# Calculate the quantity of electricity in coulombs required to liberate 10g of…

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**Calculate the quantity of electricity in coulombs required to liberate 10g of copper from a copper compound.**

**[Cu 64 F = 96500c]**

**A. 32395.5**

**B. 30156.3**

**C. 60784.5**

**D. 15196.6**

**QUICK ANSWER…**

**B**

**DETAILS… **

**According to Faraday’s law of electrolysis, the quantity of electricity needed to liberate 1 mole of any univalent ion is 1Faraday = 96500 coulombs.**

**Therefore, 1 mole of a divalent ion will be 2 Faraday = 2 x 96500 coulombs**

**And, 1 mole of a trivalent ion will be 3 Faraday = 3 x 96500 coulombs**

**But copper is normally divalent, that is, its ion is +2, hence,**

**1 mole of copper ion will need 2 x 96500 coulombs of electricity to liberate copper metal.**

**Now, 1 mole of copper is 64g,**

**This means 64g of copper will be liberated by 2 x 96500 coulombs of electricity,**

**Therefore, 10g of copper will be liberated by X coulombs.**

**Cross multiplying to find the value of X, we have:**

**X(64) = 10(2 x 96500)**

**64X = 1930000**

**X = 1930000/64 = 30,156.25 coulombs**

**Now for the right answer to the above question:**

**Option A is incorrect.****Option B is correct.****C is incorrect.****D is not the correct answer.**

**KEY-POINTS…**

**You may please note these/this:**

**1 mole of a univalent ion (like Na, K, H, Li, Cl, F, OH) will need 1Faraday of electricity to be liberated.****1 mole of a divalent ion (like Ca, Mg, Be, Zn, Cu) will need 2Faraday of electricity to be liberated.**

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**/ culled from 2016 JAMB-UTME Chemistry past question 31 /**

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