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2Sn + H2SO4 → 2SnO2 + S + H2↑

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Reaction of tin and sulfuric acid
2SnTin + H2SO4Sulfuric acid
⟶
2SnO2Tin(IV) oxide + SSulfur + H2↑Hydrogen

The reaction of tin and sulfuric acid yields tin(IV) oxide, sulfur, 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

Reaction of tin and sulfuric acid
2SnTin + H2SO4Sulfuric acid
⟶
2SnO2Tin(IV) oxide + SSulfur + H2↑Hydrogen

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 tin and sulfuric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SnTin2
Reducing
Reducing
H2SO4Sulfuric acid1
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
SnO2Tin(IV) oxide2
Oxidized
–
SSulfur1
Reduced
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of tin and sulfuric acid
◆
ΔrG−349.2 kJ/mol
K1.50 × 1061
pK−61.18
2SnCrystalline solidwhite + H2SO4Liquid
⟶
2SnO2Crystalline solid + SCrystalline solidrhombic + H2↑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
−347.4−349.27.1−36.25
per 1 mol of
−173.7−174.63.5−18.13
per 1 mol of
−347.4−349.27.1−36.25
per 1 mol of
−173.7−174.63.5−18.13
per 1 mol of
−347.4−349.27.1−36.25
per 1 mol of
−347.4−349.27.1−36.25

Changes in standard condition (2)

Reaction of tin and sulfuric acid
2SnCrystalline solidwhite + H2SO4Liquid
⟶
2SnO2Crystalline solid + SCrystalline solidmonoclinic + H2↑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
−347.1–––
per 1 mol of
−173.6–––
per 1 mol of
−347.1–––
per 1 mol of
−173.6–––
per 1 mol of
−347.1–––
per 1 mol of
−347.1–––

Changes in standard condition (3)

Reaction of tin and sulfuric acid
◆
ΔrG−349.5 kJ/mol
K1.70 × 1061
pK−61.23
2SnCrystalline solidgray + H2SO4Liquid
⟶
2SnO2Crystalline solid + SCrystalline solidrhombic + H2↑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
−343.2−349.521.9−33.81
per 1 mol of
−171.6−174.810.9−16.91
per 1 mol of
−343.2−349.521.9−33.81
per 1 mol of
−171.6−174.810.9−16.91
per 1 mol of
−343.2−349.521.9−33.81
per 1 mol of
−343.2−349.521.9−33.81

Changes in standard condition (4)

Reaction of tin and sulfuric acid
2SnCrystalline solidgray + H2SO4Liquid
⟶
2SnO2Crystalline solid + SCrystalline solidmonoclinic + H2↑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
−342.9–––
per 1 mol of
−171.4–––
per 1 mol of
−342.9–––
per 1 mol of
−171.4–––
per 1 mol of
−342.9–––
per 1 mol of
−342.9–––

Changes in aqueous solution (1)

Reaction of tin and sulfuric acid
◆
ΔrG−294.7 kJ/mol
K4.26 × 1051
pK−51.63
2SnCrystalline solidwhite + H2SO4Ionized aqueous solution
⟶
2SnO2Crystalline solid + SCrystalline solidrhombic + H2↑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
−252.1−294.7143.9396
per 1 mol of
−126.0−147.371.95198
per 1 mol of
−252.1−294.7143.9396
per 1 mol of
−126.0−147.371.95198
per 1 mol of
−252.1−294.7143.9396
per 1 mol of
−252.1−294.7143.9396

Changes in aqueous solution (2)

Reaction of tin and sulfuric acid
◆
ΔrG−277.1 kJ/mol
K3.51 × 1048
pK−48.55
2SnCrystalline solidwhite + H2SO4Ionized aqueous solution
⟶
2SnO2Crystalline solid + SCrystalline solidrhombic + H2↑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
−256.3−277.1590–
per 1 mol of
−128.2−138.6295–
per 1 mol of
−256.3−277.1590–
per 1 mol of
−128.2−138.6295–
per 1 mol of
−256.3−277.1590–
per 1 mol of
−256.3−277.1590–

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
Sn (cr)
white
0[1]0[1]51.55[1]26.99[1]
Sn (cr)
gray
-2.09[1]0.13[1]44.14[1]25.77[1]
Sn (g)302.1[1]267.3[1]168.486[1]21.259[1]
H2SO4 (cr)––––
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[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]
S (cr)
rhombic
0[1]0[1]31.80[1]22.64[1]
S (cr)
monoclinic
0.33[1]–––
S (g)278.805[1]238.250[1]167.821[1]23.673[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, (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)