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2B2H6 + 6HNO3 → 2B2O3 + 3NH4NO3 + 3H2O

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Reaction of diborane(6) and nitric acid
2B2H6Diborane(6) + 6HNO3Nitric acid
⟶
2B2O3Diboron trioxide + 3NH4NO3Ammonium nitrate + 3H2OWater

The reaction of diborane(6) and nitric acid yields diboron trioxide, ammonium nitrate, and water (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 diborane(6) and nitric acid
2B2H6Diborane(6) + 6HNO3Nitric acid
⟶
2B2O3Diboron trioxide + 3NH4NO3Ammonium nitrate + 3H2OWater

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 diborane(6) and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
B2H6Diborane(6)2
Reducing
Reducing
HNO3Nitric acid6
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
B2O3Diboron trioxide2
Oxidized
–
NH4NO3Ammonium nitrate3
Reduced
–
H2OWater3
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of diborane(6) and nitric acid
◆
ΔrG−3339.4 kJ/mol
K1.09 × 10585
pK−585.04
2B2H6Gas + 6HNO3Liquid
⟶
2B2O3Crystalline solid + 3NH4NO3Crystalline solid + 3H2OLiquid
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
−3526.3−3339.4−626.91−3.4
per 1 mol of
−1763.2−1669.7−313.45−1.7
per 1 mol of
−587.72−556.57−104.48−0.57
per 1 mol of
−1763.2−1669.7−313.45−1.7
per 1 mol of
−1175.4−1113.1−208.97−1.1
per 1 mol of
−1175.4−1113.1−208.97−1.1

Changes in standard condition (2)

Reaction of diborane(6) and nitric acid
◆
ΔrG−3316.7 kJ/mol
K1.15 × 10581
pK−581.06
2B2H6Gas + 6HNO3Liquid
⟶
2B2O3Amorphous solid + 3NH4NO3Crystalline solid + 3H2OLiquid
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
−3489.8−3316.7−579.3−7.0
per 1 mol of
−1744.9−1658.3−289.6−3.5
per 1 mol of
−581.63−552.78−96.55−1.2
per 1 mol of
−1744.9−1658.3−289.6−3.5
per 1 mol of
−1163.3−1105.6−193.1−2.3
per 1 mol of
−1163.3−1105.6−193.1−2.3

Changes in aqueous solution

Reaction of diborane(6) and nitric acid
◆
ΔrG−3176.3 kJ/mol
K2.91 × 10556
pK−556.46
2B2H6Gas + 6HNO3Ionized aqueous solution
⟶
2B2O3Crystalline solid + 3NH4NO3Ionized aqueous solution + 3H2OLiquid
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
−3249.7−3176.3−245.6737.4
per 1 mol of
−1624.8−1588.2−122.8368.7
per 1 mol of
−541.62−529.38−40.93122.9
per 1 mol of
−1624.8−1588.2−122.8368.7
per 1 mol of
−1083.2−1058.8−81.87245.8
per 1 mol of
−1083.2−1058.8−81.87245.8

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
B2H6 (g)35.6[1]86.7[1]232.11[1]56.90[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]
* (g):Gas, (l):Liquid, (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
B2O3 (cr)-1272.77[1]-1193.65[1]53.97[1]62.93[1]
B2O3 (am)-1254.53[1]-1182.3[1]77.8[1]61.1[1]
B2O3 (g)-843.79[1]-831.97[1]279.81[1]66.86[1]
NH4NO3 (cr)-365.56[1]-183.87[1]151.08[1]139.3[1]
NH4NO3 (ai)-339.87[1]-190.56[1]259.8[1]-6.7[1]
H2O (cr)––––
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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)