Explanation:
The chemical reaction equation will be as follows.
![CuCl_{2} + (NH_{4})_{2}S \rightarrow 2NH_{4}Cl + CuS](https://tex.z-dn.net/?f=CuCl_%7B2%7D%20%2B%20%28NH_%7B4%7D%29_%7B2%7DS%20%5Crightarrow%202NH_%7B4%7DCl%20%2B%20CuS)
As 1 mole
reacts with 1 mole of
Hence, moles of
= Molarity × Volume (in mL)
= 0.5 × 38.0 mL
= 0.019 mol
Moles of
= Molarity × Volume (in mL)
= 0.6 × 42.0 mL
= 0.0252 mol
As moles of CuS is less than the moles of
. 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](https://tex.z-dn.net/?f=95.6%20g%2Fmol%20%5Ctimes%200.019%20mol)
= 1.8164 g
Thus, we can conclude that maximum mass of CuS formed is 1.8164 g.