LITHIUM HYDRIDE LiH

White, light and melts without decomposition, decomposes on further heating. A strong reducing agent, reacts with water, acids, non-metals, oxides of nonmetals.


Obtaining lithium hydride LiH:

2 Li + H2 = 2 LiH (500-700° C).

Li3N + 3H2 = 3 LiH + NH3 (300° C, impurity Li2NH).


Reactions  lithium hydride LiH:

2 Li + H2 = 2 LiH (500-700° C).

Li3N + 3 H2 = 3 LiH + NH3 (300° C, impurity Li2NH).

2 LiH = 2Li + H2 (450° C).

LiH + H2O = LiOH + H2↑.

LiH + HCl (diluted) = LiCl + H2↑ (normal temp.).

2 LiH + O2 = 2 LiOH (t> 500° C).

LiH + Cl2 = LiCl + HCl (400-450° C).

2 LiH + 2S = Li2S + H2S (300—350° C).

3 LiH + N2 = Li3N +NH3 (500—600° C).

2 LiH + 4C (graphite) = Li2C2 + C2H2 (400° C).

2 LiH + 2SO2 = Li2SO4 + H2S (200° C).

LiH + CO2 = Li(HCOO) [250° C, р].

4 LiH + 3SiO2 = 2Li2SiO3 + Si + 2H2 (500° C).

LiH + NH3 = LiNH2 + H2 (350° C).

LiH + NH3(liquid) = LiNH2↓ + H2↑ (- 40° C).

4 LiH + AlCl3 = Li[AlH4] + 3LiCl↓ (in ether).

2 LiH (liquid) → Electrolysis → 2Li(on cathode) + H2↑(on anode).


 

Did you know?

Elements in horizontal rows are called periods.