Question
A current of 1.50A was passed through an electrolytic cell containing AgNO3 solution with inert electrodes. The weight of Ag deposited was 1.50g. How long did the current flow?
✓
Answer
$\text{Ag}^++\text{e}^-\xrightarrow{ \ \ \ \ \ \ }\text{Ag}$
Quantity of charge required to deposit 108g of silver = 96500C
$\therefore$ Quantity of charge required to deposit 1.50g of silver $=\frac{96500}{108}\times1.50=1340.28\text{C}$
$\text{t}=\frac{\text{Q}}{\text{I}}$
$\therefore$ Time taken $=\frac{1340.28}{1.50}=893.52\text{s}$
Quantity of charge required to deposit 108g of silver = 96500C
$\therefore$ Quantity of charge required to deposit 1.50g of silver $=\frac{96500}{108}\times1.50=1340.28\text{C}$
$\text{t}=\frac{\text{Q}}{\text{I}}$
$\therefore$ Time taken $=\frac{1340.28}{1.50}=893.52\text{s}$
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