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Chemical reactions
Pb + 2HF → PbF2 + H2

Pb + 2HF → PbF₂ + H₂

Last updated: June 13, 2022

Reaction of lead and hydrogen fluoride: PbLead + 2HFHydrogen fluoride
⟶
PbF₂Lead(II) fluoride + H₂Hydrogen

The reaction of lead and hydrogen fluoride yields lead(II) fluoride and hydrogen. This reaction is an oxidation-reduction reaction and is classified as follows:

Table of contents

Reaction data

Chemical equation

Reaction of lead and hydrogen fluoride: PbLead + 2HFHydrogen fluoride
⟶
PbF₂Lead(II) fluoride + H₂Hydrogen

General equation

Reaction of reducing species and reducible species: Reducing speciesReducing agent + Reducible speciesOxidizing agent
⟶
ProductOxidation product + ProductReduction product

Reaction of active metal and acid: Active metalReducing agent + AcidOxidizing agent
⟶
SaltOxidation product + H₂Reduction product

Reaction of amphoteric metal and acid: Amphoteric metalReducing agent + AcidOxidizing agent
⟶
SaltOxidation product + H₂Reduction product

Oxidation state of each atom

Reaction of lead and hydrogen fluoride

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
Pb	Lead	1	Reducing	Reducing Active metal Amphoteric metal
HF	Hydrogen fluoride	2	Oxidizing	Reducible Acid

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
PbF₂	Lead(II) fluoride	1	Oxidized	– Salt
H₂	Hydrogen	1	Reduced	– Hydrogen

Thermodynamic changes

Changes in standard condition

Reaction of lead and hydrogen fluoride ◆ Δ_rG −70.7 kJ/mol K 2.43 × 10¹² pK −12.39: PbCrystalline solid + 2HFGas
⟶
PbF₂Crystalline solid + H₂Gas

	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	−121.8	−70.7	−171.2	–
per 1 mol of Lead	−121.8	−70.7	−171.2	–
per 1 mol of Hydrogen fluoride	−60.90	−35.4	−85.60	–
per 1 mol of Lead(II) fluoride	−121.8	−70.7	−171.2	–
per 1 mol of Hydrogen	−121.8	−70.7	−171.2	–

Changes in aqueous solution (1)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −3.0 kJ/mol K 3.35 × 10⁰ pK −0.53: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Gas

	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	–	−3.0	–	–
per 1 mol of Lead	–	−3.0	–	–
per 1 mol of Hydrogen fluoride	–	−1.5	–	–
per 1 mol of Lead(II) fluoride	–	−3.0	–	–
per 1 mol of Hydrogen	–	−3.0	–	–

Changes in aqueous solution (2)

Reaction of lead and hydrogen fluoride ◆ Δ_rG 14.6 kJ/mol K 0.28 × 10⁻² pK 2.56: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Un-ionized 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	–	14.6	–	–
per 1 mol of Lead	–	14.6	–	–
per 1 mol of Hydrogen fluoride	–	7.30	–	–
per 1 mol of Lead(II) fluoride	–	14.6	–	–
per 1 mol of Hydrogen	–	14.6	–	–

Changes in aqueous solution (3)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −23.5 kJ/mol K 1.31 × 10⁴ pK −4.12: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Crystalline solid + H₂Gas

	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	−23.8	−23.5	−1.0	–
per 1 mol of Lead	−23.8	−23.5	−1.0	–
per 1 mol of Hydrogen fluoride	−11.9	−11.8	−0.50	–
per 1 mol of Lead(II) fluoride	−23.8	−23.5	−1.0	–
per 1 mol of Hydrogen	−23.8	−23.5	−1.0	–

Changes in aqueous solution (4)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −5.9 kJ/mol K 1.08 × 10¹ pK −1.03: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Crystalline solid + H₂Un-ionized 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	−28.0	−5.9	445	–
per 1 mol of Lead	−28.0	−5.9	445	–
per 1 mol of Hydrogen fluoride	−14.0	−3.0	223	–
per 1 mol of Lead(II) fluoride	−28.0	−5.9	445	–
per 1 mol of Hydrogen	−28.0	−5.9	445	–

Changes in aqueous solution (5)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −39.0 kJ/mol K 6.80 × 10⁶ pK −6.83: PbCrystalline solid + 2HFIonized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Gas

	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	–	−39.0	–	–
per 1 mol of Lead	–	−39.0	–	–
per 1 mol of Hydrogen fluoride	–	−19.5	–	–
per 1 mol of Lead(II) fluoride	–	−39.0	–	–
per 1 mol of Hydrogen	–	−39.0	–	–

Changes in aqueous solution (6)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −21.4 kJ/mol K 5.61 × 10³ pK −3.75: PbCrystalline solid + 2HFIonized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Un-ionized 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	–	−21.4	–	–
per 1 mol of Lead	–	−21.4	–	–
per 1 mol of Hydrogen fluoride	–	−10.7	–	–
per 1 mol of Lead(II) fluoride	–	−21.4	–	–
per 1 mol of Hydrogen	–	−21.4	–	–

Changes in aqueous solution (7)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −59.5 kJ/mol K 2.65 × 10¹⁰ pK −10.42: PbCrystalline solid + 2HFIonized aqueous solution
⟶
PbF₂Crystalline solid + H₂Gas

