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kotykmax [81]
3 years ago
8

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
Chemistry
1 answer:
ikadub [295]3 years ago
3 0

Answer:

The amount of Mg was enough

Explanation:

In this case, we have to start with the <u>reaction</u> between Mg and CuO, so:

CuO~+~Mg~->~MgO~+~Cu

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

1.525~g~CuO\frac{1~mol~CuO}{79.55~g~CuO}=0.0192~mol~CuO

The <u>molar ratio</u> between Mg and CuO is 1:1, so:

0.0192~mol~CuO=0.0192~mol~Mg.

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

0.0192~mol~Mg\frac{24.305~g~Mg}{1~mol~Mg}=0.466~g~Mg

<u>With this in mind, the student added enough Mg to recover all the Cu.</u>

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

I hope it helps!

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