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  3. 5SnS + 8HNO3 → 5SnO2 + SO2↑ + 4N2O3↑ + 4H2S↑

5SnS + 8HNO3 → 5SnO2 + SO2↑ + 4N2O3↑ + 4H2S↑

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Reaction of tin(II) sulfide and nitric acid
5SnSTin(II) sulfide + 8HNO3Nitric acid
⟶
5SnO2Tin(IV) oxide + SO2↑Sulfur dioxide + 4N2O3↑Dinitrogen trioxide + 4H2S↑Hydrogen sulfide

The reaction of tin(II) sulfide and nitric acid yields tin(IV) oxide, sulfur dioxide, dinitrogen trioxide, and hydrogen sulfide (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 tin(II) sulfide and nitric acid
5SnSTin(II) sulfide + 8HNO3Nitric acid
⟶
5SnO2Tin(IV) oxide + SO2↑Sulfur dioxide + 4N2O3↑Dinitrogen trioxide + 4H2S↑Hydrogen sulfide

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 tin(II) sulfide and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SnSTin(II) sulfide5
Reducing
Reducing
HNO3Nitric acid8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SnO2Tin(IV) oxide5
Oxidized
–
SO2Sulfur dioxide1
Oxidized
–
N2O3Dinitrogen trioxide4
Reduced
–
H2SHydrogen sulfide4
–
–

Thermodynamic changes

Changes in standard condition

Reaction of tin(II) sulfide and nitric acid
◆
ΔrG−1337.4 kJ/mol
K2.01 × 10234
pK−234.30
5SnSCrystalline solid + 8HNO3Liquid
⟶
5SnO2Crystalline solid + SO2↑Gas + 4N2O3↑Gas + 4H2S↑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
−1055−1337.4952.2−423.03
per 1 mol of
−211.0−267.48190.4−84.606
per 1 mol of
−131.9−167.18119.0−52.879
per 1 mol of
−211.0−267.48190.4−84.606
per 1 mol of
−1055−1337.4952.2−423.03
−263.8−334.35238.1−105.76
per 1 mol of
−263.8−334.35238.1−105.76

Changes in aqueous solution (1)

Reaction of tin(II) sulfide and nitric acid
◆
ΔrG−1093.1 kJ/mol
K3.18 × 10191
pK−191.50
5SnSCrystalline solid + 8HNO3Ionized aqueous solution
⟶
5SnO2Crystalline solid + SO2↑Gas + 4N2O3↑Gas + 4H2S↑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
−789−1093.11025.81148.7
per 1 mol of
−158−218.62205.16229.74
per 1 mol of
−98.6−136.64128.22143.59
per 1 mol of
−158−218.62205.16229.74
per 1 mol of
−789−1093.11025.81148.7
−197−273.27256.45287.18
per 1 mol of
−197−273.27256.45287.18

Changes in aqueous solution (2)

Reaction of tin(II) sulfide and nitric acid
◆
ΔrG−1070.2 kJ/mol
K3.10 × 10187
pK−187.49
5SnSCrystalline solid + 8HNO3Ionized aqueous solution
⟶
5SnO2Crystalline solid + SO2↑Gas + 4N2O3↑Gas + 4H2S↑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
−865−1070.2687–
per 1 mol of
−173−214.04137–
per 1 mol of
−108−133.7885.9–
per 1 mol of
−173−214.04137–
per 1 mol of
−865−1070.2687–
−216−267.55172–
per 1 mol of
−216−267.55172–

Changes in aqueous solution (3)

Reaction of tin(II) sulfide and nitric acid
◆
ΔrG−1093.6 kJ/mol
K3.89 × 10191
pK−191.59
5SnSCrystalline solid + 8HNO3Ionized aqueous solution
⟶
5SnO2Crystalline solid + SO2↑Un-ionized aqueous solution + 4N2O3↑Gas + 4H2S↑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
−815−1093.6939.5–
per 1 mol of
−163−218.72187.9–
per 1 mol of
−102−136.70117.4–
per 1 mol of
−163−218.72187.9–
per 1 mol of
−815−1093.6939.5–
−204−273.40234.9–
per 1 mol of
−204−273.40234.9–

Changes in aqueous solution (4)

Reaction of tin(II) sulfide and nitric acid
◆
ΔrG−1070.7 kJ/mol
K3.79 × 10187
pK−187.58
5SnSCrystalline solid + 8HNO3Ionized aqueous solution
⟶
5SnO2Crystalline solid + SO2↑Un-ionized aqueous solution + 4N2O3↑Gas + 4H2S↑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
−892−1070.7600–
per 1 mol of
−178−214.14120–
per 1 mol of
−112−133.8475.0–
per 1 mol of
−178−214.14120–
per 1 mol of
−892−1070.7600–
−223−267.68150–
per 1 mol of
−223−267.68150–

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
SnS (cr)-100[1]-98.3[1]77.0[1]49.25[1]
SnS (g)119.2[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, (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
SnO2 (cr)-580.7[1]-519.6[1]52.3[1]52.59[1]
SO2 (l)-320.5[1]–––
SO2 (g)-296.830[1]-300.194[1]248.22[1]39.87[1]
SO2 (ao)-322.980[1]-300.676[1]161.9[1]–
N2O3 (l)50.29[1]–––
N2O3 (g)83.72[1]139.46[1]312.28[1]65.61[1]
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]–
* (cr):Crystalline solid, (l):Liquid, (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)