	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	1.3	−59.5	204.0	–
per 1 mol of Lead	1.3	−59.5	204.0	–
per 1 mol of Hydrogen fluoride	0.65	−29.8	102.0	–
per 1 mol of Lead(II) fluoride	1.3	−59.5	204.0	–
per 1 mol of Hydrogen	1.3	−59.5	204.0	–

Changes in aqueous solution (8)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −41.9 kJ/mol K 2.19 × 10⁷ pK −7.34: PbCrystalline solid + 2HFIonized aqueous solution
⟶
PbF₂Crystalline solid + H₂Un-ionized 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	−2.9	−41.9	650	–
per 1 mol of Lead	−2.9	−41.9	650	–
per 1 mol of Hydrogen fluoride	−1.4	−20.9	325	–
per 1 mol of Lead(II) fluoride	−2.9	−41.9	650	–
per 1 mol of Hydrogen	−2.9	−41.9	650	–

Changes in aqueous solution (9)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −3.0 kJ/mol K 3.35 × 10⁰ pK −0.53: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Gas

	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	–	−3.0	–	–
per 1 mol of Lead	–	−3.0	–	–
per 1 mol of Hydrogen fluoride	–	−1.5	–	–
per 1 mol of Lead(II) fluoride	–	−3.0	–	–
per 1 mol of Hydrogen	–	−3.0	–	–

Changes in aqueous solution (10)

Reaction of lead and hydrogen fluoride ◆ Δ_rG 14.6 kJ/mol K 0.28 × 10⁻² pK 2.56: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Un-ionized aqueous solution + H₂Un-ionized 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	–	14.6	–	–
per 1 mol of Lead	–	14.6	–	–
per 1 mol of Hydrogen fluoride	–	7.30	–	–
per 1 mol of Lead(II) fluoride	–	14.6	–	–
per 1 mol of Hydrogen	–	14.6	–	–

Changes in aqueous solution (11)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −23.5 kJ/mol K 1.31 × 10⁴ pK −4.12: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Crystalline solid + H₂Gas

	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	−23.8	−23.5	−1.0	–
per 1 mol of Lead	−23.8	−23.5	−1.0	–
per 1 mol of Hydrogen fluoride	−11.9	−11.8	−0.50	–
per 1 mol of Lead(II) fluoride	−23.8	−23.5	−1.0	–
per 1 mol of Hydrogen	−23.8	−23.5	−1.0	–

Changes in aqueous solution (12)

Reaction of lead and hydrogen fluoride ◆ Δ_rG −5.9 kJ/mol K 1.08 × 10¹ pK −1.03: PbCrystalline solid + 2HFUn-ionized aqueous solution
⟶
PbF₂Crystalline solid + H₂Un-ionized 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	−28.0	−5.9	445	–
per 1 mol of Lead	−28.0	−5.9	445	–
per 1 mol of Hydrogen fluoride	−14.0	−3.0	223	–
per 1 mol of Lead(II) fluoride	−28.0	−5.9	445	–
per 1 mol of Hydrogen	−28.0	−5.9	445	–

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
Pb (cr)	0^[1]	0^[1]	64.81^[1]	26.44^[1]
Pb (g)	195.0^[1]	161.9^[1]	175.373^[1]	20.786^[1]
HF (l) x denotes undetermined zero point entropy	-299.78^[1]	–	75.40+x^[1]	–
HF (g)	-271.1^[1]	-273.2^[1]	173.779^[1]	29.133^[1]
HF (ai)	-332.63^[1]	-278.79^[1]	-13.8^[1]	-106.7^[1]
HF (ao)	-320.08^[1]	-296.82^[1]	88.7^[1]	–

* (cr):Crystalline solid, (g):Gas, (l):Liquid, (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
PbF₂ (cr)	-664.0^[1]	-617.1^[1]	110.5^[1]	–
PbF₂ (ai)	-666.9^[1]	-582.00^[1]	-17.2^[1]	–
PbF₂ (ao)	–	-596.6^[1]	–	–
H₂ (g)	0^[1]	0^[1]	130.684^[1]	28.824^[1]
H₂ (ao)	-4.2^[1]	17.6^[1]	577^[1]	–

* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-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	−70.7 kJ/mol
K	2.43 × 10¹²
pK	−12.39

Δ_rG	−3.0 kJ/mol
K	3.35 × 10⁰
pK	−0.53

Δ_rG	14.6 kJ/mol
K	0.28 × 10⁻²
pK	2.56

Δ_rG	−23.5 kJ/mol
K	1.31 × 10⁴
pK	−4.12

Pb + 2HF → PbF2 + H2

Reaction data

Chemical equation

General equation

Oxidation state of each atom

Reactants

Products

Thermodynamic changes

Changes in standard condition

Changes in aqueous solution (1)

Changes in aqueous solution (2)

Changes in aqueous solution (3)

Changes in aqueous solution (4)

Changes in aqueous solution (5)

Changes in aqueous solution (6)

Changes in aqueous solution (7)

Changes in aqueous solution (8)

Changes in aqueous solution (9)

Changes in aqueous solution (10)

Changes in aqueous solution (11)

Changes in aqueous solution (12)

Thermodynamic data of reactants

Thermodynamic data of products

References

List of references

Related categories

Type of reaction

General equation

Reactant

Product

Pb + 2HF → PbF₂ + H₂