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SrS + 2HBr → SrBr2 + H2S

The reaction of strontium sulfide and hydrogen bromide yields strontium bromide 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

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SrSStrontium sulfide1
Brønsted base
Salt of weak acid
HBrHydrogen bromide2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
SrBr2Strontium bromide1
Conjugate base
Salt of strong acid
H2SHydrogen sulfide1
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of strontium sulfide and hydrogen bromide
ΔrG−156.0 kJ/mol
K2.14 × 1027
pK−27.33
SrSCrystalline solid + 2HBrGas
SrBr2Crystalline solid + 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
−193.0−156.0−124.72.60
per 1 mol of
−193.0−156.0−124.72.60
per 1 mol of
−96.50−78.00−62.351.30
per 1 mol of
−193.0−156.0−124.72.60
per 1 mol of
−193.0−156.0−124.72.60

Changes in aqueous solution (1)

Reaction of strontium sulfide and hydrogen bromide
ΔrG−125.2 kJ/mol
K8.59 × 1021
pK−21.93
SrSCrystalline solid + 2HBrIonized aqueous solution
SrBr2Ionized 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
−94.0−125.2105.0
per 1 mol of
−94.0−125.2105.0
per 1 mol of
−47.0−62.6052.50
per 1 mol of
−94.0−125.2105.0
per 1 mol of
−94.0−125.2105.0

Changes in aqueous solution (2)

Reaction of strontium sulfide and hydrogen bromide
ΔrG−119.5 kJ/mol
K8.62 × 1020
pK−20.94
SrSCrystalline solid + 2HBrIonized aqueous solution
SrBr2Ionized 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
−113.1−119.520
per 1 mol of
−113.1−119.520
per 1 mol of
−56.55−59.7510
per 1 mol of
−113.1−119.520
per 1 mol of
−113.1−119.520

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
SrS (cr)-472.4[1]-467.8[1]68.2[1]48.70[1]
SrS (g)109[1]
HBr (g)-36.40[1]-53.45[1]198.695[1]29.142[1]
HBr (ai)-121.55[1]-103.96[1]82.4[1]-141.8[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
SrBr2 (cr)-717.6[1]-697.1[1]135.10[1]75.35[1]
SrBr2 (g)-410[1]-444[1]323.5[1]60.7[1]
SrBr2 (ai)-788.89[1]-767.39[1]132.2[1]
SrBr2 (cr)
1 hydrate
-1031.4[1]-954.3[1]180[1]120.9[1]
SrBr2 (cr)
6 hydrate
-2531.3[1]-2174.1[1]406[1]343.5[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

References

List of references

  1. 1