Calculate the mass of ' Ca ' deposited at cathode by passing 0.8 ampere current through molten…

Calculate the mass of ' Ca ' deposited at cathode by passing 0.8 ampere current through molten $\mathrm{CaCl}_2$ in 60 minutes. [Molar mass of $\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}$ ]
  1. 0.4 g
  2. 0.5 g
  3. 0.6 g
  4. 0.7 g

Solution

$\begin{aligned} & \mathrm{Ca}_{(\mathrm{aq})}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Ca}_{(\mathrm{s})} \\ & \text { Mole ratio }=\frac{1 \mathrm{~mol}}{2 \mathrm{~mol} \mathrm{e}^{-}} \\ & \mathrm{W}=\frac{\mathrm{I}(\mathrm{A}) \times \mathrm{t}(\mathrm{s})}{96500\left(\mathrm{C} / \mathrm{mole}^{-}\right)} \times \text {mole ratio } \times \mathrm{M}_{\mathrm{Ca}} \\ & =\frac{0.8 \times 60 \times 60}{96500} \times \frac{1}{2} \times 40=0.6 \mathrm{~g}\end{aligned}$

Asked in: MHT CET 2024 (15 May Shift 1)

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