LiHCO3 + HBr → LiBr + CO2 + H2O
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The reaction of lithium hydrogencarbonate and hydrogen bromide yields lithium bromide, carbon dioxide, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lithium hydrogencarbonate and hydrogen bromide
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of lithium hydrogencarbonate and hydrogen bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiHCO3 | Lithium hydrogencarbonate | 1 | Brønsted base | Salt of weak acid |
| HBr | Hydrogen bromide | 1 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| LiBr | Lithium bromide | 1 | Conjugate base | Salt of strong acid |
| CO2 | Carbon dioxide | 1 | – | Acidic oxide |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
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 |
|---|---|---|---|---|
| LiHCO3 | – | – | – | – |
| 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] |
* (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 |
|---|---|---|---|---|
| LiBr (cr) | -351.213[1] | -342.00[1] | 74.27[1] | – |
| LiBr (g) | – | – | 224.33[1] | 33.93[1] |
| LiBr (ai) | -400.041[1] | -397.27[1] | 95.8[1] | -73.2[1] |
| LiBr (cr) 1 hydrate | -662.58[1] | -594.29[1] | 109.6[1] | – |
| LiBr (cr) 2 hydrate | -962.7[1] | -840.5[1] | 162.3[1] | – |
| CO2 (g) | -393.509[1] | -394.359[1] | 213.74[1] | 37.11[1] |
| CO2 (ao) | -413.80[1] | -385.98[1] | 117.6[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, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid
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°, -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
- ^ ΔfH°, -351.213 kJ · mol−1
- ^ ΔfG°, -342.00 kJ · mol−1
- ^ S°, 74.27 J · K−1 · mol−1
- ^ S°, 224.33 J · K−1 · mol−1
- ^ Cp°, 33.93 J · K−1 · mol−1
- ^ ΔfH°, -400.041 kJ · mol−1
- ^ ΔfG°, -397.27 kJ · mol−1
- ^ S°, 95.8 J · K−1 · mol−1
- ^ Cp°, -73.2 J · K−1 · mol−1
- ^ ΔfH°, -662.58 kJ · mol−1
- ^ ΔfG°, -594.29 kJ · mol−1
- ^ S°, 109.6 J · K−1 · mol−1
- ^ ΔfH°, -962.7 kJ · mol−1
- ^ ΔfG°, -840.5 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, -393.509 kJ · mol−1
- ^ ΔfG°, -394.359 kJ · mol−1
- ^ S°, 213.74 J · K−1 · mol−1
- ^ Cp°, 37.11 J · K−1 · mol−1
- ^ ΔfH°, -413.80 kJ · mol−1
- ^ ΔfG°, -385.98 kJ · mol−1
- ^ S°, 117.6 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1