2KClO4 + (NH4)2CrO4 💧→ K2CrO4↓ + 2NH4ClO4
Last updated:
The reaction of potassium perchlorate and ammonium chromate yields potassium chromate and ammonium perchlorate. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium perchlorate 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 perchlorate and ammonium chromate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
KClO4 | Potassium perchlorate | 2 | Lewis acid | 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 |
NH4ClO4 | Ammonium perchlorate | 2 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition
- Reaction of potassium perchlorate and ammonium chromate
- 2KClO4Crystalline solid + (NH4)2CrO4Crystalline solidK2CrO4↓Crystalline solid + 2NH4ClO4Crystalline 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 | 38.5 | – | – | – |
per 1 mol of | 19.3 | – | – | – |
per 1 mol of | 38.5 | – | – | – |
per 1 mol of | 38.5 | – | – | – |
per 1 mol of | 19.3 | – | – | – |
Changes in aqueous solution
- Reaction of potassium perchlorate and ammonium chromate◆
ΔrG −0.02 kJ/mol K 1.01 × 100 pK −0.00 - 2KClO4Ionized aqueous solution + (NH4)2CrO4Ionized aqueous solutionK2CrO4↓Ionized aqueous solution + 2NH4ClO4Ionized 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 | −0.02 | 0.0 | – |
per 1 mol of | 0.00500 | −0.0100 | 0.0 | – |
per 1 mol of | 0.0100 | −0.0200 | 0.0 | – |
per 1 mol of | 0.0100 | −0.0200 | 0.0 | – |
per 1 mol of | 0.00500 | −0.0100 | 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 |
---|---|---|---|---|
KClO4 (cr) | -432.75[1] | -303.09[1] | 151.0[1] | 112.38[1] |
KClO4 (ai) | -381.71[1] | -291.79[1] | 284.5[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] | – |
NH4ClO4 (cr) | -295.31[1] | -88.75[1] | 186.2[1] | – |
NH4ClO4 (ai) | -261.83[1] | -87.83[1] | 295.4[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°, -432.75 kJ · mol−1
- ^ ΔfG°, -303.09 kJ · mol−1
- ^ S°, 151.0 J · K−1 · mol−1
- ^ Cp°, 112.38 J · K−1 · mol−1
- ^ ΔfH°, -381.71 kJ · mol−1
- ^ ΔfG°, -291.79 kJ · mol−1
- ^ S°, 284.5 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°, -295.31 kJ · mol−1
- ^ ΔfG°, -88.75 kJ · mol−1
- ^ S°, 186.2 J · K−1 · mol−1
- ^ ΔfH°, -261.83 kJ · mol−1
- ^ ΔfG°, -87.83 kJ · mol−1
- ^ S°, 295.4 J · K−1 · mol−1