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Sr(NO3)2 + K2S 💧→ SrS↓ + 2KNO3

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Reaction of strontium nitrate and potassium sulfide
Sr(NO3)2Strontium nitrate + K2SPotassium sulfide
💧
⟶
SrS↓Strontium sulfide + 2KNO3Potassium nitrate

The reaction of strontium nitrate and potassium sulfide yields strontium sulfide and potassium nitrate. 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 strontium nitrate and potassium sulfide
Sr(NO3)2Strontium nitrate + K2SPotassium sulfide
💧
⟶
SrS↓Strontium sulfide + 2KNO3Potassium nitrate

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of strontium nitrate and potassium sulfide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Sr(NO3)2Strontium nitrate1
Lewis acid
Very soluble in water
K2SPotassium sulfide1
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrSStrontium sulfide1
Lewis conjugate
Slightly soluble in water
KNO3Potassium nitrate2
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of strontium nitrate and potassium sulfide
◆
ΔrG−113.5 kJ/mol
K7.66 × 1019
pK−19.88
Sr(NO3)2Crystalline solid + K2SCrystalline solid
💧
⟶
SrS↓Crystalline solid + 2KNO3Crystalline solid
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
−102.7−113.535–
per 1 mol of
−102.7−113.535–
per 1 mol of
−102.7−113.535–
per 1 mol of
−102.7−113.535–
per 1 mol of
−51.35−56.7518–

Changes in aqueous solution

Reaction of strontium nitrate and potassium sulfide
◆
ΔrG5.8 kJ/mol
K0.96 × 10−1
pK1.02
Sr(NO3)2Ionized aqueous solution + K2SIonized aqueous solution
💧
⟶
SrS↓Crystalline solid + 2KNO3Ionized 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
40.15.8115.4–
per 1 mol of
40.15.8115.4–
per 1 mol of
40.15.8115.4–
per 1 mol of
40.15.8115.4–
per 1 mol of
20.12.957.70–

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
Sr(NO3)2 (cr)-978.22[1]-780.02[1]194.56[1]149.91[1]
Sr(NO3)2 (ai)-960.52[1]-781.98[1]260.2[1]–
Sr(NO3)2 (cr)
4 hydrate
-2154.8[1]-1730.39[1]369.0[1]–
K2S (cr)-380.7[1]-364.0[1]105[1]–
K2S (ai)-471.5[1]-480.7[1]190.4[1]–
K2S (cr)
2 hydrate
-975.3[1]–––
K2S (cr)
5 hydrate
-1871.5[1]–––
* (cr):Crystalline solid, (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
SrS (cr)-472.4[1]-467.8[1]68.2[1]48.70[1]
SrS (g)109[1]–––
KNO3 (cr)-494.63[1]-394.86[1]133.05[1]96.40[1]
KNO3 (ai)-459.74[1]-394.53[1]248.9[1]-64.9[1]
* (cr):Crystalline solid, (g):Gas, (ai):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)