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Properties of substance:

zinc

Group of substances:

inorganic

Physical appearance:

hexagonal metal

Empirical formula (Hill's system for organic substances):

Zn

Structural formula as text:

Zn

Molar/atomic mass: 65.38

Melting point (°C):

419.58

Boiling point (°C):

906.2

Solubility (g/100 g of solvent):

hydrazine: insoluble [Ref.]
mercury: 2.2 (18°C) [Ref.]
water: 0.000072 (25°C) [Ref.]

Numerical data:

Superconducting temperature (K): 0.851

Density:

7.133 (20°C, g/cm3)
6.66 (419.5°C, d4)
6.59 (500°C, g/cm3)
6.4 (800°C, g/cm3)

Reactions:

  1. [Ref.1]
    Zn + H2O → ZnO + H2
  2. Yeild 75-81%. [Ref.1aster]
    C6H5COCH3 + CH3CHBrCOOC2H5 + Zn → C6H5C(CH3)(OZnBr)CH(CH3)COOC2H5
    C6H5C(CH3)(OZnBr)CH(CH3)COOC2H5 + H2SO4 → C6H5C(CH3)(OH)CH(CH3)COOC2H5 + ZnSO4 + HBr
  3. Yeild 93%. [Ref.1aster]
    C6H5Br + 2NH4Cl + Zn → C6H6 + ZnCl2 + NH4Br + NH3
  4. Yeild 96%. [Ref.1aster]
    HOC6H5Cl + NH4Cl + Zn → HOC6H6 + ZnCl2 + NH3
  5. Yeild 95%. [Ref.1aster]
    CH3(CH2)5Br + 2NH4Cl + Zn → CH3(CH2)4CH3 + ZnCl2 + NH4Br + NH3
  6. Yeild 90%. [Ref.1, Ref.2aster]
    C6H5COCH2CH2COOH + 2Zn + 4HCl → C6H5CH2CH2CH2COOH + 2ZnCl2 + H2O
  7. [Ref.1]
    4Zn + 10HNO3 (0,5%) → 4Zn(NO3)2 + NH4NO3 + 3H2O
  8. [Ref.1, Ref.2]
    5Zn + 12HNO3 (6-10%) → 5Zn(NO3)2 + N2 + 6H2O
  9. [Ref.1]
    4Zn + 10HNO3 (20%) → 4Zn(NO3)2 + N2O + 5H2O
  10. [Ref.1]
    3Zn + 8HNO3 (40%) → 3Zn(NO3)2 + 2NO + 4H2O
  11. [Ref.1]
    3Zn + 8HNO3 (40%) → 3Zn(NO3)2 + 2NO + 4H2O
  12. [Ref.1, Ref.2]
    Zn + 4HNO3 (68%) → Zn(NO3)2 + 2NO2 + 2H2O
  13. [Ref.1]
    Zn + 2NaOH + 2H2O → Na2[Zn(OH)4] + H2
  14. [Ref.1]
    Zn + 2HCl → ZnCl2 + H2
  15. [Ref.1, Ref.2]
    Zn + H2SO4 → ZnSO4 + H2

Vapour pressure (Torr):

0.01 (345°C)
0.1 (408°C)
1 (490°C)
10 (596°C)
100 (738°C)

Electrode potential:

Zn2+ + e- → Zn+, E = -2.3 V (water, 25°C)
Zn2+ + e- → Zn, E = -1.05 V (formic acid, 25°C)
Zn2+ + e- → Zn, E = -0.76 V (water, 25°C)
Zn2+ + e- → Zn, E = -0.74 V (methanol, 25°C)
Zn2+ + e- → Zn, E = -0.74 V (acetonitrile, 25°C)
Zn2+ + e- → Zn, E = -0.64 V (ethanol, 25°C)
Zn2+ + e- → Zn, E = -0.53 V (ammonia liquid , -50°C)

Surface tension (mN/m):

780 (419.5°C)
778 (500°C)
764 (600°C)
754 (670°C)

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

0 (s)

Standard molar Gibbs energy of formation ΔfG0 (298.15 K, kJ/mol):

0 (s)

Standard molar entropy S0 (298.15 K, J/(mol·K)):

41.63 (s)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

25.44 (s)

Molar enthalpy (heat) of fusion ΔfusH (kJ/mol):

7.24

Enthalpy (heat) of vaporization ΔvapH (kJ/mol):

115.3

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

130.5 (g)

Standard molar entropy S0 (298.15 K, J/(mol·K)):

160.9 (g)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

20.8 (g)

References:

  1. Герасимов Я.И., Древинг В.П., Еремин Е.Н.. Киселев А.В., Лебедев В.П., Панченков Г.М., Шлыгин А.И. Курс физической химии. - Т.2. - М.: Химия, 1973. - pp. 528 [Russian]
  2. Гурвич Я.А. Справочник молодого аппаратчика-химика. - М.: Химия, 1991. - pp. 52 [Russian]
  3. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 62 [Russian]
  4. Неорганические синтезы. - Сб. 1. - М.: ИИЛ, 1951. - pp. 10 [Russian]
  5. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 112 [Russian]
  6. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 593-594 [Russian]
  7. Успехи химии. - 1997. - Т.66, №2. - pp. 112 [Russian]
  8. Химическая энциклопедия. - Т. 5. - М.: Советская энциклопедия, 1999. - pp. 377-379 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru