$0.066 \mathrm{~g}$ of metal was deposited when a current of 2 ampere is passed through a metal ion solution…

$0.066 \mathrm{~g}$ of metal was deposited when a current of 2 ampere is passed through a metal ion solution for 100 seconds. What is the electrochemical equivalent (in gram coulomb $^{-1}$ ) of the metal?
  1. $3.3 \times 10^{-6}$
  2. $3.3 \times 10^{-4}$
  3. $0.033$
  4. $3.3$

Solution

$w=z \cdot i \cdot t$ $z=\frac{w}{i \times t}=\frac{0.066}{2 \times 100}=3.3 \times 10^{-4} \mathrm{~g} /$ coulomb .

Asked in: JEE-TOPICTESTS-CHEMISTRY

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