaction of zinc iodide and nitric acid under acidic condition
10ZnI2Zinc iodide + 2HNO3Nitric acid + 20H+Hydrogen ion
⟶
10Zn2+Zinc ion + 9I2Iodine + 2NH4IAmmonium iodide + 6H2OWater + H2↑Hydrogen

The reaction of zinc iodide, nitric acid, and hydrogen ion yields zinc ion, iodine, ammonium iodide, water, and hydrogen (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 zinc iodide and nitric acid under acidic condition
10ZnI2Zinc iodide + 2HNO3Nitric acid + 20H+Hydrogen ion
⟶
10Zn2+Zinc ion + 9I2Iodine + 2NH4IAmmonium iodide + 6H2OWater + H2↑Hydrogen

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
⟶
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of zinc iodide and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
ZnI2Zinc iodide10
Reducing
Oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion20
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
Zn2+Zinc ion10
–
–
I2Iodine9
Oxidized
–
NH4IAmmonium iodide2
Reduced
–
H2OWater6
–
Water
H2Hydrogen1
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc iodide and nitric acid under acidic condition
◆
ΔrG−283.03 kJ/mol
K3.84 × 1049
pK−49.58
10ZnI2Ionized aqueous solution + 2HNO3Ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
10Zn2+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2NH4IIonized aqueous solution + 6H2OLiquid + H2↑Gas
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
−368.5−283.03−284.5–
per 1 mol of
−36.85−28.303−28.45–
per 1 mol of
−184.3−141.51−142.3–
per 1 mol of
Hydrogen ion
−18.43−14.151−14.22–
per 1 mol of
Zinc ion
−36.85−28.303−28.45–
per 1 mol of
−40.94−31.448−31.61–
per 1 mol of
−184.3−141.51−142.3–
per 1 mol of
−61.42−47.172−47.42–
per 1 mol of
−368.5−283.03−284.5–

Changes in standard condition (2)

Reaction of zinc iodide and nitric acid under acidic condition
◆
ΔrG−265.4 kJ/mol
K3.13 × 1046
pK−46.50
10ZnI2Ionized aqueous solution + 2HNO3Ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
10Zn2+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2NH4IIonized aqueous solution + 6H2OLiquid + H2↑Un-ionized aqueous solution
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
−372.7−265.4162–
per 1 mol of
−37.27−26.5416.2–
per 1 mol of
−186.3−132.781.0–
per 1 mol of
Hydrogen ion
−18.63−13.278.10–
per 1 mol of
Zinc ion
−37.27−26.5416.2–
per 1 mol of
−41.41−29.4918.0–
per 1 mol of
−186.3−132.781.0–
per 1 mol of
−62.12−44.2327.0–
per 1 mol of
−372.7−265.4162–

Changes in standard condition (3)

Reaction of zinc iodide and nitric acid under acidic condition
◆
ΔrG−379.0 kJ/mol
K2.50 × 1066
pK−66.40
10ZnI2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
10Zn2+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2NH4IIonized aqueous solution + 6H2OLiquid + H2↑Gas
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
–−379.0––
per 1 mol of
–−37.90––
per 1 mol of
–−189.5––
per 1 mol of
Hydrogen ion
–−18.95––
per 1 mol of
Zinc ion
–−37.90––
per 1 mol of
–−42.11––
per 1 mol of
–−189.5––
per 1 mol of
–−63.17––
per 1 mol of
–−379.0––

Changes in standard condition (4)

Reaction of zinc iodide and nitric acid under acidic condition
◆
ΔrG−361.4 kJ/mol
K2.06 × 1063
pK−63.31
10ZnI2Un-ionized aqueous solution + 2HNO3Ionized aqueous solution + 20H+Un-ionized aqueous solution
⟶
10Zn2+Un-ionized aqueous solution + 9I2Un-ionized aqueous solution + 2NH4IIonized aqueous solution + 6H2OLiquid + H2↑Un-ionized aqueous solution
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
–−361.4––
per 1 mol of
–−36.14––
per 1 mol of
–−180.7––
per 1 mol of
Hydrogen ion
–−18.07––
per 1 mol of
Zinc ion
–−36.14––
per 1 mol of
–−40.16––
per 1 mol of
–−180.7––
per 1 mol of
–−60.23––
per 1 mol of
–−361.4––

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
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]––
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (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
Zn2+ (g)2782.78[1]–––
Zn2+ (ao)-153.89[1]-147.06[1]-112.1[1]46[1]
I2 (cr)0[1]0[1]116.135[1]54.438[1]
I2 (g)62.438[1]19.327[1]260.69[1]36.90[1]
I2 (ao)22.6[1]16.40[1]137.2[1]–
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[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]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution, (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)