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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:

  1. Option A is incorrect.
  2. Option B is correct.
  3. C is incorrect.
  4. D is not the correct answer.
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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 /

Calculate the quantity of electricity in coulombs required to liberate 10g of... » QuizTablet
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