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6Na + 2CH3COONH4 → 4NaOH + 2NaCN + 2CH4↑ + H2↑

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Reaction of sodium and ammonium acetate
6NaSodium + 2CH3COONH4Ammonium acetate
⟶
4NaOHSodium hydroxide + 2NaCNSodium cyanide + 2CH4↑Methane + H2↑Hydrogen

The reaction of sodium and ammonium acetate yields sodium hydroxide, sodium cyanide, methane, and hydrogen (Other reactions are here). This reaction is an oxidation-reduction 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 sodium and ammonium acetate
6NaSodium + 2CH3COONH4Ammonium acetate
⟶
4NaOHSodium hydroxide + 2NaCNSodium cyanide + 2CH4↑Methane + H2↑Hydrogen

General equation

Reaction of reducing species and reducible species
Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reaction of sodium and ammonium acetate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium6
Reducing
Reducing
CH3COONH4Ammonium acetate2
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaOHSodium hydroxide4
Oxidized
–
NaCNSodium cyanide2
Redoxed product
–
CH4Methane2
Reduced
–
H2Hydrogen1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and ammonium acetate
6NaCrystalline solid + 2CH3COONH4Crystalline solid
⟶
4NaOHCrystalline solid + 2NaCNCrystalline solidcubic + 2CH4↑Gas + H2↑Gas
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
−794.76–––
per 1 mol of
−132.46–––
per 1 mol of
−397.38–––
per 1 mol of
−198.69–––
per 1 mol of
−397.38–––
per 1 mol of
−397.38–––
per 1 mol of
−794.76–––

Changes in standard condition (2)

Reaction of sodium and ammonium acetate
6NaCrystalline solid + 2CH3COONH4Crystalline solid
⟶
4NaOHCrystalline solid + 2NaCNCrystalline solidorthorhombic + 2CH4↑Gas + H2↑Gas
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
−801.28–––
per 1 mol of
−133.55–––
per 1 mol of
−400.64–––
per 1 mol of
−200.32–––
per 1 mol of
−400.64–––
per 1 mol of
−400.64–––
per 1 mol of
−801.28–––

Changes in aqueous solution (1)

Reaction of sodium and ammonium acetate
◆
ΔrG−1059.8 kJ/mol
K4.67 × 10185
pK−185.67
6NaCrystalline solid + 2CH3COONH4Ionized aqueous solution
⟶
4NaOHIonized aqueous solution + 2NaCNIonized aqueous solution + 2CH4↑Gas + H2↑Gas
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
−972.0−1059.8294.6–
per 1 mol of
−162.0−176.6349.10–
per 1 mol of
−486.0−529.90147.3–
per 1 mol of
−243.0−264.9573.65–
per 1 mol of
−486.0−529.90147.3–
per 1 mol of
−486.0−529.90147.3–
per 1 mol of
−972.0−1059.8294.6–

Changes in aqueous solution (2)

Reaction of sodium and ammonium acetate
◆
ΔrG−1042.2 kJ/mol
K3.85 × 10182
pK−182.59
6NaCrystalline solid + 2CH3COONH4Ionized aqueous solution
⟶
4NaOHIonized aqueous solution + 2NaCNIonized aqueous solution + 2CH4↑Gas + H2↑Un-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
−976.2−1042.2741–
per 1 mol of
−162.7−173.70124–
per 1 mol of
−488.1−521.10371–
per 1 mol of
−244.1−260.55185–
per 1 mol of
−488.1−521.10371–
per 1 mol of
−488.1−521.10371–
per 1 mol of
−976.2−1042.2741–

Changes in aqueous solution (3)

Reaction of sodium and ammonium acetate
◆
ΔrG−1027.0 kJ/mol
K8.37 × 10179
pK−179.92
6NaCrystalline solid + 2CH3COONH4Ionized aqueous solution
⟶
4NaOHIonized aqueous solution + 2NaCNIonized aqueous solution + 2CH4↑Un-ionized aqueous solution + H2↑Gas
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
−1000.5−1027.089.4–
per 1 mol of
−166.75−171.1714.9–
per 1 mol of
−500.25−513.5044.7–
per 1 mol of
−250.13−256.7522.4–
per 1 mol of
−500.25−513.5044.7–
per 1 mol of
−500.25−513.5044.7–
per 1 mol of
−1000.5−1027.089.4–

Changes in aqueous solution (4)

Reaction of sodium and ammonium acetate
◆
ΔrG−1009.4 kJ/mol
K6.91 × 10176
pK−176.84
6NaCrystalline solid + 2CH3COONH4Ionized aqueous solution
⟶
4NaOHIonized aqueous solution + 2NaCNIonized aqueous solution + 2CH4↑Un-ionized aqueous solution + H2↑Un-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
−1004.7−1009.4536–
per 1 mol of
−167.45−168.2389.3–
per 1 mol of
−502.35−504.70268–
per 1 mol of
−251.18−252.35134–
per 1 mol of
−502.35−504.70268–
per 1 mol of
−502.35−504.70268–
per 1 mol of
−1004.7−1009.4536–

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
Na (cr)0[1]0[1]51.21[1]28.24[1]
Na (g)107.32[1]76.761[1]153.712[1]20.786[1]
CH3COONH4 (cr)-616.14[1]–––
CH3COONH4 (ai)-618.52[1]-448.61[1]200.0[1]73.6[1]
* (cr):Crystalline solid, (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
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]–
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]–
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]–
NaCN (cr)
cubic
-87.49[1]-76.43[1]115.60[1]70.37[1]
NaCN (cr)
orthorhombic
-90.75[1]–––
NaCN (g)109[1]79.94[1]249.43[1]51.17[1]
NaCN (ai)-89.5[1]-89.5[1]153.1[1]–
NaCN (cr)
1/2 hydrate
-235.77[1]–––
NaCN (cr)
2 hydrate
-679.77[1]–––
CH4 (g)-74.81[1]-50.72[1]186.264[1]35.309[1]
CH4 (ao)-89.04[1]-34.33[1]83.7[1]–
H2 (g)0[1]0[1]130.684[1]28.824[1]
H2 (ao)-4.2[1]17.6[1]577[1]–
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-ionized aqueous solution

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)