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CuS + 2HNO3 🔥→ Cu(NO3)2 + H2S↑

The reaction of copper(II) sulfide and nitric acid yields copper(II) nitrate and hydrogen sulfide (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
CuSCopper(II) sulfide1
Brønsted base
Salt of weak acid
HNO3Nitric acid2
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Cu(NO3)2Copper(II) nitrate1
Conjugate base
Salt of strong acid
H2SHydrogen sulfide1
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of copper(II) sulfide and nitric acid
CuSCrystalline solid + 2HNO3Liquid
🔥
Cu(NO3)2Crystalline solid + H2SGas
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
77.8
per 1 mol of
77.8
per 1 mol of
38.9
per 1 mol of
77.8
per 1 mol of
77.8

Changes in aqueous solution (1)

Reaction of copper(II) sulfide and nitric acid
ΔrG85.5 kJ/mol
K0.10 × 10−14
pK14.98
CuSCrystalline solid + 2HNO3Ionized aqueous solution
🔥
Cu(NO3)2Ionized aqueous solution + H2SGas
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
97.285.539.8
per 1 mol of
97.285.539.8
per 1 mol of
48.642.819.9
per 1 mol of
97.285.539.8
per 1 mol of
97.285.539.8

Changes in aqueous solution (2)

Reaction of copper(II) sulfide and nitric acid
ΔrG91.3 kJ/mol
K0.10 × 10−15
pK16.00
CuSCrystalline solid + 2HNO3Ionized aqueous solution
🔥
Cu(NO3)2Ionized aqueous solution + H2SUn-ionized 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
78.291.3−45
per 1 mol of
78.291.3−45
per 1 mol of
39.145.6−23
per 1 mol of
78.291.3−45
per 1 mol of
78.291.3−45

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
CuS (cr)-53.1[1]-53.6[1]66.5[1]47.82[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
Cu(NO3)2 (cr)-302.9[1]
Cu(NO3)2 (ai)-349.95[1]-157.02[1]193.3[1]
Cu(NO3)2 (cr)
3 hydrate
-1217.1[1]
Cu(NO3)2 (cr)
6 hydrate
-2110.8[1]
H2S (g)-20.63[1]-33.56[1]205.79[1]34.23[1]
H2S (ao)-39.7[1]-27.83[1]121[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution

References

List of references

  1. 1