Q25 / 160 · TS EAMCET 2019 (03 May Shift 1) · Chemistry

A current of $19296 \mathrm{C}$ is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (ing) of copper deposited at the cathode? (Molar mass of $\mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$ )

  • A
    3.17
  • B
    1.58
  • Correct answer
    C
    6.35
  • D
    0.79

Solution

Given, Charge used $=19296 \mathrm{C}$ Molar mass of $\mathrm{Cu}=63.5$ $\because \mathrm{Cu}$ in $\mathrm{CuSO}_4$ has $\mathrm{Cu}^{2+}$ charge means : $2 \times 96500 \mathrm{C}$ of charge give $=63.5 \mathrm{~g}$ of $\mathrm{Cu}$ Thus, $19296 \mathrm{C}$ of charge give $=\frac{635 \times 19296}{2 \times 96500}$ $=6.35 \mathrm{~g}$ of copper (Cu). Hence, option (3) is the correct answer.

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

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