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