6. how to calculate the mass of copper that can be plated out of a 1.0 m cu(no3)2 solution using a current of 0.75 a for 5.0 minutes?

Approximately 0.074 grams.

Explanation:

How does the electroplating works for copper? Copper exists as copper(II) ions in the copper(II) nitrate solution. It takes two moles of electrons to reduce one mole of copper(II) ions to metallic copper .

. (Reduction half of the ionic equation.)

Start by finding the charge on the electrons that have been supplied to this electrochemical cell. After that,

For a constant direct current , the charge that has been delivered in time is equal to

.

In case

will be in Coulombs (which is the same as .)

For this electrochemical cell,

.

The Faraday's Constant gives the size of charge (in Coulombs) on one mole of electrons.

.

.

Assume that copper(II) ions are in excess. Refer to the reduction half-equation, it takes two moles of electrons to deposit one mole of metallic copper.

.

. As a result,

.

The Relative atomic mass of copper is .

.

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