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2AuCl3 + 3Mg(OH)2 → 3MgCl2 + 2Au(OH)3

The reaction of gold(III) chloride and magnesium hydroxide yields magnesium chloride and gold(III) hydroxide. 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
AuCl3Gold(III) chloride2
Brønsted acid
Salt of weak base
Mg(OH)2Magnesium hydroxide3
Brønsted base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
MgCl2Magnesium chloride3
Conjugate acid
Salt of strong base
Au(OH)3Gold(III) hydroxide2
Conjugate base
Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of gold(III) chloride and magnesium hydroxide
2AuCl3Crystalline solid + 3Mg(OH)2Crystalline solid
3MgCl2Crystalline solid + 2Au(OH)3Crystalline solidprecipitated
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
235.5
per 1 mol of
117.8
78.50
per 1 mol of
78.50
117.8

Changes in standard condition (2)

Reaction of gold(III) chloride and magnesium hydroxide
2AuCl3Crystalline solid + 3Mg(OH)2Amorphous solidprecipitated
3MgCl2Crystalline solid + 2Au(OH)3Crystalline solidprecipitated
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
223.3
per 1 mol of
111.7
74.43
per 1 mol of
74.43
111.7

Changes in aqueous solution (1)

Reaction of gold(III) chloride and magnesium hydroxide
2AuCl3Crystalline solid + 3Mg(OH)2Crystalline solid
3MgCl2Ionized aqueous solution + 2Au(OH)3Un-ionized 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
per 1 mol of
per 1 mol of

Changes in aqueous solution (2)

Reaction of gold(III) chloride and magnesium hydroxide
2AuCl3Crystalline solid + 3Mg(OH)2Amorphous solidprecipitated
3MgCl2Ionized aqueous solution + 2Au(OH)3Un-ionized 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
per 1 mol of
per 1 mol of

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
AuCl3 (cr)-117.6[1]
AuCl3 (cr)
2 hydrate
-715.0[1]
Mg(OH)2 (cr)-924.54[1]-833.51[1]63.18[1]77.03[1]
Mg(OH)2 (am)
precipitated
-920.5[1]
Mg(OH)2 (g)-561[1]
Mg(OH)2 (ai)-926.84[1]-769.4[1]-159.4[1]
* (cr):Crystalline solid, (am):Amorphous solid, (g):Gas, (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
MgCl2 (cr)-641.32[1]-591.79[1]89.62[1]71.38[1]
MgCl2 (g)-400.4[1]
MgCl2 (ai)-801.15[1]-717.1[1]-25.1[1]
MgCl2 (cr)
1 hydrate
-966.63[1]-861.74[1]137.2[1]115.27[1]
MgCl2 (cr)
2 hydrate
-1279.72[1]-1118.00[1]179.9[1]159.20[1]
MgCl2 (cr)
4 hydrate
-1898.99[1]-1623.29[1]264.0[1]241.42[1]
MgCl2 (cr)
6 hydrate
-2499.02[1]-2114.64[1]366.1[1]315.06[1]
Au(OH)3 (cr)
precipitated
-424.7[1]-316.92[1]189.5[1]
Au(OH)3 (ao)-283.37[1]
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (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)