K2SO3 + 2HBr → 2KBr + SO2 + H2O
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The reaction of potassium sulfite and hydrogen bromide yields potassium bromide, sulfur 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 potassium sulfite 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 potassium sulfite and hydrogen bromide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
K2SO3 | Potassium sulfite | 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 |
---|---|---|---|---|
KBr | Potassium bromide | 2 | Conjugate base | Salt of strong acid |
SO2 | Sulfur dioxide | 1 | – | Acidic oxide |
H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium sulfite and hydrogen bromide
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 | −172.0 | – | – | – |
per 1 mol of | −172.0 | – | – | – |
per 1 mol of | −86.00 | – | – | – |
per 1 mol of | −86.00 | – | – | – |
per 1 mol of | −172.0 | – | – | – |
per 1 mol of | −172.0 | – | – | – |
Changes in aqueous solution (1)
- Reaction of potassium sulfite and hydrogen bromide◆
ΔrG −50.8 kJ/mol K 7.94 × 108 pK −8.90
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 | 52.7 | −50.8 | 347 | – |
per 1 mol of | 52.7 | −50.8 | 347 | – |
per 1 mol of | 26.4 | −25.4 | 174 | – |
per 1 mol of | 26.4 | −25.4 | 174 | – |
per 1 mol of | 52.7 | −50.8 | 347 | – |
per 1 mol of | 52.7 | −50.8 | 347 | – |
Changes in aqueous solution (2)
- Reaction of potassium sulfite and hydrogen bromide◆
ΔrG −51.2 kJ/mol K 9.33 × 108 pK −8.97
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 | 26.5 | −51.2 | 261 | – |
per 1 mol of | 26.5 | −51.2 | 261 | – |
per 1 mol of | 13.3 | −25.6 | 131 | – |
per 1 mol of | 13.3 | −25.6 | 131 | – |
per 1 mol of | 26.5 | −51.2 | 261 | – |
per 1 mol of | 26.5 | −51.2 | 261 | – |
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 |
---|---|---|---|---|
K2SO3 (cr) | -1125.5[1] | – | – | – |
K2SO3 (ai) | -1140.1[1] | -1053.1[1] | 176[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 |
---|---|---|---|---|
KBr (cr) | -393.798[1] | -380.66[1] | 95.90[1] | 52.30[1] |
KBr (g) | -180.08[1] | -212.96[1] | 250.52[1] | 36.920[1] |
KBr (ai) | -373.92[1] | -387.23[1] | 184.9[1] | -120.1[1] |
SO2 (l) | -320.5[1] | – | – | – |
SO2 (g) | -296.830[1] | -300.194[1] | 248.22[1] | 39.87[1] |
SO2 (ao) | -322.980[1] | -300.676[1] | 161.9[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, (l):Liquid, (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°, -1125.5 kJ · mol−1
- ^ ΔfH°, -1140.1 kJ · mol−1
- ^ ΔfG°, -1053.1 kJ · mol−1
- ^ S°, 176. 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°, -393.798 kJ · mol−1
- ^ ΔfG°, -380.66 kJ · mol−1
- ^ S°, 95.90 J · K−1 · mol−1
- ^ Cp°, 52.30 J · K−1 · mol−1
- ^ ΔfH°, -180.08 kJ · mol−1
- ^ ΔfG°, -212.96 kJ · mol−1
- ^ S°, 250.52 J · K−1 · mol−1
- ^ Cp°, 36.920 J · K−1 · mol−1
- ^ ΔfH°, -373.92 kJ · mol−1
- ^ ΔfG°, -387.23 kJ · mol−1
- ^ S°, 184.9 J · K−1 · mol−1
- ^ Cp°, -120.1 J · K−1 · mol−1
- ^ ΔfH°, -320.5 kJ · mol−1
- ^ ΔfH°, -296.830 kJ · mol−1
- ^ ΔfG°, -300.194 kJ · mol−1
- ^ S°, 248.22 J · K−1 · mol−1
- ^ Cp°, 39.87 J · K−1 · mol−1
- ^ ΔfH°, -322.980 kJ · mol−1
- ^ ΔfG°, -300.676 kJ · mol−1
- ^ S°, 161.9 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