Question

What type of reaction is the following:

3Cu3CuS +2Al −> Al2​S3​+3Cu

Answer 1

Answer:

Answer: 14 g of copper metal we can produce if we begin the reaction with 35.00 g of solid aluminum metal and 35.00 g of aqueous copper (II) sulfate

Explanation:

Looks like the real equation is

2Al + 3CuSO_4 => 3Cu + Al_2(SO_4)_32Al+3CuSO

4

=>3Cu+Al

2

(SO

4

)

3

CuS -- is not copper (II) sulfate and is not soluble in water.

First find the amounts of reagents given to find out which reagent is in excess:

\nu = m/Mν=m/M

\nu (Al) = 35/27 = 1.3 (mol)ν(Al)=35/27=1.3(mol)

\nu (CuSO_4) = 35/160 = 0.21875 (mol)ν(CuSO

4

)=35/160=0.21875(mol)

As 2 mol of Al require 3 mol of CuSO4, then 1.3 mol of Al react with 1.95 mol of CuSO4, but we have less. So we calculate the mass of copper using CuSO4.

1 mol of CuSO4 contains 1 mol of Cu, then 0.21875 mol of CuSO4 contains 0.21875 mol of Cu.

m = M * \num=M∗ν

m(Cu) = 64 * 0.21875 = 14 (g)m(Cu)=64∗0.21875=14(g)

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