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Mg(NO3)2 + K2CO3 💧→ MgCO3↓ + 2KNO3

The reaction of magnesium nitrate and potassium carbonate yields magnesium carbonate and potassium nitrate. 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 categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Mg(NO3)2Magnesium nitrate1
Lewis acid
Very soluble in water
K2CO3Potassium carbonate1
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgCO3Magnesium carbonate1
Lewis conjugate
Very slightly soluble in water
KNO3Potassium nitrate2
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of magnesium nitrate and potassium carbonate
ΔrG−148.9 kJ/mol
K1.22 × 1026
pK−26.09
Mg(NO3)2Crystalline solid + K2CO3Crystalline solid
💧
MgCO3Crystalline solid + 2KNO3Crystalline 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
−143.4−148.912.311.97
per 1 mol of
−143.4−148.912.311.97
−143.4−148.912.311.97
−143.4−148.912.311.97
per 1 mol of
−71.70−74.456.155.985

Changes in aqueous solution

Reaction of magnesium nitrate and potassium carbonate
ΔrG−29.5 kJ/mol
K1.47 × 105
pK−5.17
Mg(NO3)2Ionized aqueous solution + K2CO3Ionized aqueous solution
💧
MgCO3Crystalline solid + 2KNO3Ionized 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
48.2−29.5260.6
per 1 mol of
48.2−29.5260.6
48.2−29.5260.6
48.2−29.5260.6
per 1 mol of
24.1−14.8130.3

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
Mg(NO3)2 (cr)-790.65[1]-589.4[1]164.0[1]141.92[1]
Mg(NO3)2 (ai)-881.57[1]-677.3[1]154.8[1]
Mg(NO3)2 (cr)
2 hydrate
-1409.2[1]
Mg(NO3)2 (cr)
6 hydrate
-2613.28[1]-2080.3[1]452[1]
K2CO3 (cr)-1151.02[1]-1063.5[1]155.52[1]114.43[1]
K2CO3 (ai)-1181.90[1]-1094.36[1]148.1[1]
K2CO3 (cr)
1.5 hydrate
-1609.2[1]-1432.5[1]203.3[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

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
MgCO3 (cr)-1095.8[1]-1012.1[1]65.7[1]75.52[1]
MgCO3 (cr)
3 hydrate
-1726.1[1]
MgCO3 (cr)
5 hydrate
-2199.2[1]
KNO3 (cr)-494.63[1]-394.86[1]133.05[1]96.40[1]
KNO3 (ai)-459.74[1]-394.53[1]248.9[1]-64.9[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1