Question

Copper(II) sulfide, CuS, is used in the development of aniline black dye in textile printing. What is the maximum mass of CuS which can be formed when 38.0 mL of 0.500 M CuCl2 are mixed with 42.0 mL of 0.600 M (NH4)2S

Answer 1

Explanation:

The chemical reaction equation will be as follows.

           $CuCl_{2} + (NH_{4})_{2}S \rightarrow 2NH_{4}Cl + CuS$

As 1 mole $CuCl_{2}$ reacts with 1 mole of $(NH_{4})_{2}S$

Hence, moles of $CuCl_{2}$ = Molarity × Volume (in mL)

                                              = 0.5 × 38.0 mL

                                              = 0.019 mol

Moles of $(NH_{4})_{2}S$ = Molarity × Volume (in mL)

                                           = 0.6 × 42.0 mL

                                           = 0.0252 mol

As moles of CuS is less than the moles of $(NH_{4})_{2}S$. This means that CuS is the limiting reagent.

Thus, maximum moles of CuS formed are 0.019 mol. As molar mass of CuS is 95.6 g/mol.

Therefore, maximum mass of CuS can be formed is $95.6 g/mol \times 0.019 mol$

                    = 1.8164 g

Thus, we can conclude that maximum mass of CuS formed is 1.8164 g.