Questions: Consider the balanced equation. CuSO4 + Zn → ZnSO4 + Cu If 200.0 g of copper(II) sulfate react with an excess of zinc metal, what is the theoretical yield of copper? 1.253 g 50.72 g 194.3 g

Solution Steps

First, calculate the molar mass of copper(II) sulfate (\(\mathrm{CuSO}_4\)):

• Cu: \(63.55 \, \text{g/mol}\)
• S: \(32.07 \, \text{g/mol}\)
• O: \(16.00 \, \text{g/mol} \times 4 = 64.00 \, \text{g/mol}\)

\[ \text{Molar mass of } \mathrm{CuSO}_4 = 63.55 + 32.07 + 64.00 = 159.62 \, \text{g/mol} \]

Using the given mass of copper(II) sulfate (200.0 g), calculate the number of moles:

\[ \text{Moles of } \mathrm{CuSO}_4 = \frac{200.0 \, \text{g}}{159.62 \, \text{g/mol}} = 1.253 \, \text{mol} \]

From the balanced equation, the mole ratio of \(\mathrm{CuSO}_4\) to \(\mathrm{Cu}\) is 1:1. Therefore, the moles of copper produced will also be 1.253 mol.

Calculate the mass of copper produced:

• Cu: \(63.55 \, \text{g/mol}\)

\[ \text{Mass of Cu} = 1.253 \, \text{mol} \times 63.55 \, \text{g/mol} = 79.63 \, \text{g} \]

Final Answer