Consider The Balanced Equation:${ \text{CuSO}_4 + \text{Zn} \rightarrow \text{ZnSO}_4 + \text{Cu} }$If 200.0 G Of Copper(II) Sulfate React With An Excess Of Zinc Metal, What Is The Theoretical Yield Of Copper?A. 1.253 G B. 50.72 G C. 79.63

Understanding the Balanced Equation

The given balanced equation is:

${ \text{CuSO}_4 + \text{Zn} \rightarrow \text{ZnSO}_4 + \text{Cu} }$

This equation represents the reaction between copper(II) sulfate (CuSO4) and zinc metal (Zn) to produce zinc sulfate (ZnSO4) and copper (Cu). The equation is balanced, meaning that the number of atoms of each element is the same on both the reactant and product sides.

Calculating the Theoretical Yield of Copper

To calculate the theoretical yield of copper, we need to know the molar masses of the reactants and products. The molar masses are:

• CuSO4: 159.61 g/mol
• Zn: 65.38 g/mol
• ZnSO4: 161.45 g/mol
• Cu: 63.55 g/mol

We are given 200.0 g of copper(II) sulfate (CuSO4). To calculate the number of moles of CuSO4, we divide the given mass by the molar mass:

${ \text{moles of CuSO}_4 = \frac{200.0 \text{ g}}{159.61 \text{ g/mol}} = 1.253 \text{ mol} }$

Since the reaction is a 1:1 ratio, the number of moles of Cu produced will be equal to the number of moles of CuSO4 reacted:

${ \text{moles of Cu} = 1.253 \text{ mol} }$

To calculate the mass of Cu produced, we multiply the number of moles by the molar mass of Cu:

${ \text{mass of Cu} = 1.253 \text{ mol} \times 63.55 \text{ g/mol} = 79.63 \text{ g} }$

Therefore, the theoretical yield of copper is 79.63 g.

Conclusion

In this problem, we used the balanced equation to calculate the theoretical yield of copper produced in a reaction between copper(II) sulfate and zinc metal. We calculated the number of moles of CuSO4 reacted and then used the 1:1 ratio to determine the number of moles of Cu produced. Finally, we multiplied the number of moles of Cu by its molar mass to obtain the mass of Cu produced.

Key Takeaways

• The balanced equation is a crucial tool in chemistry for understanding chemical reactions.
• The molar masses of reactants and products are essential in calculating the number of moles and mass of substances involved in a reaction.
• The theoretical yield of a substance can be calculated using the number of moles and molar mass of the substance.

Additional Resources

For further practice and understanding of chemical reactions, we recommend the following resources:

• Online chemistry textbooks and resources, such as Khan Academy and Chemistry LibreTexts.
• Chemistry laboratory manuals and experiments.
• Online forums and discussion groups for chemistry enthusiasts.

Frequently Asked Questions

Q: What is the balanced equation for the reaction between copper(II) sulfate and zinc metal? A: The balanced equation is:

${ \text{CuSO}_4 + \text{Zn} \ \text{ZnSO}_4 + \text{Cu} }$

Q: How do I calculate the number of moles of a substance? A: To calculate the number of moles of a substance, you divide the given mass by the molar mass of the substance.

Q: What is the balanced equation for the reaction between copper(II) sulfate and zinc metal?

A: The balanced equation is:

${ \text{CuSO}_4 + \text{Zn} \rightarrow \text{ZnSO}_4 + \text{Cu} }$

Q: What is the molar mass of copper(II) sulfate (CuSO4)?

A: The molar mass of copper(II) sulfate (CuSO4) is 159.61 g/mol.

Q: How do I calculate the number of moles of copper(II) sulfate (CuSO4) reacted?

A: To calculate the number of moles of copper(II) sulfate (CuSO4) reacted, you divide the given mass by the molar mass of CuSO4:

${ \text{moles of CuSO}_4 = \frac{200.0 \text{ g}}{159.61 \text{ g/mol}} = 1.253 \text{ mol} }$

Q: What is the molar mass of copper (Cu)?

A: The molar mass of copper (Cu) is 63.55 g/mol.

Q: How do I calculate the mass of copper (Cu) produced?

A: To calculate the mass of copper (Cu) produced, you multiply the number of moles of Cu by its molar mass:

${ \text{mass of Cu} = 1.253 \text{ mol} \times 63.55 \text{ g/mol} = 79.63 \text{ g} }$

Q: What is the theoretical yield of copper in this reaction?

A: The theoretical yield of copper is 79.63 g.

Q: What is the difference between theoretical yield and actual yield?

A: Theoretical yield is the maximum amount of product that can be obtained from a given amount of reactant, assuming 100% efficiency. Actual yield is the amount of product obtained in a real-world experiment, which is often less than the theoretical yield due to factors such as impurities, equipment limitations, and human error.

Q: How can I improve the actual yield of copper in this reaction?

A: To improve the actual yield of copper, you can try to minimize impurities, optimize the reaction conditions, and use high-quality equipment. Additionally, you can try to use a catalyst or modify the reaction conditions to increase the reaction rate.

Q: What are some common mistakes to avoid when calculating the theoretical yield of copper?

A: Some common mistakes to avoid when calculating the theoretical yield of copper include:

• Not using the correct molar masses of the reactants and products
• Not converting the given mass of CuSO4 to moles
• Not multiplying the number of moles of Cu by its molar mass to obtain the mass of Cu produced
• Not considering the 1:1 ratio of CuSO4 to Cu in the balanced equation

Q: Where can I find more information on calculating the theoretical yield of copper?

A: You can find more information on calculating the theoretical yield of copper in online chemistry textbooks and resources, such as Khan Academy and Chemistry LibreTexts. You can also consult with a chemistry teacher or professor for additional guidance.