You-iggy
  1. Home
  2. Chemical reactions
  3. (NH4)2S + 2HI → 2NH4I + H2S

(NH4)2S + 2HI → 2NH4I + H2S

Last updated:
Reaction of ammonium sulfide and hydrogen iodide
(NH4)2SAmmonium sulfide + 2HIHydrogen iodide
⟶
2NH4IAmmonium iodide + H2SHydrogen sulfide

The reaction of ammonium sulfide and hydrogen iodide yields ammonium iodide and hydrogen sulfide. 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

Reaction of ammonium sulfide and hydrogen iodide
(NH4)2SAmmonium sulfide + 2HIHydrogen iodide
⟶
2NH4IAmmonium iodide + H2SHydrogen sulfide

General equation

Reaction of salt of weak acid and strong acid with generating weak acid
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Weak acidConjugate acid

Oxidation state of each atom

Reaction of ammonium sulfide and hydrogen iodide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2SAmmonium sulfide1
Brønsted base
Salt of weak acid
HIHydrogen iodide2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NH4IAmmonium iodide2
Conjugate base
Salt of strong acid
H2SHydrogen sulfide1
Conjugate acid
Weak acid

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of ammonium sulfide and hydrogen iodide
◆
ΔrG−119.6 kJ/mol
K8.97 × 1020
pK−20.95
(NH4)2SIonized aqueous solution + 2HIIonized aqueous solution
⟶
2NH4IIonized aqueous solution + H2SGas
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
−53.8−119.6220.5–
per 1 mol of
−53.8−119.6220.5–
per 1 mol of
−26.9−59.80110.3–
per 1 mol of
−26.9−59.80110.3–
per 1 mol of
−53.8−119.6220.5–

Changes in aqueous solution (2)

Reaction of ammonium sulfide and hydrogen iodide
◆
ΔrG−113.9 kJ/mol
K9.00 × 1019
pK−19.95
(NH4)2SIonized aqueous solution + 2HIIonized aqueous solution
⟶
2NH4IIonized aqueous solution + H2SUn-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
−72.9−113.9136–
per 1 mol of
−72.9−113.9136–
per 1 mol of
−36.5−56.9568.0–
per 1 mol of
−36.5−56.9568.0–
per 1 mol of
−72.9−113.9136–

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
(NH4)2S (ai)-231.8[1]-72.6[1]212.1[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]
* (ai):Ionized aqueous solution, (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
NH4I (cr)-201.42[1]-112.5[1]117[1]–
NH4I (ai)-187.69[1]-130.88[1]224.7[1]-62.3[1]
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized 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)