You-iggy
  1. Home
  2. Chemical reactions
  3. 8Na + 9H2CO3 → 8NaHCO3 + 3H2O + CH4↑

8Na + 9H2CO3 → 8NaHCO3 + 3H2O + CH4↑

Last updated:
Reaction of sodium and carbonic acid
8NaSodium + 9H2CO3Carbonic acid
⟶
8NaHCO3Sodium hydrogencarbonate + 3H2OWater + CH4↑Methane

The reaction of sodium and carbonic acid yields sodium hydrogencarbonate, water, and methane (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 carbonic acid
8NaSodium + 9H2CO3Carbonic acid
⟶
8NaHCO3Sodium hydrogencarbonate + 3H2OWater + CH4↑Methane

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 carbonic acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaSodium8
Reducing
Reducing
H2CO3Carbonic acid9
Oxidizing
Reducible

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaHCO3Sodium hydrogencarbonate8
Oxidized
–
H2OWater3
–
–
CH4Methane1
Reduced
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium and carbonic acid
◆
ΔrG−1943.67 kJ/mol
K3.28 × 10340
pK−340.52
8NaCrystalline solid + 9H2CO3Un-ionized aqueous solution
⟶
8NaHCO3Ionized aqueous solution + 3H2OLiquid + CH4↑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
−2092.33−1943.67−498.7–
per 1 mol of
−261.541−242.959−62.34–
per 1 mol of
−232.481−215.963−55.41–
−261.541−242.959−62.34–
per 1 mol of
−697.443−647.890−166.2–
per 1 mol of
−2092.33−1943.67−498.7–

Changes in standard condition (2)

Reaction of sodium and carbonic acid
◆
ΔrG−1927.28 kJ/mol
K4.41 × 10337
pK−337.64
8NaCrystalline solid + 9H2CO3Un-ionized aqueous solution
⟶
8NaHCO3Ionized aqueous solution + 3H2OLiquid + CH4↑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
−2106.56−1927.28−601.3–
per 1 mol of
−263.320−240.910−75.16–
per 1 mol of
−234.062−214.142−66.81–
−263.320−240.910−75.16–
per 1 mol of
−702.187−642.427−200.4–
per 1 mol of
−2106.56−1927.28−601.3–

Changes in standard condition (3)

Reaction of sodium and carbonic acid
◆
ΔrG−1952.0 kJ/mol
K9.45 × 10341
pK−341.98
8NaCrystalline solid + 9H2CO3Un-ionized aqueous solution
⟶
8NaHCO3Un-ionized aqueous solution + 3H2OLiquid + CH4↑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
−2186.7−1952.0−789.9–
per 1 mol of
−273.34−244.00−98.74–
per 1 mol of
−242.97−216.89−87.77–
−273.34−244.00−98.74–
per 1 mol of
−728.90−650.67−263.3–
per 1 mol of
−2186.7−1952.0−789.9–

Changes in standard condition (4)

Reaction of sodium and carbonic acid
◆
ΔrG−1935.6 kJ/mol
K1.27 × 10339
pK−339.10
8NaCrystalline solid + 9H2CO3Un-ionized aqueous solution
⟶
8NaHCO3Un-ionized aqueous solution + 3H2OLiquid + CH4↑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
−2200.9−1935.6−892.5–
per 1 mol of
−275.11−241.95−111.6–
per 1 mol of
−244.54−215.07−99.17–
−275.11−241.95−111.6–
per 1 mol of
−733.63−645.20−297.5–
per 1 mol of
−2200.9−1935.6−892.5–

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]
H2CO3 (ao)-699.65[1]-623.08[1]187.4[1]–
* (cr):Crystalline solid, (g):Gas, (ao):Un-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
NaHCO3 (cr)-950.81[1]-851.0[1]101.7[1]87.61[1]
NaHCO3 (ai)-932.11[1]-848.66[1]150.2[1]–
NaHCO3 (ao)-943.9[1]-849.7[1]113.8[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]
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]–
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (l):Liquid, (g):Gas

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)