You-iggy

3SrBr2 + 8HNO3 → 3Sr(NO3)2 + 3Br2 + 2NO↑ + 4H2O

The reaction of strontium bromide and nitric acid yields strontium nitrate, bromine, nitrogen monoxide, and water (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
SrBr2Strontium bromide3
Reducing
Hardly oxidizable
HNO3Nitric acid8
Oxidizing
Oxidizing

Products

Chemical formulaNameCoefficientTypeType in general
equation
Sr(NO3)2Strontium nitrate3
Br2Bromine3
Oxidized
NONitrogen monoxide2
Reduced
H2OWater4

Thermodynamic changes

Changes in standard condition

Reaction of strontium bromide and nitric acid
ΔrG−378.5 kJ/mol
K2.04 × 1066
pK−66.31
3SrBr2Crystalline solid + 8HNO3Liquid
3Sr(NO3)2Crystalline solid + 3Br2Liquid + 2NOGas + 4H2OLiquid
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
−351.9−378.591.43−67.36
per 1 mol of
−117.3−126.230.48−22.45
per 1 mol of
−43.99−47.3111.43−8.420
per 1 mol of
−117.3−126.230.48−22.45
per 1 mol of
−117.3−126.230.48−22.45
per 1 mol of
−175.9−189.345.72−33.68
per 1 mol of
−87.97−94.6322.86−16.84

Changes in aqueous solution

Reaction of strontium bromide and nitric acid
ΔrG82.60 kJ/mol
K0.34 × 10−14
pK14.47
3SrBr2Ionized aqueous solution + 8HNO3Ionized aqueous solution
3Sr(NO3)2Ionized aqueous solution + 3Br2Un-ionized aqueous solution + 2NOGas + 4H2OLiquid
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
173.4082.60305.5
per 1 mol of
57.80027.53101.8
per 1 mol of
21.67510.3238.19
per 1 mol of
57.80027.53101.8
per 1 mol of
57.80027.53101.8
per 1 mol of
86.70041.30152.8
per 1 mol of
43.35020.6576.38

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
SrBr2 (cr)-717.6[1]-697.1[1]135.10[1]75.35[1]
SrBr2 (g)-410[1]-444[1]323.5[1]60.7[1]
SrBr2 (ai)-788.89[1]-767.39[1]132.2[1]
SrBr2 (cr)
1 hydrate
-1031.4[1]-954.3[1]180[1]120.9[1]
SrBr2 (cr)
6 hydrate
-2531.3[1]-2174.1[1]406[1]343.5[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, (ai):Ionized aqueous solution, (l):Liquid

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
Sr(NO3)2 (cr)-978.22[1]-780.02[1]194.56[1]149.91[1]
Sr(NO3)2 (ai)-960.52[1]-781.98[1]260.2[1]
Sr(NO3)2 (cr)
4 hydrate
-2154.8[1]-1730.39[1]369.0[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]
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]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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)