How much electricity in terms of Faraday is required to produce 40g of Ca from molten CaCl₂?

2F

The balanced equation for the electrolysis of molten \(CaCl_2\) is:

\(Ca^{2+} + 2e^- → Ca\)

The molar mass of Ca is 40 g/mol, so 40 g of Ca corresponds to 1 mol of Ca.

From the balanced equation, it can be seen that 2 moles of electrons are required to produce 1 mole of Ca.

So, the amount of electricity required to produce 1 mol of Ca is 2 F (Faraday).

Therefore, the amount of electricity required to produce 40 g of Ca is:

2 F/mol x 1 mol = 2 F

So, 2 Faraday of electricity is required to produce 40g of Ca from molten \(CaCl_2\).