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2NH4I + 4O2 → N2 + I2 + 4H2O2

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Reaction of ammonium iodide and oxygen
2NH4IAmmonium iodide + 4O2Oxygen
⟶
N2Nitrogen + I2Iodine + 4H2O2Hydrogen peroxide

The reaction of ammonium iodide and oxygen yields nitrogen, iodine, and hydrogen peroxide (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 ammonium iodide and oxygen
2NH4IAmmonium iodide + 4O2Oxygen
⟶
N2Nitrogen + I2Iodine + 4H2O2Hydrogen peroxide

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of ammonium iodide and oxygen

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NH4IAmmonium iodide2
Reducing
Reducing
O2Oxygen4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
N2Nitrogen1
Oxidized
–
I2Iodine1
Oxidized
–
H2O2Hydrogen peroxide4
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of ammonium iodide and oxygen
◆
ΔrG−256.4 kJ/mol
K8.30 × 1044
pK−44.92
2NH4ICrystalline solid + 4O2Gas
⟶
N2Gas + I2Crystalline solid + 4H2O2Liquid
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
−348.28−256.4−308–
per 1 mol of
−174.14−128.2−154–
per 1 mol of
−87.070−64.10−77.0–
per 1 mol of
−348.28−256.4−308–
per 1 mol of
−348.28−256.4−308–
per 1 mol of
−87.070−64.10−77.0–

Changes in aqueous solution

Reaction of ammonium iodide and oxygen
◆
ΔrG−323.6 kJ/mol
K4.92 × 1056
pK−56.69
2NH4IIonized aqueous solution + 4O2Un-ionized aqueous solution
⟶
N2Gas + I2Un-ionized aqueous solution + 4H2O2Un-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
−319.9−323.611.4–
per 1 mol of
−159.9−161.85.70–
per 1 mol of
−79.97−80.902.85–
per 1 mol of
−319.9−323.611.4–
per 1 mol of
−319.9−323.611.4–
per 1 mol of
−79.97−80.902.85–

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
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[1]
O2 (g)0[1]0[1]205.138[1]29.355[1]
O2 (ao)-11.7[1]16.4[1]110.9[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (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
N2 (g)0[1]0[1]191.61[1]29.125[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]–
H2O2 (l)-187.78[1]-120.35[1]109.6[1]89.1[1]
H2O2 (g)-136.31[1]-105.57[1]232.7[1]43.1[1]
H2O2 (ao)-191.17[1]-134.03[1]143.9[1]–
* (g):Gas, (cr):Crystalline solid, (ao):Un-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)