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PbCrO4 + 2HNO3 → Pb(NO3)2 + CrO3 + H2O

The reaction of lead(II) chromate and nitric acid yields lead(II) nitrate, chromium(VI) oxide, 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
PbCrO4Lead(II) chromate1
Brønsted base
Salt of weak acid
HNO3Nitric acid2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Pb(NO3)2Lead(II) nitrate1
Conjugate base
Salt of strong acid
CrO3Chromium(VI) oxide1
Acidic oxide
H2OWater1
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of lead(II) chromate and nitric acid
PbCrO4Crystalline solid + 2HNO3Liquid
Pb(NO3)2Crystalline solid + CrO3Crystalline solid + 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
−48.1
per 1 mol of
−48.1
per 1 mol of
−24.1
per 1 mol of
−48.1
per 1 mol of
−48.1
per 1 mol of
−48.1

Changes in aqueous solution

Reaction of lead(II) chromate and nitric acid
PbCrO4Crystalline solid + 2HNO3Ionized aqueous solution
Pb(NO3)2Ionized aqueous solution + CrO3Crystalline solid + 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
54.0
per 1 mol of
54.0
per 1 mol of
27.0
per 1 mol of
54.0
per 1 mol of
54.0
per 1 mol of
54.0

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
PbCrO4 (cr)-930.9[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, (l):Liquid, (g):Gas, (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
Pb(NO3)2 (cr)-451.9[1]
Pb(NO3)2 (ai)-416.3[1]-246.93[1]303.3[1]
CrO3 (cr)-589.5[1]
CrO3 (g)-385.8[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, (l):Liquid

References

List of references

  1. 1