# 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 0.50g of Mg was added. was this enough Mg to displace all the Cu2+ ions from the solution?A. If there is not enough Mg present, how much more Mg metal would be needed (Minimum)?B. If there was enough Mg to displace the Cu, how much 6 M HCl (in mL) would be required to decompose the excess Mg present?

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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 0.50g of Mg was added. was this enough Mg to displace all the Cu2+ ions from the solution?

A. If there is not enough Mg present, how much more Mg metal would be needed (Minimum)?

B. If there was enough Mg to displace the Cu, how much 6 M HCl (in mL) would be required to decompose the excess Mg present?

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Step 1

CuO + 2 HCl ------> CuCl2 + H2O

As per the balanced chemical equation given,

the theoretical moles of CuO : HCl = 1 : 2

Calculating the actual moles of reactants based on data given in the question:

Actual moles of CuO = Given mass mass/molar mass

= 1.525/79.546

= 0.0191713 mol

Actual moles of HCl = 15.0/1000 x 6

= 0.09 mol

Actual moles of CuO : HCl = 0.0191713: 0.09 = 1 : 4.695

HCl is in excess as per the calculations and hence CuO is the limiting reagent.

So, the reaction would proceed forward as per the amount of CuO.

Moles of CuCl2 = moles of CuO = 0.0191713 mol

Step 2

The reaction between Mg and CuCl2:

Mg + CuCl2 -----------> MgCl2 + Cu

From the balan...

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### Redox Reactions 