3PbS + 2HNO3 → 3PbO2 + 3S + N2↑ + H2↑
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- Reaction of lead(II) sulfide and nitric acid
The reaction of lead(II) sulfide and nitric acid yields lead(IV) oxide, , , and (Other reactions are here). This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) sulfide and nitric acid
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 lead(II) sulfide and nitric acid
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbS | Lead(II) sulfide | 3 | Reducing | Reducing |
HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbO2 | Lead(IV) oxide | 3 | Oxidized | – |
3 | Oxidized | – | ||
1 | Reduced | – | ||
1 | Reduced | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of lead(II) sulfide and nitric acid◆
ΔrG −194.5 kJ/mol K 1.19 × 1034 pK −34.07
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 | −182.8 | −194.5 | 38.7 | −48.45 |
per 1 mol of | −60.93 | −64.83 | 12.9 | −16.15 |
per 1 mol of | −91.40 | −97.25 | 19.4 | −24.23 |
per 1 mol of | −60.93 | −64.83 | 12.9 | −16.15 |
−60.93 | −64.83 | 12.9 | −16.15 | |
−182.8 | −194.5 | 38.7 | −48.45 | |
−182.8 | −194.5 | 38.7 | −48.45 |
Changes in standard condition (2)
- Reaction of lead(II) sulfide and nitric acid
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 | −181.8 | – | – | – |
per 1 mol of | −60.60 | – | – | – |
per 1 mol of | −90.90 | – | – | – |
per 1 mol of | −60.60 | – | – | – |
−60.60 | – | – | – | |
−181.8 | – | – | – | |
−181.8 | – | – | – |
Changes in aqueous solution (1)
- Reaction of lead(II) sulfide and nitric acid◆
ΔrG −133.4 kJ/mol K 2.35 × 1023 pK −23.37
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 | −116.3 | −133.4 | 57.1 | 344.5 |
per 1 mol of | −38.77 | −44.47 | 19.0 | 114.8 |
per 1 mol of | −58.15 | −66.70 | 28.6 | 172.3 |
per 1 mol of | −38.77 | −44.47 | 19.0 | 114.8 |
−38.77 | −44.47 | 19.0 | 114.8 | |
−116.3 | −133.4 | 57.1 | 344.5 | |
−116.3 | −133.4 | 57.1 | 344.5 |
Changes in aqueous solution (2)
- Reaction of lead(II) sulfide and nitric acid◆
ΔrG −115.8 kJ/mol K 1.94 × 1020 pK −20.29
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 | −120.5 | −115.8 | 503 | – |
per 1 mol of | −40.17 | −38.60 | 168 | – |
per 1 mol of | −60.25 | −57.90 | 252 | – |
per 1 mol of | −40.17 | −38.60 | 168 | – |
−40.17 | −38.60 | 168 | – | |
−120.5 | −115.8 | 503 | – | |
−120.5 | −115.8 | 503 | – |
Thermodynamic data of reactants
Chemical formula | Standard 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 |
---|---|---|---|---|
PbS (cr) | -100.4[1] | -98.7[1] | 91.2[1] | 49.50[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, (l):Liquid, (g):Gas, (ai):Ionized aqueous solution
Thermodynamic data of products
Chemical formula | Standard 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 |
---|---|---|---|---|
PbO2 (cr) | -277.4[1] | -217.33[1] | 68.6[1] | 64.64[1] |
(cr) rhombic | 0[1] | 0[1] | 31.80[1] | 22.64[1] |
(cr) monoclinic | 0.33[1] | – | – | – |
(g) | 278.805[1] | 238.250[1] | 167.821[1] | 23.673[1] |
(g) | 0[1] | 0[1] | 191.61[1] | 29.125[1] |
(g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
(ao) | -4.2[1] | 17.6[1] | 577[1] | – |
* (cr):Crystalline solid, (g):Gas, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -100.4 kJ · mol−1
- ^ ΔfG°, -98.7 kJ · mol−1
- ^ S°, 91.2 J · K−1 · mol−1
- ^ Cp°, 49.50 J · K−1 · mol−1
- ^ ΔfH°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 J · K−1 · mol−1
- ^ ΔfH°, -277.4 kJ · mol−1
- ^ ΔfG°, -217.33 kJ · mol−1
- ^ S°, 68.6 J · K−1 · mol−1
- ^ Cp°, 64.64 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 31.80 J · K−1 · mol−1
- ^ Cp°, 22.64 J · K−1 · mol−1
- ^ ΔfH°, 0.33 kJ · mol−1
- ^ ΔfH°, 278.805 kJ · mol−1
- ^ ΔfG°, 238.250 kJ · mol−1
- ^ S°, 167.821 J · K−1 · mol−1
- ^ Cp°, 23.673 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 191.61 J · K−1 · mol−1
- ^ Cp°, 29.125 J · K−1 · mol−1
- ^ ΔfH°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 130.684 J · K−1 · mol−1
- ^ Cp°, 28.824 J · K−1 · mol−1
- ^ ΔfH°, -4.2 kJ · mol−1
- ^ ΔfG°, 17.6 kJ · mol−1
- ^ S°, 577 J · K−1 · mol−1