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  3. 15NaI + 12HNO3 + 5H^+ → 10NaIO3 + 5Na^+ + 6N2↑ + 6H2O + 5HI↑

15NaI + 12HNO3 + 5H+ → 10NaIO3 + 5Na+ + 6N2↑ + 6H2O + 5HI↑

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Reaction of sodium iodide and nitric acid under acidic condition
15NaISodium iodide + 12HNO3Nitric acid + 5H+Hydrogen ion
⟶
10NaIO3Sodium iodate + 5Na+Sodium ion + 6N2↑Nitrogen + 6H2OWater + 5HI↑Hydrogen iodide

The reaction of sodium iodide, nitric acid, and hydrogen ion yields sodium iodate, sodium ion, nitrogen, water, and hydrogen iodide (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 iodide and nitric acid under acidic condition
15NaISodium iodide + 12HNO3Nitric acid + 5H+Hydrogen ion
⟶
10NaIO3Sodium iodate + 5Na+Sodium ion + 6N2↑Nitrogen + 6H2OWater + 5HI↑Hydrogen iodide

General equation

Reaction of oxidizable species and oxidizing species under acidic condition
Oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent + H+Non-redox agent
⟶
ProductOxidation product + ProductReduction product + H2ONon-redox product

Oxidation state of each atom

Reaction of sodium iodide and nitric acid under acidic condition

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
NaISodium iodide15
Reducing
Oxidizable
HNO3Nitric acid12
Oxidizing
Oxidizing under acidic condition
H+Hydrogen ion5
–
Hydrogen ion

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaIO3Sodium iodate10
Oxidized
–
Na+Sodium ion5
–
–
N2Nitrogen6
Reduced
–
H2OWater6
–
Water
HIHydrogen iodide5
–
–

Thermodynamic changes

Changes in standard condition (1)

Reaction of sodium iodide and nitric acid under acidic condition
◆
ΔrG−585.7 kJ/mol
K4.08 × 10102
pK−102.61
15NaIIonized aqueous solution + 12HNO3Ionized aqueous solution + 5H+Un-ionized aqueous solution
⟶
10NaIO3Ionized aqueous solution + 5Na+Un-ionized aqueous solution + 6N2↑Gas + 6H2OLiquid + 5HI↑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
−480.2−585.7359.8–
per 1 mol of
−32.01−39.0523.99–
per 1 mol of
−40.02−48.8129.98–
per 1 mol of
Hydrogen ion
−96.04−117.171.96–
per 1 mol of
−48.02−58.5735.98–
per 1 mol of
Sodium ion
−96.04−117.171.96–
per 1 mol of
−80.03−97.6259.97–
per 1 mol of
−80.03−97.6259.97–
per 1 mol of
−96.04−117.171.96–

Changes in standard condition (2)

Reaction of sodium iodide and nitric acid under acidic condition
◆
ΔrG−852.1 kJ/mol
K1.91 × 10149
pK−149.28
15NaIIonized aqueous solution + 12HNO3Ionized aqueous solution + 5H+Un-ionized aqueous solution
⟶
10NaIO3Ionized aqueous solution + 5Na+Un-ionized aqueous solution + 6N2↑Gas + 6H2OLiquid + 5HI↑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
−888.6−852.1−116.7–
per 1 mol of
−59.24−56.81−7.780–
per 1 mol of
−74.05−71.01−9.725–
per 1 mol of
Hydrogen ion
−177.7−170.4−23.34–
per 1 mol of
−88.86−85.21−11.67–
per 1 mol of
Sodium ion
−177.7−170.4−23.34–
per 1 mol of
−148.1−142.0−19.45–
per 1 mol of
−148.1−142.0−19.45–
per 1 mol of
−177.7−170.4−23.34–

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
NaI (cr)-287.78[1]-286.06[1]98.53[1]52.09[1]
NaI (g)-79.5[1]-121.0[1]248.978[1]36.65[1]
NaI (ai)-295.31[1]-313.47[1]170.3[1]-95.8[1]
NaI (cr)
1 hydrate
-883.096[1]-771.10[1]196.2[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]
H+ (g)1536.202[1]–––
H+ (ao)0[1]0[1]0[1]0[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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
NaIO3 (cr)-481.788[1]––92.0[1]
NaIO3 (ai)-461.5[1]-389.9[1]177.4[1]–
NaIO3 (cr)
1 hydrate
-779.48[1]-634.03[1]162.3[1]–
NaIO3 (cr)
5 hydrate
-1952.25[1]–––
Na+ (g)609.358[1]–––
Na+ (ao)-240.12[1]-261.905[1]59.0[1]46.4[1]
N2 (g)0[1]0[1]191.61[1]29.125[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]
HI (g)26.48[1]1.70[1]206.594[1]29.158[1]
HI (ai)-55.19[1]-51.57[1]111.3[1]-142.3[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)