Calculate the amount of electricity required in coulombs to convert 0.08 mol of $\mathrm{MnO}_4^{-}$to…

Calculate the amount of electricity required in coulombs to convert 0.08 mol of $\mathrm{MnO}_4^{-}$to $\mathrm{Mn}^{2+}$.
  1. 96500 C
  2. 38600 C
  3. 48250 C
  4. 19300 C

Solution

The reaction is $\mathrm{MnO}_4^{-}+5 \mathrm{e}^{-} \longrightarrow \mathrm{Mn}^{2+}$
For reduction of 1 mole, 5 F electricity is required $\therefore \quad$ For 0.08 mole, 0.4 F electricity is required. $\begin{aligned} & 1 \mathrm{~F}=96500 \mathrm{C} \\ \therefore \quad & 0.4 \mathrm{~F}=96500 \times 0.4=38600 \mathrm{C} \end{aligned}$

Asked in: MHT CET 2024 (04 May Shift 1)

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