Q12 / 160 · AP EAMCET 2006 · Chemistry

What is the time (in sec) required for depositing all the silver present in $125 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}{ }_3$ solution by passing a current of $241.25 \mathrm{~A}$ ? (1F $=96500$ coulombs $)$

  • A
    10
  • Correct answer
    B
    50
  • C
    1000
  • D
    100

Solution

Given $125 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_3$ solution. It means that $\because 1000 \mathrm{~mL}$ of $\mathrm{AgNO}_3$ solution contains $=108 \mathrm{~g} \mathrm{Ag}$ $\therefore 125 \mathrm{~mL}$ of $\mathrm{AgNO}_3$ solution contains $=\frac{108 \times 125}{1000} \mathrm{~g} \mathrm{Ag}$ $=13.5 \mathrm{~g} \mathrm{Ag}$ $\because 108 \mathrm{~g}$ of $\mathrm{Ag}$ is deposited by $96500 \mathrm{C}$ $\therefore 13.5 \mathrm{~g}$ of $\mathrm{Ag}$ is deposited by $=\frac{96500}{108} \times 13.5$ $=12062.5 \mathrm{C}$ $Q=i t$ $t=\frac{Q}{i}=\frac{12062.5}{241.25}=50$

Hence, the correct answer is option: 'B'.

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