TS EAMCET · Chemistry · Electrochemistry
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
- B 50
- C 1000
- D 100
Answer & Solution
Correct Answer
(B) 50
Step-by-step Solution
Detailed explanation
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…
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