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ZnCl2 + 2RbF 💧→ ZnF2↓ + 2RbCl

ZnCl₂ + 2RbF 💧→ ZnF₂↓ + 2RbCl

Last updated: June 13, 2022

Reaction of zinc chloride and rubidium fluoride: ZnCl₂Zinc chloride + 2RbFRubidium fluoride
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ZnF₂↓Zinc fluoride + 2RbClRubidium chloride

The reaction of zinc chloride and rubidium fluoride yields zinc fluoride and rubidium chloride. This reaction is an acid-base reaction and is classified as follows:

Precipitation reaction

Table of contents

Reaction data

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
ZnCl₂	Zinc chloride	1	Lewis acid	Very soluble in water
RbF	Rubidium fluoride	2	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
ZnF₂	Zinc fluoride	1	Lewis conjugate	Slightly soluble in water
RbCl	Rubidium chloride	2	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of zinc chloride and rubidium fluoride: ZnCl₂Crystalline solid + 2RbFCrystalline solid
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ZnF₂↓Crystalline solid + 2RbClCrystalline solid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−104.7	–	–	–
per 1 mol of Zinc chloride	−104.7	–	–	–
per 1 mol of Rubidium fluoride	−52.35	–	–	–
per 1 mol of Zinc fluoride	−104.7	–	–	–
per 1 mol of Rubidium chloride	−52.35	–	–	–

Changes in aqueous solution (1)

Reaction of zinc chloride and rubidium fluoride ◆ Δ_rG −8.7 kJ/mol K 3.34 × 10¹ pK −1.52: ZnCl₂Ionized aqueous solution + 2RbFIonized aqueous solution
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ZnF₂↓Crystalline solid + 2RbClIonized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	54.7	−8.7	213.9	–
per 1 mol of Zinc chloride	54.7	−8.7	213.9	–
per 1 mol of Rubidium fluoride	27.4	−4.3	107.0	–
per 1 mol of Zinc fluoride	54.7	−8.7	213.9	–
per 1 mol of Rubidium chloride	27.4	−4.3	107.0	–

Changes in aqueous solution (2)

Reaction of zinc chloride and rubidium fluoride ◆ Δ_rG −14.5 kJ/mol K 3.47 × 10² pK −2.54: ZnCl₂Un-ionized aqueous solution + 2RbFIonized aqueous solution
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ZnF₂↓Crystalline solid + 2RbClIonized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	–	−14.5	–	–
per 1 mol of Zinc chloride	–	−14.5	–	–
per 1 mol of Rubidium fluoride	–	−7.25	–	–
per 1 mol of Zinc fluoride	–	−14.5	–	–
per 1 mol of Rubidium chloride	–	−7.25	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
ZnCl₂ (cr)	-415.05^[1]	-369.398^[1]	111.46^[1]	71.34^[1]
ZnCl₂ (g)	-266.1^[1]	–	–	–
ZnCl₂ (ai)	-488.19^[1]	-409.50^[1]	0.8^[1]	-226^[1]
ZnCl₂ (ao)	–	-403.7^[1]	–	–
RbF (cr)	-557.7^[1]	–	–	–
RbF (g)	-331.4^[1]	-349.0^[1]	237.09^[1]	35.69^[1]
RbF (ai)	-583.79^[1]	-562.77^[1]	107.5^[1]	–
RbF (cr) 1.5 hydrate	-1013.8^[1]	–	–	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
ZnF₂ (cr)	-764.4^[1]	-713.3^[1]	73.68^[1]	65.65^[1]
ZnF₂ (ai)	-819.14^[1]	-704.64^[1]	-139.7^[1]	-167^[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]	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas

References

List of references

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
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list

Δ_rG	−8.7 kJ/mol
K	3.34 × 10¹
pK	−1.52

Δ_rG	−14.5 kJ/mol
K	3.47 × 10²
pK	−2.54

ZnCl2 + 2RbF 💧→ ZnF2↓ + 2RbCl

Reaction data

Chemical equation

General equation

Oxidation state of each atom