When dealing with questions related to mole calculations, following a few simple steps can make it easier to solve them. 🤔

🤓Here is an example:

**1.57 calculate the amounts of the products of the electrolysis of molten salts and aqueous solutions**

One faraday is 96500 coulombs. It is also one mole of electrons.

If current of 0.2 Amps is passed through copper(II) sulphate for two hours, how much copper do you get?

**Step 1:**

Start by writing out the equation

**Cu ^{2+} + 2e **→

**Cu**

**Step 2:**

Find out the coulombs of electrons flowing

**Charge (coulomb, C) = Current (ampere, A) × Time (second, s)**.

*Remember to convert the time into seconds !

**Therefore, Charge = 0.2 × 7200 = 1440 coulombs**

**Step 3:**

Convert Coulombs into moles of electrons

**Moles = Coulombs / faraday**

**Moles = 1440/96500 = 0.015**

**Step 4:**

Find the moles of the product using the **scale factor**

*From the equation, for every **2 moles of electrons**, there will be** 1 copper.**

**Scale factor = moles of product/moles of electrons = 1/2**

**Thus, there are 0.015 × 1/2 = 0.0075 moles of Cu**

**LAST STEP**👏

Convert moles into mass

**Mass = Moles × **

**Molar Mass**

**The mass of Cu = 0.0075 × 63.5 = 0.48 g**

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