Saline hydrides [i.e.,LiH, NaH etc.] react with water to form hydrogen gas
And a base. The chemical equation to represent this reaction is
\( MH_{(g)}+H_{2}O_{(aq)}\rightarrow MOH_{(aq)}+H_{2(g)} \)
This reaction behaves violent and also fire is produced from this.
Dioxygen weights lighter than CO2. CO2 is commonly used as fire extinguisher as it covers the fire like blanket and inhibits the dioxygen supply, thereby dousing the fire.
It can be used in this scenario also. It weights higher than di hydrogen and effective in isolating the burning surface from dioxygen and dihydrogen.
Answered by Pragya Singh | 1 year agoWhat do you understand by the terms :
(i) Hydrogen economy
(ii) Hydrogenation
(iii) ‘syngas’
(iv) Water-gas shift reaction
(v) Fuel cell?
Do you expect different products in solution when aluminium (III) chloride and potassium chloride treated separately with
(i) alkaline water
(ii) acidified water, and
(iii) normal water. Write equations wherever necessary.
What do you expect the nature of hydrides is, if formed by elements of atomic numbers 15, 19, 23 and 44 with dihydrogen? Compare their behaviour with water.
How can saline hydrides remove traces of water from organic compounds?