Q23 / 160 · AP EAMCET 2024 (20 May Shift 1) · Chemistry

Figure

  • A
    $0.195$
  • Correct answer
    B
    $0.39$
  • C
    $0.78$
  • D
    $1.56$

Solution

Given:- Time $(\mathrm{t})=10 \mathrm{~min}=10 \times 60=600 \mathrm{sec}$. Current $(A)=2.0 \mathrm{Amp}$. The reaction at Cathode as:- $\mathrm{Cu}^{+2}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}$ $2 \mathrm{e}^{-}$are transfer in this reaction The mass of copper is $63.5 \mathrm{~g} \mathrm{~mol}^{-1}$ Charge $=$ time $\times$ current Charge $=600 \times 2=1200 \mathrm{C}$ Now the mass of copper deposited $=\frac{\text { molar mass } \times \text { charge }}{\text { electron transferred } \times \text { Faradey constant }}$ $\Rightarrow \frac{63.5 \times 1200}{2 \times 96500}=\frac{762}{1930}=0.39 \mathrm{~g}$

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

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