| Direction (Q. Nos. 56): Electrolysis involves electronation and de-electronation al the respective electrodes. Anode of electrolytic cell is the electrode at winch de-electronation takes place whereas at cathode electronation is noticed. If two or more ions of same charge are to be electronated or de-electronated, the ion having lesser discharge potential is discharged. Discharge potential of an ion refers for \[{{E}^{o}}{{\,}_{OP}}\] or \[{{E}^{o}}_{RP}\] as the case may be. The products formed at either electrode is given in terms of Faraday?s law of electrolysis, i.e., \[W=\frac{Eit}{96500}\] |
A) 1 : 2
B) 2 : 1
C) 1 : 3
D) 3 : 1
Correct Answer: C
Solution :
At anode \[\therefore \] \[PQ=PR+RQ=1+2=3\,m\] (2 moles) \[{{\mu }_{e}}=0.14\,{{m}^{2}}{{V}^{-1}}{{s}^{-1}},\] (1 mole) Thus, at anode, 2 moles \[{{n}^{e}}=1.5\times {{10}^{16}}{{m}^{-3}},\] and 1 mole \[l=10\,cm=0.1\,m,\] is formed. At cathode \[A=1.0\times {{10}^{-4}}{{m}^{2}}\] i.e., 1 mole of \[V=2\] is liberated. Thus, ratio of gases at cathode and anode is 1 : 3.
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