Calcium is obtained industrially by electrolysis of molten${\mathbf{CaCl}}_{\mathbf{2}}$and is used in aluminium alloys. How many coulombs are needed to produce 10.0 gof Cametal? If a cell runs at 15 A, how many minutes will it take to produce 10.0 gof Ca(s)?

The process of dissolving ionic compounds into their constituent components by delivering a direct electric current through the complex in a fluid form is known as electrolysis. At the cathode, cations are reduced, whereas anions are oxidized.

To get the charge, convert the mass required to moles of electrons. There are two electrons involved in reducing ${\mathrm{Ca}}^{2+}\to \mathrm{Ca}$.

$10.0\mathrm{gCa}\times \frac{1\mathrm{molCa}}{10.01\mathrm{gCa}}\times \frac{2{\mathrm{mole}}^{-}}{1\mathrm{molCa}}=0.50{\mathrm{mole}}^{-}$

Multiply by Faraday's constant to get the charge.

$0.50{\mathrm{mole}}^{-}\times \frac{96500\mathrm{C}}{{\mathrm{mole}}^{-}}=48,238\mathrm{C}$

Therefore, the value for the charge is obtained as $48,238\mathrm{C}$.

Given the current, divide the charge needed by the current to get the time.

$48,238\mathrm{C}\times \frac{1\mathrm{s}}{15\mathrm{C}}=3215.9\mathrm{s}$

Convert to minutes.

$321.59\mathrm{s}\times \frac{1\min }{60\mathrm{s}}=53.60\min$

Therefore, the value for time is obtained as $53.60\min$.