The electricity required to produce 20.0 g of calcium from molten CaCl2 is (Given: Molar mass of Ca=40 g mol−1.

The electricity required to produce 20.0 g of calcium from molten ${CaCl}_{2}$ is (Given: Molar mass of $Ca = 40 g {mol}^{- 1})$ .

A
(0.5 mol) F
B
(1.0 mol) F
C
(1.5 mol) F
D
(2.0 mol) F

Solution:

Amount of Ca to be deposited, $n = \frac{m}{M} = \frac{20.0 g}{40 g {mol}^{- 1}} = 0.5 mol .$

Since each ${Ca}^{2 +}$ 10n requires $2 e^{-}$ to produce Ca, the quantity of electricity required will be $(2 \times 0.5 mol) F, i.e. (1.0 mol) F$ .

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