CHEM - Faraday and Mole Calculation Example 2

Chemistry, Faraday, Mole Calculations- IBID | DSE | GCE | IAL | AP Chemistry

April 30, 2018

Here is another example of mole calculation🧐

Calculate the quantity of electricity, in coulombs, needed to produce 18 cm³ of chlorine gas. *(1 Faraday=96500 coulombs)

Step 1:

Start by writing down the equation

2Cl^- → Cl₂ + 2e^-

Step 2:

Find the number of moles in the 18 cm³ of chlorine gas

Volume = Moles × Molar Volume

❗️❗️ Remember to use the same units (cm³)

By rearranging the above equation,

Moles = 18 cm³/ 24000 cm³ = 0.00075 moles

Step 3:

Note that electricity always refers to the flow of electrons

From the half equation, 2 electrons are needed to produce chlorine gas

Hence, 2e^-= 96500 × 2 = 193000 C

Final Step💪

Don't forget about the moles!

Multiply the number of coulombs by the amount of moles calculated earlier

193000 × 0.00075 = 144.75 Coulombs

Therefore, 144.75 Coulombs are required to produce 18 cm³ of chlorine gas

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