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2RbCl + H2SO4 → Rb2SO4 + 2HCl↑

The reaction of rubidium chloride and sulfuric acid yields rubidium sulfate and hydrogen chloride. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
RbClRubidium chloride2
Brønsted base
Salt of volatile acid
H2SO4Sulfuric acid1
Brønsted acid
Nonvolatile acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
Rb2SO4Rubidium sulfate1
Conjugate base
Salt of non volatile acid
HClHydrogen chloride2
Conjugate acid
Volatile acid

Thermodynamic changes

Changes in standard condition

Reaction of rubidium chloride and sulfuric acid
ΔrG−1.89 kJ/mol
K2.14 × 100
pK−0.33
2RbClCrystalline solid + H2SO4Liquid
Rb2SO4Crystalline solid + 2HClGas
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
64.47−1.89222.55−51.37
per 1 mol of
32.23−0.945111.28−25.68
per 1 mol of
64.47−1.89222.55−51.37
per 1 mol of
64.47−1.89222.55−51.37
per 1 mol of
32.23−0.945111.28−25.68

Changes in aqueous solution (1)

Reaction of rubidium chloride and sulfuric acid
ΔrG71.83 kJ/mol
K0.26 × 10−12
pK12.58
2RbClIonized aqueous solution + H2SO4Ionized aqueous solution
Rb2SO4Ionized aqueous solution + 2HClGas
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
149.7071.83260.9
per 1 mol of
74.85035.91130.4
per 1 mol of
149.7071.83260.9
per 1 mol of
149.7071.83260.9
per 1 mol of
74.85035.91130.4

Changes in aqueous solution (2)

Reaction of rubidium chloride and sulfuric acid
ΔrG−0.03 kJ/mol
K1.01 × 100
pK−0.01
2RbClIonized aqueous solution + H2SO4Ionized aqueous solution
Rb2SO4Ionized aqueous solution + 2HClIonized 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
−0.01−0.030.1
per 1 mol of
−0.00500−0.01500.050
per 1 mol of
−0.0100−0.03000.10
per 1 mol of
−0.0100−0.03000.10
per 1 mol of
−0.00500−0.01500.050

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
RbCl (cr)-435.35[1]-407.80[1]95.90[1]52.38[1]
RbCl (g)-228.9[1]-247.3[1]249.56[1]36.82[1]
RbCl (ai)-418.32[1]-415.20[1]177.99[1]
H2SO4 (cr)
H2SO4 (l)-813.989[1]-690.003[1]156.904[1]138.91[1]
H2SO4 (ai)-909.27[1]-744.53[1]20.1[1]-293[1]
H2SO4 (l)
1 hydrate
-1127.621[1]-950.383[1]211.54[1]214.85[1]
H2SO4 (l)
2 hydrate
-1427.100[1]-1199.650[1]276.40[1]260.83[1]
H2SO4 (l)
3 hydrate
-1720.402[1]-1443.980[1]345.39[1]318.95[1]
H2SO4 (l)
4 hydrate
-2011.199[1]-1685.863[1]414.59[1]382.21[1]
H2SO4 (l)
6.5 hydrate
-2733.256[1]-2285.734[1]587.89[1]570.28[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
Rb2SO4 (cr)-1435.61[1]-1316.89[1]197.44[1]134.06[1]
Rb2SO4 (g)-1068.6[1]
Rb2SO4 (ai)-1411.60[1]-1312.50[1]263.2[1]
HCl (g)-92.307[1]-95.299[1]186.908[1]29.12[1]
HCl (ai)-167.159[1]-131.228[1]56.5[1]-136.4[1]
* (cr):Crystalline solid, (g):Gas, (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)