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? Aqueous ammonium chloride is the other product. A)2.41 g B)1.82 g C)1.21 g D)0.909 g E)0.044 g

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To find the maximum mass of CuS that can be formed, we first need to determine the limiting reactant. The balanced chemical equation for the reaction is:$$ \text{CuCl}_2 + \text{NH}_4_2\text{S} \rightarrow \text{CuS} + 2\text{NH}_4\text{Cl} $$From the given concentrations and volumes, we can calculate the moles of each reactant:- Moles of $\text{CuCl}_2 = 0.500 \, \text{M} \times 0.038 \, \text{L} = 0.019 \, \text{mol}$- Moles of $\text{NH}_4_2\text{S} = 0.600 \, \text{M} \times 0.042 \, \text{L} = 0.0252 \, \text{mol}$Since the reaction requires 1 mole of $\text{CuCl}_2$ for every 1 mole of $\text{NH}_4_2\text{S}$, $\text{CuCl}_2$ is the limiting reactant because it will be completely consumed first.The theoretical yield of CuS can be calculated using the moles of the limiting reactant ($\text{CuCl}_2$):- Moles of CuS formed = Moles of $\text{CuCl}_2$ = 0.019 molThe molar mass of CuS is approximately 95.611 g/mol, so the maximum mass of CuS that can be formed is:$$ 0.019 \, \text{mol} \times 95.611 \, \text{g/mol} = 1.816 \, \text{g} $$Therefore, the maximum mass of CuS that can be formed is 1.82 g.

Copper(II) Sulfide, CuS, Is Used in the Development of Aniline