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8Na + (NH4)3PO4 → 4Na2O + PH3↑ + 3NH3↑

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Reaction of sodium and ammonium phosphate
8NaSodium + (NH4)3PO4Ammonium phosphate
⟶
4Na2OSodium oxide + PH3↑Phosphine + 3NH3↑Ammonia

The reaction of sodium and ammonium phosphate yields sodium oxide, phosphine, and ammonia (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

Reaction of sodium and ammonium phosphate
8NaSodium + (NH4)3PO4Ammonium phosphate
⟶
4Na2OSodium oxide + PH3↑Phosphine + 3NH3↑Ammonia

General equation

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

Oxidation state of each atom

Reaction of sodium and ammonium phosphate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium8
Reducing
Reducing
(NH4)3PO4Ammonium phosphate1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2OSodium oxide4
Oxidized
–
PH3Phosphine1
Reduced
–
NH3Ammonia3
–
–

Thermodynamic changes

Changes in standard condition

Reaction of sodium and ammonium phosphate
8NaCrystalline solid + (NH4)3PO4Crystalline solid
⟶
4Na2OCrystalline solid + PH3↑Gas + 3NH3↑Gas
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
−117.9–––
per 1 mol of
−14.74–––
per 1 mol of
−117.9–––
per 1 mol of
−29.48–––
per 1 mol of
−117.9–––
per 1 mol of
−39.30–––

Changes in aqueous solution (1)

Reaction of sodium and ammonium phosphate
◆
ΔrG−281.2 kJ/mol
K1.84 × 1049
pK−49.26
8NaCrystalline solid + (NH4)3PO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + PH3↑Gas + 3NH3↑Gas
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
−114.9−281.2561–
per 1 mol of
−14.36−35.1570.1–
per 1 mol of
−114.9−281.2561–
per 1 mol of
−28.73−70.30140–
per 1 mol of
−114.9−281.2561–
per 1 mol of
−38.30−93.73187–

Changes in aqueous solution (2)

Reaction of sodium and ammonium phosphate
◆
ΔrG−311.3 kJ/mol
K3.45 × 1054
pK−54.54
8NaCrystalline solid + (NH4)3PO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + PH3↑Gas + 3NH3↑Un-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
−217.5−311.3318–
per 1 mol of
−27.19−38.9139.8–
per 1 mol of
−217.5−311.3318–
per 1 mol of
−54.38−77.8379.5–
per 1 mol of
−217.5−311.3318–
per 1 mol of
−72.50−103.8106–

Changes in aqueous solution (3)

Reaction of sodium and ammonium phosphate
◆
ΔrG−269.2 kJ/mol
K1.45 × 1047
pK−47.16
8NaCrystalline solid + (NH4)3PO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + PH3↑Un-ionized aqueous solution + 3NH3↑Gas
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
−129.8−269.2471–
per 1 mol of
−16.23−33.6558.9–
per 1 mol of
−129.8−269.2471–
per 1 mol of
−32.45−67.30118–
per 1 mol of
−129.8−269.2471–
per 1 mol of
−43.27−89.73157–

Changes in aqueous solution (4)

Reaction of sodium and ammonium phosphate
◆
ΔrG−299.4 kJ/mol
K2.84 × 1052
pK−52.45
8NaCrystalline solid + (NH4)3PO4Ionized aqueous solution
⟶
4Na2OCrystalline solid + PH3↑Un-ionized aqueous solution + 3NH3↑Un-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
−232.4−299.4228–
per 1 mol of
−29.05−37.4228.5–
per 1 mol of
−232.4−299.4228–
per 1 mol of
−58.10−74.8557.0–
per 1 mol of
−232.4−299.4228–
per 1 mol of
−77.47−99.8076.0–

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]
(NH4)3PO4 (cr)-1671.9[1]–––
(NH4)3PO4 (ai)-1674.9[1]-1256.6[1]117[1]–
(NH4)3PO4 (cr)
3 hydrate
-2555.6[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
Na2O (cr)-414.22[1]-375.46[1]75.06[1]69.12[1]
Na2O (g)-35.6[1]-52.3[1]261.2[1]55.2[1]
PH3 (g)5.4[1]13.4[1]210.23[1]37.11[1]
PH3 (ao)-9.50[1]25.36[1]120.1[1]–
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]–
* (cr):Crystalline solid, (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)