Na2SeO4 + 2H2SO4 → 2NaHSO4 + SeO3 + H2O
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The reaction of sodium selenate and sulfuric acid yields sodium hydrogensulfate, selenium trioxide, 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 sodium selenate and sulfuric acid
General equation
- Oxoacid saltBrønsted base + Dehydrating acidBrønsted acid ⟶ SaltConjugate base + Acidic oxide + H2OConjugate acid
Oxidation state of each atom
- Reaction of sodium selenate and sulfuric acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Na2SeO4 | Sodium selenate | 1 | Brønsted base | Oxoacid salt |
| H2SO4 | Sulfuric acid | 2 | Brønsted acid | Dehydrating acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| NaHSO4 | Sodium hydrogensulfate | 2 | Conjugate base | Salt |
| SeO3 | Selenium trioxide | 1 | – | Acidic oxide |
| H2O | Water | 1 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition
- Reaction of sodium selenate and sulfuric acid
| 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 | −6.8 | – | – | – |
per 1 mol of | −6.8 | – | – | – |
per 1 mol of | −3.4 | – | – | – |
per 1 mol of | −3.4 | – | – | – |
per 1 mol of | −6.8 | – | – | – |
per 1 mol of | −6.8 | – | – | – |
Changes in aqueous solution
- Reaction of sodium selenate and sulfuric acid
| 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 | 190.4 | – | – | – |
per 1 mol of | 190.4 | – | – | – |
per 1 mol of | 95.20 | – | – | – |
per 1 mol of | 95.20 | – | – | – |
per 1 mol of | 190.4 | – | – | – |
per 1 mol of | 190.4 | – | – | – |
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 |
|---|---|---|---|---|
| Na2SeO4 (cr) | -1069.0[1] | – | – | – |
| Na2SeO4 (ai) | -1079.5[1] | -965.2[1] | 172.0[1] | – |
| Na2SeO4 (cr) 10 hydrate | -4006.6[1] | – | – | – |
| H2SO4 (cr) | – | – | – | – |
| H2SO4 (l) | -813.989[1] | -690.003[1] | 156.904[1] | 138.91[1] |
| H2SO4 (ai) | -909.27[1] | -744.53[1] | 20.1[1] | -293[1] |
| H2SO4 (l) 1 hydrate | -1127.621[1] | -950.383[1] | 211.54[1] | 214.85[1] |
| H2SO4 (l) 2 hydrate | -1427.100[1] | -1199.650[1] | 276.40[1] | 260.83[1] |
| H2SO4 (l) 3 hydrate | -1720.402[1] | -1443.980[1] | 345.39[1] | 318.95[1] |
| H2SO4 (l) 4 hydrate | -2011.199[1] | -1685.863[1] | 414.59[1] | 382.21[1] |
| H2SO4 (l) 6.5 hydrate | -2733.256[1] | -2285.734[1] | 587.89[1] | 570.28[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid
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 |
|---|---|---|---|---|
| NaHSO4 (cr) | -1125.5[1] | -992.8[1] | 113.0[1] | – |
| NaHSO4 (ai) | -1127.46[1] | -1017.80[1] | 190.8[1] | -38[1] |
| NaHSO4 (cr) 1 hydrate | -1421.7[1] | -1231.6[1] | 155[1] | – |
| SeO3 (cr) | -166.9[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, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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°, -1069.0 kJ · mol−1
- ^ ΔfH°, -1079.5 kJ · mol−1
- ^ ΔfG°, -965.2 kJ · mol−1
- ^ S°, 172.0 J · K−1 · mol−1
- ^ ΔfH°, -4006.6 kJ · mol−1
- ^ ΔfH°, -813.989 kJ · mol−1
- ^ ΔfG°, -690.003 kJ · mol−1
- ^ S°, 156.904 J · K−1 · mol−1
- ^ Cp°, 138.91 J · K−1 · mol−1
- ^ ΔfH°, -909.27 kJ · mol−1
- ^ ΔfG°, -744.53 kJ · mol−1
- ^ S°, 20.1 J · K−1 · mol−1
- ^ Cp°, -293. J · K−1 · mol−1
- ^ ΔfH°, -1127.621 kJ · mol−1
- ^ ΔfG°, -950.383 kJ · mol−1
- ^ S°, 211.54 J · K−1 · mol−1
- ^ Cp°, 214.85 J · K−1 · mol−1
- ^ ΔfH°, -1427.100 kJ · mol−1
- ^ ΔfG°, -1199.650 kJ · mol−1
- ^ S°, 276.40 J · K−1 · mol−1
- ^ Cp°, 260.83 J · K−1 · mol−1
- ^ ΔfH°, -1720.402 kJ · mol−1
- ^ ΔfG°, -1443.980 kJ · mol−1
- ^ S°, 345.39 J · K−1 · mol−1
- ^ Cp°, 318.95 J · K−1 · mol−1
- ^ ΔfH°, -2011.199 kJ · mol−1
- ^ ΔfG°, -1685.863 kJ · mol−1
- ^ S°, 414.59 J · K−1 · mol−1
- ^ Cp°, 382.21 J · K−1 · mol−1
- ^ ΔfH°, -2733.256 kJ · mol−1
- ^ ΔfG°, -2285.734 kJ · mol−1
- ^ S°, 587.89 J · K−1 · mol−1
- ^ Cp°, 570.28 J · K−1 · mol−1
- ^ ΔfH°, -1125.5 kJ · mol−1
- ^ ΔfG°, -992.8 kJ · mol−1
- ^ S°, 113.0 J · K−1 · mol−1
- ^ ΔfH°, -1127.46 kJ · mol−1
- ^ ΔfG°, -1017.80 kJ · mol−1
- ^ S°, 190.8 J · K−1 · mol−1
- ^ Cp°, -38. J · K−1 · mol−1
- ^ ΔfH°, -1421.7 kJ · mol−1
- ^ ΔfG°, -1231.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -166.9 kJ · 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