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Na2S2O3 + 4HNO3 → 2NaNO3 + 2SO3 + NH4NO3

The reaction of sodium thiosulfate and nitric acid yields sodium nitrate, sulfur trioxide, and ammonium nitrate (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

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2S2O3Sodium thiosulfate1
Reducing
Reducing
HNO3Nitric acid4
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaNO3Sodium nitrate2
SO3Sulfur trioxide2
Oxidized
NH4NO3Ammonium nitrate1
Reduced

Thermodynamic changes

Changes in standard condition

Reaction of sodium thiosulfate and nitric acid
ΔrG−314.5 kJ/mol
K1.25 × 1055
pK−55.10
Na2S2O3Crystalline solid + 4HNO3Liquid
2NaNO3Crystalline solid + 2SO3Liquid + NH4NO3Crystalline 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
−363.9−314.5−166
per 1 mol of
−363.9−314.5−166
per 1 mol of
−90.97−78.63−41.5
per 1 mol of
−181.9−157.3−83.0
per 1 mol of
−181.9−157.3−83.0
per 1 mol of
−363.9−314.5−166

Changes in aqueous solution

Reaction of sodium thiosulfate and nitric acid
ΔrG−194.3 kJ/mol
K1.10 × 1034
pK−34.04
Na2S2O3Ionized aqueous solution + 4HNO3Ionized aqueous solution
2NaNO3Ionized aqueous solution + 2SO3Crystalline solidβ + NH4NO3Ionized 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
−182.01−194.342.3
per 1 mol of
−182.01−194.342.3
per 1 mol of
−45.502−48.5810.6
per 1 mol of
−91.005−97.1521.1
per 1 mol of
−91.005−97.1521.1
per 1 mol of
−182.01−194.342.3

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
Na2S2O3 (cr)-1123.0[1]-1028.0[1]155[1]
Na2S2O3 (ai)-1132.40[1]-1046.0[1]184.1[1]
Na2S2O3 (cr)
5 hydrate
-2607.93[1]-2229.8[1]372[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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
NaNO3 (cr)-467.85[1]-367.00[1]116.52[1]92.88[1]
NaNO3 (ai)-447.48[1]-373.15[1]205.4[1]-40.2[1]
SO3 (cr)
β
-454.51[1]-374.21[1]70.7[1]
SO3 (l)-441.04[1]-373.75[1]113.8[1]
SO3 (g)-395.72[1]-371.06[1]256.76[1]50.67[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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

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)