2PbBr2 + 2HNO3 🔥→ 2PbO2 + Br2 + 2NO↑ + 2HBr↑
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- Reaction of lead(II) bromide and nitric acid
The reaction of lead(II) bromide and nitric acid yields lead(IV) oxide, , nitrogen monoxide, and hydrogen bromide (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) bromide and nitric acid
General equation
- Reaction of hardly oxidizable species and oxidizing species
- Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent ⟶ ProductOxidation product + ProductReduction product
Oxidation state of each atom
- Reaction of lead(II) bromide and nitric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbBr2 | Lead(II) bromide | 2 | Reducing | Hardly oxidizable |
| HNO3 | Nitric acid | 2 | Oxidizing | Oxidizing |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| PbO2 | Lead(IV) oxide | 2 | Oxidized | – |
| 1 | Oxidized | – | ||
| NO | Nitrogen monoxide | 2 | Reduced | – |
| HBr | Hydrogen bromide | 2 | – | – |
Thermodynamic changes
Changes in standard condition
- Reaction of lead(II) bromide and nitric acid◆
ΔrG 316.80 kJ/mol K 0.32 × 10−55 pK 55.50
| 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 | 458.5 | 316.80 | 474.1 | −57.04 |
per 1 mol of | 229.3 | 158.40 | 237.1 | −28.52 |
per 1 mol of | 229.3 | 158.40 | 237.1 | −28.52 |
per 1 mol of | 229.3 | 158.40 | 237.1 | −28.52 |
| 458.5 | 316.80 | 474.1 | −57.04 | |
per 1 mol of | 229.3 | 158.40 | 237.1 | −28.52 |
per 1 mol of | 229.3 | 158.40 | 237.1 | −28.52 |
Changes in aqueous solution (1)
- Reaction of lead(II) bromide and nitric acid◆
ΔrG 322.65 kJ/mol K 0.30 × 10−56 pK 56.53
| 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 | 454.6 | 322.65 | 443.2 | – |
per 1 mol of | 227.3 | 161.32 | 221.6 | – |
per 1 mol of | 227.3 | 161.32 | 221.6 | – |
per 1 mol of | 227.3 | 161.32 | 221.6 | – |
| 454.6 | 322.65 | 443.2 | – | |
per 1 mol of | 227.3 | 161.32 | 221.6 | – |
per 1 mol of | 227.3 | 161.32 | 221.6 | – |
Changes in aqueous solution (2)
- Reaction of lead(II) bromide and nitric acid◆
ΔrG 221.63 kJ/mol K 0.15 × 10−38 pK 38.83
| 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 | 284.3 | 221.63 | 210.6 | – |
per 1 mol of | 142.2 | 110.81 | 105.3 | – |
per 1 mol of | 142.2 | 110.81 | 105.3 | – |
per 1 mol of | 142.2 | 110.81 | 105.3 | – |
| 284.3 | 221.63 | 210.6 | – | |
per 1 mol of | 142.2 | 110.81 | 105.3 | – |
per 1 mol of | 142.2 | 110.81 | 105.3 | – |
Changes in aqueous solution (3)
- Reaction of lead(II) bromide and nitric acid◆
ΔrG 339.2 kJ/mol K 0.38 × 10−59 pK 59.43
| 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 | – | 339.2 | – | – |
per 1 mol of | – | 169.6 | – | – |
per 1 mol of | – | 169.6 | – | – |
per 1 mol of | – | 169.6 | – | – |
| – | 339.2 | – | – | |
per 1 mol of | – | 169.6 | – | – |
per 1 mol of | – | 169.6 | – | – |
Changes in aqueous solution (4)
- Reaction of lead(II) bromide and nitric acid◆
ΔrG 238.2 kJ/mol K 0.19 × 10−41 pK 41.73
| 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 | – | 238.2 | – | – |
per 1 mol of | – | 119.1 | – | – |
per 1 mol of | – | 119.1 | – | – |
per 1 mol of | – | 119.1 | – | – |
| – | 238.2 | – | – | |
per 1 mol of | – | 119.1 | – | – |
per 1 mol of | – | 119.1 | – | – |
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 |
|---|---|---|---|---|
| PbBr2 (cr) | -278.7[1] | -261.92[1] | 161.5[1] | 80.12[1] |
| PbBr2 (ai) | -244.8[1] | -232.34[1] | 175.3[1] | – |
| PbBr2 (ao) | – | -240.6[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, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas
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) | – | – | – | – |
| (l) | 0[1] | 0[1] | 152.231[1] | 75.689[1] |
| (g) | 30.907[1] | 3.110[1] | 245.463[1] | 36.02[1] |
| (ao) | -2.59[1] | 3.93[1] | 130.5[1] | – |
| NO (g) | 90.25[1] | 86.55[1] | 210.761[1] | 29.844[1] |
| HBr (g) | -36.40[1] | -53.45[1] | 198.695[1] | 29.142[1] |
| HBr (ai) | -121.55[1] | -103.96[1] | 82.4[1] | -141.8[1] |
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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°, -278.7 kJ · mol−1
- ^ ΔfG°, -261.92 kJ · mol−1
- ^ S°, 161.5 J · K−1 · mol−1
- ^ Cp°, 80.12 J · K−1 · mol−1
- ^ ΔfH°, -244.8 kJ · mol−1
- ^ ΔfG°, -232.34 kJ · mol−1
- ^ S°, 175.3 J · K−1 · mol−1
- ^ ΔfG°, -240.6 kJ · 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°, 152.231 J · K−1 · mol−1
- ^ Cp°, 75.689 J · K−1 · mol−1
- ^ ΔfH°, 30.907 kJ · mol−1
- ^ ΔfG°, 3.110 kJ · mol−1
- ^ S°, 245.463 J · K−1 · mol−1
- ^ Cp°, 36.02 J · K−1 · mol−1
- ^ ΔfH°, -2.59 kJ · mol−1
- ^ ΔfG°, 3.93 kJ · mol−1
- ^ S°, 130.5 J · K−1 · mol−1
- ^ ΔfH°, 90.25 kJ · mol−1
- ^ ΔfG°, 86.55 kJ · mol−1
- ^ S°, 210.761 J · K−1 · mol−1
- ^ Cp°, 29.844 J · K−1 · mol−1
- ^ ΔfH°, -36.40 kJ · mol−1
- ^ ΔfG°, -53.45 kJ · mol−1
- ^ S°, 198.695 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -121.55 kJ · mol−1
- ^ ΔfG°, -103.96 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, -141.8 J · K−1 · mol−1