The reaction between water and fluorine can be represented as:
\( 2F_{2(g)}+2H_{2}O_{(l)}\rightarrow 4H^{+}_{(aq)}+4F^{-}_{(aq)}+O_{2(g)} \)
This is an example of redox reaction
\( 2F_{2(g)}+2H_{2}O_{(l)}\rightarrow 4H^{+}_{(aq)}+4F^{-}_{(aq)}+O_{2(g)} \)
Water is getting oxidized to oxygen and fluorine is being reduced to fluoride ion.
The oxidation number of various species can be represented as:
\( 2F_{2(g)}+2H_{2}O_{(l)}\rightarrow 4H^{+}_{(aq)}+4F^{-}_{(aq)}+O_{2(g)} \)
Water is oxidized from (– 2) to zero oxidation state. An increase in oxidation state indicates oxidation of water.
Fluorine is reduced from zero to (– 1) oxidation state. A decrease in oxidation state indicates the reduction of fluorine.
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?