2KHSO4 + (NH4)2CrO4 💧→ K2CrO4↓ + 2NH4HSO4
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The reaction of potassium hydrogensulfate and ammonium chromate yields potassium chromate and ammonium hydrogensulfate (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 hydrogensulfate and ammonium chromate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of potassium hydrogensulfate and ammonium chromate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KHSO4 | Potassium hydrogensulfate | 2 | Lewis acid | Very soluble in water |
| (NH4)2CrO4 | Ammonium chromate | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K2CrO4 | Potassium chromate | 1 | Lewis conjugate | Insoluble in water |
| NH4HSO4 | Ammonium hydrogensulfate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium hydrogensulfate and ammonium chromate
- 2KHSO4Crystalline solid + (NH4)2CrO4Crystalline solidK2CrO4↓Crystalline solid + 2NH4HSO4Crystalline solid💧⟶
| 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 | 30.9 | – | – | – |
per 1 mol of | 15.4 | – | – | – |
per 1 mol of | 30.9 | – | – | – |
per 1 mol of | 30.9 | – | – | – |
per 1 mol of | 15.4 | – | – | – |
Changes in aqueous solution
- Reaction of potassium hydrogensulfate and ammonium chromate◆
ΔrG 0.00 kJ/mol K 1.00 × 100 pK 0.00 - 2KHSO4Ionized aqueous solution + (NH4)2CrO4Ionized aqueous solutionK2CrO4↓Ionized aqueous solution + 2NH4HSO4Ionized aqueous solution💧⟶
| 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 | −0.01 | 0.00 | 0.0 | – |
per 1 mol of | −0.00500 | 0.00 | 0.0 | – |
per 1 mol of | −0.0100 | 0.00 | 0.0 | – |
per 1 mol of | −0.0100 | 0.00 | 0.0 | – |
per 1 mol of | −0.00500 | 0.00 | 0.0 | – |
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 |
|---|---|---|---|---|
| KHSO4 (cr) | -1160.6[1] | -1031.3[1] | 138.1[1] | – |
| KHSO4 (ai) | -1139.72[1] | -1039.18[1] | 234.3[1] | -63[1] |
| (NH4)2CrO4 (cr) | -1167.3[1] | – | – | – |
| (NH4)2CrO4 (ai) | -1146.16[1] | -886.36[1] | 277.0[1] | – |
* (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 |
|---|---|---|---|---|
| K2CrO4 (cr) | -1403.7[1] | -1295.7[1] | 200.12[1] | 145.98[1] |
| K2CrO4 (ai) | -1385.91[1] | -1294.30[1] | 255.2[1] | – |
| NH4HSO4 (cr) | -1026.96[1] | – | – | – |
| NH4HSO4 (ai) | -1019.85[1] | -835.21[1] | 245.2[1] | -3.8[1] |
* (cr):Crystalline solid, (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°, -1160.6 kJ · mol−1
- ^ ΔfG°, -1031.3 kJ · mol−1
- ^ S°, 138.1 J · K−1 · mol−1
- ^ ΔfH°, -1139.72 kJ · mol−1
- ^ ΔfG°, -1039.18 kJ · mol−1
- ^ S°, 234.3 J · K−1 · mol−1
- ^ Cp°, -63. J · K−1 · mol−1
- ^ ΔfH°, -1167.3 kJ · mol−1
- ^ ΔfH°, -1146.16 kJ · mol−1
- ^ ΔfG°, -886.36 kJ · mol−1
- ^ S°, 277.0 J · K−1 · mol−1
- ^ ΔfH°, -1403.7 kJ · mol−1
- ^ ΔfG°, -1295.7 kJ · mol−1
- ^ S°, 200.12 J · K−1 · mol−1
- ^ Cp°, 145.98 J · K−1 · mol−1
- ^ ΔfH°, -1385.91 kJ · mol−1
- ^ ΔfG°, -1294.30 kJ · mol−1
- ^ S°, 255.2 J · K−1 · mol−1
- ^ ΔfH°, -1026.96 kJ · mol−1
- ^ ΔfH°, -1019.85 kJ · mol−1
- ^ ΔfG°, -835.21 kJ · mol−1
- ^ S°, 245.2 J · K−1 · mol−1
- ^ Cp°, -3.8 J · K−1 · mol−1