BaCO3 + 2HBr → BaBr2 + CO2 + H2O
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The reaction of barium carbonate and hydrogen bromide yields barium 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 barium carbonate 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 barium carbonate and hydrogen bromide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaCO3 | Barium carbonate | 1 | Brønsted base | Salt of weak acid |
HBr | Hydrogen bromide | 2 | Brønsted acid | Strong acid |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
BaBr2 | Barium bromide | 1 | Conjugate base | Salt of strong acid |
CO2 | Carbon dioxide | 1 | – | Acidic oxide |
H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of barium carbonate and hydrogen bromide◆
ΔrG −123.8 kJ/mol K 4.88 × 1021 pK −21.69
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 | −147.5 | −123.8 | −80 | – |
per 1 mol of | −147.5 | −123.8 | −80 | – |
per 1 mol of | −73.75 | −61.90 | −40 | – |
per 1 mol of | −147.5 | −123.8 | −80 | – |
per 1 mol of | −147.5 | −123.8 | −80 | – |
per 1 mol of | −147.5 | −123.8 | −80 | – |
Changes in aqueous solution (1)
- Reaction of barium carbonate and hydrogen bromide◆
ΔrG −54.6 kJ/mol K 3.68 × 109 pK −9.57
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 | −0.7 | −54.6 | 181.3 | – |
per 1 mol of | −0.70 | −54.6 | 181.3 | – |
per 1 mol of | −0.35 | −27.3 | 90.65 | – |
per 1 mol of | −0.70 | −54.6 | 181.3 | – |
per 1 mol of | −0.70 | −54.6 | 181.3 | – |
per 1 mol of | −0.70 | −54.6 | 181.3 | – |
Changes in aqueous solution (2)
- Reaction of barium carbonate and hydrogen bromide◆
ΔrG −46.3 kJ/mol K 1.29 × 108 pK −8.11
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 | −21.0 | −46.3 | 85.1 | – |
per 1 mol of | −21.0 | −46.3 | 85.1 | – |
per 1 mol of | −10.5 | −23.1 | 42.5 | – |
per 1 mol of | −21.0 | −46.3 | 85.1 | – |
per 1 mol of | −21.0 | −46.3 | 85.1 | – |
per 1 mol of | −21.0 | −46.3 | 85.1 | – |
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 |
---|---|---|---|---|
BaCO3 (cr) | -1216.3[1] | -1137.6[1] | 112.1[1] | 85.35[1] |
BaCO3 (ai) | -1214.78[1] | -1088.59[1] | -47.3[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, (ai):Ionized aqueous solution, (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 |
---|---|---|---|---|
BaBr2 (cr) | -757.3[1] | -736.8[1] | 146[1] | – |
BaBr2 (g) | -439[1] | -473[1] | 331[1] | 61.5[1] |
BaBr2 (ai) | -780.73[1] | -768.68[1] | 174.5[1] | – |
BaBr2 (cr) 1 hydrate | -1068.2[1] | – | – | – |
BaBr2 (cr) 2 hydrate | -1366.1[1] | -1230.4[1] | 226[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°, -1216.3 kJ · mol−1
- ^ ΔfG°, -1137.6 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 85.35 J · K−1 · mol−1
- ^ ΔfH°, -1214.78 kJ · mol−1
- ^ ΔfG°, -1088.59 kJ · mol−1
- ^ S°, -47.3 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
- ^ ΔfH°, -757.3 kJ · mol−1
- ^ ΔfG°, -736.8 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -439. kJ · mol−1
- ^ ΔfG°, -473. kJ · mol−1
- ^ S°, 331. J · K−1 · mol−1
- ^ Cp°, 61.5 J · K−1 · mol−1
- ^ ΔfH°, -780.73 kJ · mol−1
- ^ ΔfG°, -768.68 kJ · mol−1
- ^ S°, 174.5 J · K−1 · mol−1
- ^ ΔfH°, -1068.2 kJ · mol−1
- ^ ΔfH°, -1366.1 kJ · mol−1
- ^ ΔfG°, -1230.4 kJ · mol−1
- ^ S°, 226. 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