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2Na + SrBr2 🔥→ 2NaBr + Sr

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Reaction of sodium and strontium bromide
2NaSodium + SrBr2Strontium bromide
🔥
⟶
2NaBrSodium bromide + SrStrontium

The reaction of sodium and strontium bromide yields sodium bromide and strontium. 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 categories

Reaction data

Chemical equation

Reaction of sodium and strontium bromide
2NaSodium + SrBr2Strontium bromide
🔥
⟶
2NaBrSodium bromide + SrStrontium

General equation

Reaction of reducing species and hardly reducible species
Reducing speciesReducing agent + Hardly reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium and strontium bromide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium2
Reducing
Reducing
SrBr2Strontium bromide1
Oxidizing
Hardly reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaBrSodium bromide2
Oxidized
–
SrStrontium1
Reduced
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and strontium bromide
◆
ΔrG−0.9 kJ/mol
K1.44 × 100
pK−0.16
2NaCrystalline solid + SrBr2Crystalline solid
🔥
⟶
2NaBrCrystalline solid + SrCrystalline solidα
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
−4.5−0.9−11.6−2.7
per 1 mol of
−2.3−0.45−5.80−1.4
per 1 mol of
−4.5−0.90−11.6−2.7
per 1 mol of
−2.3−0.45−5.80−1.4
per 1 mol of
−4.5−0.90−11.6−2.7

Changes in aqueous solution

Reaction of sodium and strontium bromide
◆
ΔrG35.69 kJ/mol
K0.56 × 10−6
pK6.25
2NaCrystalline solid + SrBr2Ionized aqueous solution
🔥
⟶
2NaBrIonized aqueous solution + SrCrystalline solidα
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
65.5635.69100.5–
per 1 mol of
32.7817.8450.25–
per 1 mol of
65.5635.69100.5–
per 1 mol of
32.7817.8450.25–
per 1 mol of
65.5635.69100.5–

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[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]
* (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
NaBr (cr)-361.062[1]-348.983[1]86.82[1]51.38[1]
NaBr (g)-143.1[1]-177.06[1]241.19[1]36.32[1]
NaBr (ai)-361.665[1]-365.849[1]141.4[1]-95.4[1]
NaBr (cr)
2 hydrate
-951.94[1]-828.29[1]179.1[1]–
Sr (cr)
α
0[1]0[1]52.3[1]26.4[1]
Sr (g)164.4[1]130.9[1]164.62[1]20.786[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)