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Zn3P2 + 6HNO3 → 3Zn(NO3)2 + 2P + 3H2

The reaction of zinc phosphide and nitric acid yields zinc nitrate, phosphorus, and hydrogen (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

General equation

Reaction of reducing species and oxidizing species
Reducing speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of zinc phosphide and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Zn3P2Zinc phosphide1
Reducing
Reducing
HNO3Nitric acid6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Zn(NO3)2Zinc nitrate3
PPhosphorus2
Oxidized
H2Hydrogen3
Reduced

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Liquid
3Zn(NO3)2Crystalline solid + 2PCrystalline solidwhite + 3H2Gas
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
67
per 1 mol of
67
per 1 mol of
11
per 1 mol of
22
per 1 mol of
34
per 1 mol of
22

Changes in standard condition (2)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Liquid
3Zn(NO3)2Crystalline solid + 2PCrystalline solidred, triclinic + 3H2Gas
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
31
per 1 mol of
31
per 1 mol of
5.2
per 1 mol of
10
per 1 mol of
16
per 1 mol of
10

Changes in standard condition (3)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Liquid
3Zn(NO3)2Crystalline solid + 2PCrystalline solidblack + 3H2Gas
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
−12
per 1 mol of
−12
per 1 mol of
−2.0
per 1 mol of
−4.0
per 1 mol of
−6.0
per 1 mol of
−4.0

Changes in standard condition (4)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Liquid
3Zn(NO3)2Crystalline solid + 2PAmorphous solidred + 3H2Gas
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
52
per 1 mol of
52
per 1 mol of
8.7
per 1 mol of
17
per 1 mol of
26
per 1 mol of
17

Changes in aqueous solution (1)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Ionized aqueous solution
3Zn(NO3)2Ionized aqueous solution + 2PCrystalline solidwhite + 3H2Gas
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
11
per 1 mol of
11
per 1 mol of
1.8
per 1 mol of
3.7
per 1 mol of
5.5
per 1 mol of
3.7

Changes in aqueous solution (2)

Reaction of zinc phosphide and nitric acid
Zn3P2Crystalline solid + 6HNO3Ionized aqueous solution
3Zn(NO3)2Ionized aqueous solution + 2PCrystalline solidwhite + 3H2Un-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
−1
per 1 mol of
−1
per 1 mol of
−0.2
per 1 mol of
−0.3
per 1 mol of
−0.5
per 1 mol of
−0.3

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
Zn3P2 (cr)-473[1]
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (l):Liquid, (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
Zn(NO3)2 (cr)-483.7[1]
Zn(NO3)2 (ai)-568.61[1]-369.57[1]180.7[1]-126[1]
Zn(NO3)2 (cr)
1 hydrate
-805.0[1]
Zn(NO3)2 (cr)
2 hydrate
-1110.27[1]
Zn(NO3)2 (cr)
4 hydrate
-1699.12[1]
Zn(NO3)2 (cr)
6 hydrate
-2306.64[1]-1772.71[1]456.9[1]323.0[1]
P (cr)
white
0[1]0[1]41.09[1]23.84[1]
P (cr)
red, triclinic
-17.6[1]-12.1[1]22.80[1]21.21[1]
P (cr)
black
-39.3[1]
P (am)
red
-7.5[1]
P (g)314.64[1]278.25[1]163.193[1]20.786[1]
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (am):Amorphous 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)