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2Ag + 2H2SO4 🔥→ Ag2SO4 + SO2↑ + 2H2O

The reaction of silver and sulfuric acid yields silver(I) sulfate, sulfur dioxide, 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

General equation

Reaction of oxidizable species and reducible species
Oxidizable speciesReducing agent + Reducible speciesOxidizing agent
🔥
ProductOxidation product + ProductReduction product
Reaction of inactive metal and oxidizing acid
Inactive metalReducing agent + Oxidizing acidOxidizing agent
SaltOxidation product + Acidic oxide/Neutral oxideReduction product + H2O

Oxidation state of each atom

Reaction of silver and sulfuric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
AgSilver2
Reducing
Oxidizable
Inactive metal
H2SO4Sulfuric acid2
Oxidizing
Reducible
Oxidizing acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ag2SO4Silver(I) sulfate1
Oxidized
Salt
SO2Sulfur dioxide1
Reduced
Acidic oxide
H2OWater2
Water

Thermodynamic changes

Changes in standard condition

Reaction of silver and sulfuric acid
ΔrG−12.86 kJ/mol
K1.79 × 102
pK−2.25
2AgCrystalline solid + 2H2SO4Liquid
🔥
Ag2SO4Crystalline solid + SO2Gas + 2H2OLiquid
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
43.61−12.86189.5−6.69
per 1 mol of
21.80−6.43094.75−3.35
per 1 mol of
21.80−6.43094.75−3.35
per 1 mol of
43.61−12.86189.5−6.69
per 1 mol of
43.61−12.86189.5−6.69
per 1 mol of
21.80−6.43094.75−3.35

Changes in aqueous solution (1)

Reaction of silver and sulfuric acid
ΔrG124.31 kJ/mol
K0.17 × 10−21
pK21.78
2AgCrystalline solid + 2H2SO4Ionized aqueous solution
🔥
Ag2SO4Ionized aqueous solution + SO2Gas + 2H2OLiquid
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
251.95124.31428.4475
per 1 mol of
125.9762.155214.2238
per 1 mol of
125.9762.155214.2238
per 1 mol of
251.95124.31428.4475
per 1 mol of
251.95124.31428.4475
per 1 mol of
125.9762.155214.2238

Changes in aqueous solution (2)

Reaction of silver and sulfuric acid
ΔrG123.83 kJ/mol
K0.20 × 10−21
pK21.69
2AgCrystalline solid + 2H2SO4Ionized aqueous solution
🔥
Ag2SO4Ionized aqueous solution + SO2Un-ionized aqueous solution + 2H2OLiquid
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
225.80123.83342.1
per 1 mol of
112.9061.915171.1
per 1 mol of
112.9061.915171.1
per 1 mol of
225.80123.83342.1
per 1 mol of
225.80123.83342.1
per 1 mol of
112.9061.915171.1

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
Ag (cr)0[1]0[1]42.55[1]25.351[1]
Ag (g)284.55[1]245.65[1]172.997[1]20.786[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
Ag2SO4 (cr)-715.88[1]-618.41[1]200.4[1]131.38[1]
Ag2SO4 (ai)-698.10[1]-590.30[1]165.7[1]-251[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]
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, (ai):Ionized aqueous solution, (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)