(NH4)2CrO4 + 2KOH → K2CrO4↓ + 2NH3↑ + 2H2O
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- Reaction of ammonium chromate and potassium hydroxide
The reaction of ammonium chromate and potassium hydroxide yields potassium chromate, ammonia, and water (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
- Reaction of salt of weak base and strong base
- Reaction of volatile acid and non volatile base
- Precipitation reaction
Table of contents
Reaction data
Chemical equation
- Reaction of ammonium chromate and potassium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
- Reaction of volatile acid and non volatile base
- Salt of volatile baseBrønsted acid + Nonvolatile baseBrønsted base ⟶ Salt of non volatile baseConjugate acid + Volatile baseConjugate base + (H2O)
- 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 ammonium chromate and potassium hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
(NH4)2CrO4 | Ammonium chromate | 1 | Brønsted acid Lewis acid | Salt of weak base Salt of volatile base Very soluble in water |
KOH | Potassium hydroxide | 2 | Brønsted base Lewis base | Strong base Nonvolatile base Very soluble in water |
Products
Thermodynamic changes
Changes in standard condition
- Reaction of ammonium chromate and potassium hydroxide
- (NH4)2CrO4Crystalline solid + 2KOHCrystalline solidK2CrO4↓Crystalline solid + 2NH3↑Gas + 2H2OLiquid⟶
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 | −50.8 | – | – | – |
per 1 mol of | −50.8 | – | – | – |
per 1 mol of | −25.4 | – | – | – |
per 1 mol of | −50.8 | – | – | – |
per 1 mol of | −25.4 | – | – | – |
per 1 mol of | −25.4 | – | – | – |
Changes in aqueous solution (1)
- Reaction of ammonium chromate and potassium hydroxide◆
ΔrG −34.10 kJ/mol K 9.42 × 105 pK −5.97 - (NH4)2CrO4Ionized aqueous solution + 2KOHIonized aqueous solutionK2CrO4↓Ionized aqueous solution + 2NH3↑Gas + 2H2OLiquid⟶
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 | 61.11 | −34.10 | 319.7 | – |
per 1 mol of | 61.11 | −34.10 | 319.7 | – |
per 1 mol of | 30.55 | −17.05 | 159.8 | – |
per 1 mol of | 61.11 | −34.10 | 319.7 | – |
per 1 mol of | 30.55 | −17.05 | 159.8 | – |
per 1 mol of | 30.55 | −17.05 | 159.8 | – |
Changes in aqueous solution (2)
- Reaction of ammonium chromate and potassium hydroxide◆
ΔrG −54.20 kJ/mol K 3.13 × 109 pK −9.50 - (NH4)2CrO4Ionized aqueous solution + 2KOHIonized aqueous solutionK2CrO4↓Ionized aqueous solution + 2NH3↑Un-ionized aqueous solution + 2H2OLiquid⟶
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 | −7.25 | −54.20 | 157.4 | – |
per 1 mol of | −7.25 | −54.20 | 157.4 | – |
per 1 mol of | −3.63 | −27.10 | 78.70 | – |
per 1 mol of | −7.25 | −54.20 | 157.4 | – |
per 1 mol of | −3.63 | −27.10 | 78.70 | – |
per 1 mol of | −3.63 | −27.10 | 78.70 | – |
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 |
---|---|---|---|---|
(NH4)2CrO4 (cr) | -1167.3[1] | – | – | – |
(NH4)2CrO4 (ai) | -1146.16[1] | -886.36[1] | 277.0[1] | – |
KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[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 |
---|---|---|---|---|
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] | – |
NH3 (g) | -46.11[1] | -16.45[1] | 192.45[1] | 35.06[1] |
NH3 (ao) | -80.29[1] | -26.50[1] | 111.3[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, (g):Gas, (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°, -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°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 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°, -46.11 kJ · mol−1
- ^ ΔfG°, -16.45 kJ · mol−1
- ^ S°, 192.45 J · K−1 · mol−1
- ^ Cp°, 35.06 J · K−1 · mol−1
- ^ ΔfH°, -80.29 kJ · mol−1
- ^ ΔfG°, -26.50 kJ · mol−1
- ^ S°, 111.3 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