Electrochemical equivalent for copper is `3.2xx10^(-7) kg C^(-1)` An electric current of 3.0 A is passed through a copper voltamater for one minture .How much will be deposited during electrolysis?
The reaction taking place at anode is :
`underset(71.0 g)(2Cl^(-)) rarr underset((71.0 g),("1 mole"))(Cl_(2))+underset(2xx96500" coulomb")(2e^(-))`
`Q=I xx t=100 xx 5xx 60xx 60` coulomb
The amount of chlorine liberated by passing...
Amount of charge passed `=1.70xx230` coulomb
Amount of actual charge passed `=90/100xx1.70xx230`
`=351.9` coulomb
No. of moles of Zn deposited by passing 351.9 coulomb of charge
`=1/(2xx96500)xx351.9=0.000182`
Molarity of `Zn^(2+)`...
Correct Answer - C
`underset(1" mole")(Na^(+))+underset(1" faraday")(e^(-)to)Na(s)`
`AP^(+)+underset(1" faraday")(3e^(-)to)Al(s)`
No. of mole of `Al=(1)/(3)` mole