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(NH4)2CrO4 + 2KOH → K2CrO4↓ + 2NH3↑ + 2H2O

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:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
(NH4)2CrO4Ammonium chromate1
Brønsted acid
Lewis acid
Salt of weak base
Salt of volatile base
Very soluble in water
KOHPotassium hydroxide2
Brønsted base
Lewis base
Strong base
Nonvolatile base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2CrO4Potassium chromate1
Conjugate acid
Lewis conjugate
Salt of strong base
Salt of non volatile base
Insoluble in water
NH3Ammonia2
Conjugate base
Non-redox product
Weak base
Volatile base
H2OWater2
Non-redox product
Water

Thermodynamic changes

Changes in standard condition

Reaction of ammonium chromate and potassium hydroxide
(NH4)2CrO4Crystalline solid + 2KOHCrystalline solid
K2CrO4Crystalline solid + 2NH3Gas + 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
−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
K9.42 × 105
pK−5.97
(NH4)2CrO4Ionized aqueous solution + 2KOHIonized aqueous solution
K2CrO4Ionized aqueous solution + 2NH3Gas + 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
61.11−34.10319.7
per 1 mol of
61.11−34.10319.7
30.55−17.05159.8
per 1 mol of
61.11−34.10319.7
per 1 mol of
30.55−17.05159.8
per 1 mol of
30.55−17.05159.8

Changes in aqueous solution (2)

Reaction of ammonium chromate and potassium hydroxide
ΔrG−54.20 kJ/mol
K3.13 × 109
pK−9.50
(NH4)2CrO4Ionized aqueous solution + 2KOHIonized aqueous solution
K2CrO4Ionized aqueous solution + 2NH3Un-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
−7.25−54.20157.4
per 1 mol of
−7.25−54.20157.4
−3.63−27.1078.70
per 1 mol of
−7.25−54.20157.4
per 1 mol of
−3.63−27.1078.70
per 1 mol of
−3.63−27.1078.70

Thermodynamic data of reactants

Chemical formulaStandard 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 formulaStandard 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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)