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K2CO3 + 2HNO3 → 2KNO3 + CO2↑ + H2O

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Reaction of potassium carbonate and nitric acid
K2CO3Potassium carbonate + 2HNO3Nitric acid
⟶
2KNO3Potassium nitrate + CO2↑Carbon dioxide + H2OWater

The reaction of potassium carbonate and nitric acid yields potassium nitrate, carbon dioxide, 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

Reaction of potassium carbonate and nitric acid
K2CO3Potassium carbonate + 2HNO3Nitric acid
⟶
2KNO3Potassium nitrate + CO2↑Carbon dioxide + H2OWater

General equation

Reaction of salt of weak acid and strong acid with generating weak acidic oxide
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Acidic oxide + H2OConjugate acid

Oxidation state of each atom

Reaction of potassium carbonate and nitric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
K2CO3Potassium carbonate1
Brønsted base
Salt of weak acid
HNO3Nitric acid2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
KNO3Potassium nitrate2
Conjugate base
Salt of strong acid
CO2Carbon dioxide1
–
Acidic oxide
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of potassium carbonate and nitric acid
◆
ΔrG−196.3 kJ/mol
K2.46 × 1034
pK−34.39
K2CO3Crystalline solid + 2HNO3Liquid
⟶
2KNO3Crystalline solid + CO2↑Gas + H2OLiquid
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
−169.38−196.383.03−28.97
−169.38−196.383.03−28.97
per 1 mol of
−84.690−98.1541.52−14.48
per 1 mol of
−84.690−98.1541.52−14.48
per 1 mol of
−169.38−196.383.03−28.97
per 1 mol of
−169.38−196.383.03−28.97

Changes in aqueous solution (1)

Reaction of potassium carbonate and nitric acid
◆
ΔrG−103.69 kJ/mol
K1.46 × 1018
pK−18.17
K2CO3Ionized aqueous solution + 2HNO3Ionized aqueous solution
⟶
2KNO3Ionized aqueous solution + CO2↑Gas + H2OLiquid
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
−2.20−103.69340.6–
−2.20−103.69340.6–
per 1 mol of
−1.10−51.845170.3–
per 1 mol of
−1.10−51.845170.3–
per 1 mol of
−2.20−103.69340.6–
per 1 mol of
−2.20−103.69340.6–

Changes in aqueous solution (2)

Reaction of potassium carbonate and nitric acid
◆
ΔrG−95.31 kJ/mol
K4.98 × 1016
pK−16.70
K2CO3Ionized aqueous solution + 2HNO3Ionized aqueous solution
⟶
2KNO3Ionized aqueous solution + CO2↑Un-ionized aqueous solution + H2OLiquid
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
−22.49−95.31244.4–
−22.49−95.31244.4–
per 1 mol of
−11.24−47.66122.2–
per 1 mol of
−11.24−47.66122.2–
per 1 mol of
−22.49−95.31244.4–
per 1 mol of
−22.49−95.31244.4–

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
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]–
HNO3 (l)-174.10[1]-80.71[1]155.60[1]109.87[1]
HNO3 (g)-135.06[1]-74.72[1]266.38[1]53.35[1]
HNO3 (ai)-207.36[1]-111.25[1]146.4[1]-86.6[1]
HNO3 (l)
1 hydrate
-473.46[1]-328.77[1]216.90[1]182.46[1]
HNO3 (l)
3 hydrate
-1056.04[1]-811.09[1]346.98[1]325.14[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (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
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]
CO2 (g)-393.509[1]-394.359[1]213.74[1]37.11[1]
CO2 (ao)-413.80[1]-385.98[1]117.6[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)