H2 + PbBr2 🔥→ Pb + 2HBr
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- Reaction of and lead(II) bromide
The reaction of and lead(II) bromide yields and hydrogen bromide. This reaction is an oxidation-reduction reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of and lead(II) bromide
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 and lead(II) bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reducing | Reducing | ||
| PbBr2 | Lead(II) bromide | 1 | Oxidizing | Reducible |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| 1 | Reduced | – | ||
| HBr | Hydrogen bromide | 2 | Oxidized | – |
Thermodynamic changes
Changes in standard condition
- Reaction of and lead(II) bromide◆
ΔrG 155.02 kJ/mol K 0.69 × 10−27 pK 27.16
| 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 | 205.9 | 155.02 | 170.0 | −24.22 |
| 205.9 | 155.02 | 170.0 | −24.22 | |
per 1 mol of | 205.9 | 155.02 | 170.0 | −24.22 |
| 205.9 | 155.02 | 170.0 | −24.22 | |
per 1 mol of | 103.0 | 77.510 | 85.00 | −12.11 |
Changes in aqueous solution (1)
- Reaction of and lead(II) bromide◆
ΔrG 107.8 kJ/mol K 0.13 × 10−18 pK 18.89
| 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 | 176.2 | 107.8 | −290 | – |
| 176.2 | 107.8 | −290 | – | |
per 1 mol of | 176.2 | 107.8 | −290 | – |
| 176.2 | 107.8 | −290 | – | |
per 1 mol of | 88.10 | 53.90 | −145 | – |
Changes in aqueous solution (2)
- Reaction of and lead(II) bromide◆
ΔrG 6.8 kJ/mol K 0.64 × 10−1 pK 1.19
| 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 | 5.9 | 6.8 | −523 | – |
| 5.9 | 6.8 | −523 | – | |
per 1 mol of | 5.9 | 6.8 | −523 | – |
| 5.9 | 6.8 | −523 | – | |
per 1 mol of | 3.0 | 3.4 | −262 | – |
Changes in aqueous solution (3)
- Reaction of and lead(II) bromide◆
ΔrG 116.1 kJ/mol K 0.46 × 10−20 pK 20.34
| 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 | – | 116.1 | – | – |
| – | 116.1 | – | – | |
per 1 mol of | – | 116.1 | – | – |
| – | 116.1 | – | – | |
per 1 mol of | – | 58.05 | – | – |
Changes in aqueous solution (4)
- Reaction of and lead(II) bromide◆
ΔrG 15.1 kJ/mol K 0.23 × 10−2 pK 2.65
| 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 | – | 15.1 | – | – |
| – | 15.1 | – | – | |
per 1 mol of | – | 15.1 | – | – |
| – | 15.1 | – | – | |
per 1 mol of | – | 7.55 | – | – |
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 |
|---|---|---|---|---|
| (g) | 0[1] | 0[1] | 130.684[1] | 28.824[1] |
| (ao) | -4.2[1] | 17.6[1] | 577[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] | – | – |
* (g):Gas, (ao):Un-ionized aqueous solution, (cr):Crystalline solid, (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 |
|---|---|---|---|---|
| (cr) | 0[1] | 0[1] | 64.81[1] | 26.44[1] |
| (g) | 195.0[1] | 161.9[1] | 175.373[1] | 20.786[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, (g):Gas, (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°, 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
- ^ 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°, 0 kJ · mol−1
- ^ ΔfG°, 0 kJ · mol−1
- ^ S°, 64.81 J · K−1 · mol−1
- ^ Cp°, 26.44 J · K−1 · mol−1
- ^ ΔfH°, 195.0 kJ · mol−1
- ^ ΔfG°, 161.9 kJ · mol−1
- ^ S°, 175.373 J · K−1 · mol−1
- ^ Cp°, 20.786 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