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3Mg(ClO4)2 + 2Na3PO4 💧→ Mg3(PO4)2↓ + 6NaClO4

The reaction of magnesium perchlorate and sodium phosphate yields magnesium phosphate and sodium perchlorate. 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
Mg(ClO4)2Magnesium perchlorate3
Lewis acid
Very soluble in water
Na3PO4Sodium phosphate2
Lewis base
Soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Mg3(PO4)2Magnesium phosphate1
Lewis conjugate
Very slightly soluble in water
NaClO4Sodium perchlorate6
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of magnesium perchlorate and sodium phosphate
3Mg(ClO4)2Crystalline solid + 2Na3PO4Crystalline solid
💧
Mg3(PO4)2Crystalline solid + 6NaClO4Crystalline 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
−539.0
−179.7
per 1 mol of
−269.5
−539.0
per 1 mol of
−89.83

Changes in aqueous solution

Reaction of magnesium perchlorate and sodium phosphate
ΔrG−136.8 kJ/mol
K9.25 × 1023
pK−23.97
3Mg(ClO4)2Ionized aqueous solution + 2Na3PO4Ionized aqueous solution
💧
Mg3(PO4)2Crystalline solid + 6NaClO4Ionized 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
174.9−136.81044.1
58.30−45.60348.03
per 1 mol of
87.45−68.40522.05
174.9−136.81044.1
per 1 mol of
29.15−22.80174.02

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
Mg(ClO4)2 (cr)-568.90[1]
Mg(ClO4)2 (ai)-725.51[1]-471.8[1]225.9[1]
Mg(ClO4)2 (cr)
2 hydrate
-1218.8[1]
Mg(ClO4)2 (cr)
4 hydrate
-1837.2[1]
Mg(ClO4)2 (cr)
6 hydrate
-2445.5[1]-1862.7[1]520.9[1]
Na3PO4 (cr)-1917.40[1]-1788.80[1]173.80[1]153.47[1]
Na3PO4 (ai)-1997.9[1]-1804.5[1]-43.3[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
Mg3(PO4)2 (cr)-3780.7[1]-3538.7[1]189.20[1]213.47[1]
NaClO4 (cr)-383.30[1]-254.85[1]142.3[1]
NaClO4 (ai)-369.45[1]-270.41[1]241.0[1]
NaClO4 (cr)
1 hydrate
-677.77[1]-494.29[1]190.8[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1