Which one of the following could not be liberated from a suitable electrolyte by the passage of 0.25 faraday of electricity through that electrolyte :

0.25 mole of Ag

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16gm of Cu

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2gm of O

_{2}

(g)

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2.8ltrs of H

_{2}

at STP

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Solution

The correct option is B 16gm of Cu
$0.25 f a r a d a y c h a r g e = 0.25 m o l e s o f e l e c t r o n s$
$A g^{+} + e^{-} \to A g$
$(A) 0.25 e^{-} l i b e r a t e s 0.25 m o l e s o f C u$
$(B) 16 g C u = \frac{16 \times 2}{63.5} = \frac{32}{64} = 0.5$
$∴ C u r e q u i r e s 0.5 m o l e s o f e^{-}$
$(C) 2 g o / o_{2} r e q u i r s \frac{2 \times 4}{32} = 0.25 m o l e$
$(D) 2.8 r u l e s H_{2} = \frac{2.1}{22.4} = 0.125$
1 mole $H_{2}$ require 2 mole $e^{-}$
$∴ m o l e s o f e^{-} r e q u i r e d = 0.125 \times 2 = 0.25$

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Which one of the following could not be liberated from a suitable electrolyte by the passage of 0.25 faraday of electricity through that electrolyte :

The correct option is B 16gm of Cu0.25faradaycharge=0.25molesofelectronsAg++e−→Ag(A)0.25e−liberates0.25molesofCu(B)16gCu=16×263.5=3264=0.5∴Curequires0.5molesofe−(C)2go/o2requirs2×432=0.25mole(D)2.8rulesH2=2.122.4=0.1251 mole H2 require 2 mole e−∴molesofe−required=0.125×2=0.25