Respuesta :
Explanation:
The chemical reaction equation will be as follows.
      [tex]CuCl_{2} + (NH_{4})_{2}S \rightarrow 2NH_{4}Cl + CuS[/tex]
As 1 mole [tex]CuCl_{2}[/tex] reacts with 1 mole of [tex](NH_{4})_{2}S[/tex]
Hence, moles of [tex]CuCl_{2}[/tex] = Molarity × Volume (in mL)
                       = 0.5 × 38.0 mL
                       = 0.019 mol
Moles of [tex](NH_{4})_{2}S[/tex] = Molarity × Volume (in mL)
                      = 0.6 × 42.0 mL
                      = 0.0252 mol
As moles of CuS is less than the moles of [tex](NH_{4})_{2}S[/tex]. 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 [tex]95.6 g/mol \times 0.019 mol[/tex]
          = 1.8164 g
Thus, we can conclude that maximum mass of CuS formed is 1.8164 g.
The maximum mass of CuS that can be formed = 1.82g
Calculation of molar mass of a compound
The balanced equation of the mixture of CuCl2 and NH4)2S;
CuCl2 + (NH4)2S ---> 2NH4Cl + CuS
To calculate the number of moles for CuCl2 and (NH4)2S,
the following formula is used.
Number of moles = molarity × volume
Number of moles of CuCl2 = 0.5× 38= 0.019 mol
Number of moles of (NH4)2S = 0.6 × 42 = 0.025 mol
But 1 mol of CuS = 95.6g/mol
If 1 mole of CuCl2 produced 98.6g of CuS
0.019 mol of CuCl2 will produce = X g
X g = 0.019 × 95.6= 1.82g of CuS
Therefore, the maximum mass of CuS that can be formed = 1.82g
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