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:

Look up the relative atomic mass of copper on a modern periodic table: . Look up the Faraday's Constant: . This constant gives the amount of electrical charge on each mole of electrons.

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.)

What are the steps for finding the mass of copper that has been deposited.

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

Find the number of moles of electrons that have been supplied based on the charge supplied;  Find the number of moles of copper that have been reduced based on the number of moles of electrons supplied; andFind the mass of copper based on the number of moles of copper atoms reduced.What's the charge on the electrons supplied to this electrochemical cell?

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

.

In case

is in Amperes and is in seconds ,

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

For this electrochemical cell,

.

How many moles of electrons were supplied to this electrochemical cell?

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

.

.

How many moles of copper atoms have been deposited?

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,

.

What's the mass of that many copper atoms?

The Relative atomic mass of copper is .

.

The mass has escaped into a gas which you can not see so the law stays true.

As cooking food that has to go in the oven