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Calculate the number of moles of electrons required to deposit 6.35 g of copper on a...

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mahmuda092569 | Student | eNoter

Posted February 7, 2011 at 3:01 AM via web

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Calculate the number of moles of electrons required to deposit 6.35 g of copper on a metal surface. (Ar: Cu = 63.5)

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ndnordic | High School Teacher | (Level 2) Associate Educator

Posted February 7, 2011 at 3:05 AM (Answer #1)

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To solve this type of problem, first determine the number of moles of copper produced.

moles = mass/elemental mass = 6.35/63.5 = 0.1 moles

Now write the reaction taking place, and assume you have a copper +2 ion in solution.

Cu^+2 + 2 e^-1 = Cu

This means that it takes two moles of electrons for every mole of copper that has been reduced.

Since you produced 0.1 moles of copper, you had to use 0.2 moles of electrons.

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