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$0.066 \mathrm{~g}$ 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?
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The correct answer is:
$3.3 \times 10^{-4}$
$w=z \cdot i \cdot t$
$z=\frac{w}{i \times t}=\frac{0.66}{2 \times 100}=3.3 \times 10^{-4} \mathrm{~g} /$ coulomb
$z=\frac{w}{i \times t}=\frac{0.66}{2 \times 100}=3.3 \times 10^{-4} \mathrm{~g} /$ coulomb
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