LITHIUM SULFIDE Li2S

Properties of lithium sulfide:

Light yellow, melts without decomposition. Readily soluble in water (hydrolysis of the strong anion). Crystalline hydrates are not. Reductant, in the moist state oxidized by atmospheric oxygen. Reacts with acids, non-metals.


Obtaining lithium sulfide Li2S:

2Li + S = Li2S (t>130° C)

2LiH + 2S = Li2S + H2S (300-50°C).

Li2O + H2S = Li2S + H2O (900-1000°C).

Li2SO4 + 4C (coke) = Li2S + 4CO (800-900°C).

Li2SO4 + 4H2 = Li2S + 4H2O (600-700°C).


Reactions with lithium sulfide Li2S:

Li2S (diluted) + 8H2O = 2[Li(H2O)4]+ + S2-

S2- + H2O ↔ HS- + OH-.

Li2S + 2HCl(diluted) = 2LiCl + H2S↑.

Li2S + 3H2SO4(conc.) = 2LiHSO4 + SO2↑ + S↓ + 2H2O.

Li2S + 4HNO3(conc.) = 2LiNO3 +  2NO2↑ + S↓ + 2H2O.

Li2S(cold) + H2S (saturated) = 2LiHS.

Li2S + 2 O2 = Li2SO4 (t>300°C).

2Li2S + 2 H2O (cold) + O2 = S↓ + 4LiOH.


 

Did you know?

The only letter that doesn't appear on theperiodic table is J.