A student is given 1.525 g of pure CuO. To recover the Cu present in the compound, the dark powdery solid was dissolved in 15.0 mL of 6 M HCl, the solution diluted with 50.0 mL of water, and 0.50 g of Mg was added. Was this enough Mg to displace all the ions from the solution

The amount of Mg was enough

Explanation:

In this case, we have to start with the reaction between and , so:

If we check the reaction is already balanced. Now, we can do some stoichiometry to calculate the amount of Mg. The first step is the number of moles of . To this we have to calculate the molar mass of first, so:

Cu: 63.55 g/mol and O: 16 g/mol. So, (63.55+16)= 79.55 g/mol.

Now, we can calculate the moles:

The molar ratio between and is 1:1, so:

.

Now we can calculate the mass of Mg if we know the atomic mass of Mg (24.305 g/mol). So:

With this in mind, the student added enough Mg to recover all the Cu.

Note: The HCl doesn't take a role in the reaction. The function of HCl is to dissolve the .

I hope it helps!

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