MHT CET · Chemistry · Electrochemistry
A solution of \(\mathrm{CuSO}_{4}\) is electrolysed using a current of \(1 \cdot 5\) amperes for 10 minutes. What mass of Cu is deposited at cathode ? (At. mass of \(\mathrm{Cu}=63 \cdot 7\) )
- A 0.395g
- B 0.150g
- C 0.637g
- D 0.297g
Answer & Solution
Correct Answer
(D) 0.297g
Step-by-step Solution
Detailed explanation
(D)
The half reaction at cathode is
\(\mathrm{Cu}_{\text {(aq) }}^{2+}+2 \mathrm{e}^{--} \longrightarrow \mathrm{Cu}_{(\mathrm{s})}\) Mole ratio \(=\frac{1}{2}, \mathrm{t}=10 \mathrm{~min}=600 \mathrm{~s}\)
Mass of \(\mathrm{Cu}\) deposited \(=\frac{\mathrm{I} \times \mathrm{t}}{96500} \times\) mole ratio \(\times\) molar mass of \(\mathrm{Cu}\)
\(=\frac{1.5 \times 600}{96500} \times \frac{1}{2} \times 63.7=0.297 \mathrm{~g}\)
The half reaction at cathode is
\(\mathrm{Cu}_{\text {(aq) }}^{2+}+2 \mathrm{e}^{--} \longrightarrow \mathrm{Cu}_{(\mathrm{s})}\) Mole ratio \(=\frac{1}{2}, \mathrm{t}=10 \mathrm{~min}=600 \mathrm{~s}\)
Mass of \(\mathrm{Cu}\) deposited \(=\frac{\mathrm{I} \times \mathrm{t}}{96500} \times\) mole ratio \(\times\) molar mass of \(\mathrm{Cu}\)
\(=\frac{1.5 \times 600}{96500} \times \frac{1}{2} \times 63.7=0.297 \mathrm{~g}\)
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