1.

22.2 gm Sn is deposited on electrode when 2 ampere current is pass through molten tin salt solution for 2 hours. So what is the oxidation state of Sn in salt ? (Sn=119 gm mol^(-1))

Answer»

`-2`
`+2`
`+3`
`+4`

Solution :(i) Required electricity=`Q=Ixxt`
`=(2amp.)(5xx3600)` SECOND
`=(2xx5xx3600)/(96500)` Faraday
`=(72)/(193)` Faraday
and 22.2 gm `Sn=(22.2)/(119)` mole Sn
(II) So, `(72)/(193)` faraday give `(22.2)/(119)` mole Sn
`=(1xx22.2)/(119)xx(193)/(72)=0.50` mole Sn
So, 1F GIVES 0.50 mole Sn and 1 mole Sn required 2F.
So oxidation state of Sn is +2.


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