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2SnBr4 + 2HNO3 → 2SnO2 + 3Br2 + 2NO↑ + 2HBr↑

The reaction of tin(IV) bromide and nitric acid yields tin(IV) oxide, bromine, nitrogen monoxide, and hydrogen bromide (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

General equation

Reaction of hardly oxidizable species and oxidizing species
Hardly oxidizable speciesReducing agent + Oxidizing speciesOxidizing agent
ProductOxidation product + ProductReduction product

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SnBr4Tin(IV) bromide2
Reducing
Hardly oxidizable
HNO3Nitric acid2
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
SnO2Tin(IV) oxide2
Br2Bromine3
Oxidized
NONitrogen monoxide2
Reduced
HBrHydrogen bromide2

Thermodynamic changes

Changes in aqueous solution (1)

Reaction of tin(IV) bromide and nitric acid
ΔrG−38.3 kJ/mol
K5.13 × 106
pK−6.71
2SnBr4Crystalline solid + 2HNO3Ionized aqueous solution
2SnO2Crystalline solid + 3Br2Un-ionized aqueous solution + 2NOGas + 2HBrGas
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
108.1−38.3493.4
per 1 mol of
54.05−19.1246.7
per 1 mol of
54.05−19.1246.7
per 1 mol of
54.05−19.1246.7
per 1 mol of
36.03−12.8164.5
per 1 mol of
54.05−19.1246.7
per 1 mol of
54.05−19.1246.7

Changes in aqueous solution (2)

Reaction of tin(IV) bromide and nitric acid
ΔrG−139.3 kJ/mol
K2.54 × 1024
pK−24.40
2SnBr4Crystalline solid + 2HNO3Ionized aqueous solution
2SnO2Crystalline solid + 3Br2Un-ionized aqueous solution + 2NOGas + 2HBrIonized 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
−62.3−139.3260.8
per 1 mol of
−31.1−69.65130.4
per 1 mol of
−31.1−69.65130.4
per 1 mol of
−31.1−69.65130.4
per 1 mol of
−20.8−46.4386.93
per 1 mol of
−31.1−69.65130.4
per 1 mol of
−31.1−69.65130.4

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
SnBr4 (cr)-377.4[1]-350.2[1]264.4[1]
SnBr4 (g)-314.6[1]-331.4[1]411.94[1]103.39[1]
SnBr4 (cr)
8 hydrate
-2767.7[1]
SnBr4 (l)
8 hydrate
-2725.0[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, (g):Gas, (l):Liquid, (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
SnO2 (cr)-580.7[1]-519.6[1]52.3[1]52.59[1]
Br2 (cr)
Br2 (l)0[1]0[1]152.231[1]75.689[1]
Br2 (g)30.907[1]3.110[1]245.463[1]36.02[1]
Br2 (ao)-2.59[1]3.93[1]130.5[1]
NO (g)90.25[1]86.55[1]210.761[1]29.844[1]
HBr (g)-36.40[1]-53.45[1]198.695[1]29.142[1]
HBr (ai)-121.55[1]-103.96[1]82.4[1]-141.8[1]
* (cr):Crystalline solid, (l):Liquid, (g):Gas, (ao):Un-ionized aqueous solution, (ai):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)