If 10.1 G Of Fe Are Reacted, What Mass Of Copper Would Form? 2Fe + 3CuSO4 --> Fe2(SO4)3 + 3Cu Equivalence Statements: 1 Mol Fe = 55.85 G Fe 1 Mol Cu = 63.55 G Cu

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Understanding the Chemical Reaction

In the given chemical equation, 2 moles of iron (Fe) react with 3 moles of copper(II) sulfate (CuSO4) to form 1 mole of iron(III) sulfate (Fe2(SO4)3) and 3 moles of copper (Cu). The balanced chemical equation is:

2Fe + 3CuSO4 --> Fe2(SO4)3 + 3Cu

Given Information

We are given that 10.1 g of Fe are reacted. We need to determine the mass of copper that would form.

Equivalence Statements

To solve this problem, we need to use the equivalence statements provided:

  • 1 mol Fe = 55.85 g Fe
  • 1 mol Cu = 63.55 g Cu

Step 1: Calculate the Number of Moles of Iron

First, we need to calculate the number of moles of iron that are reacted. We can do this by dividing the given mass of iron (10.1 g) by the molar mass of iron (55.85 g/mol).

moles_Fe = mass_Fe / molar_mass_Fe
moles_Fe = 10.1 g / 55.85 g/mol
moles_Fe = 0.181 mol

Step 2: Determine the Number of Moles of Copper

Since the balanced chemical equation shows that 2 moles of iron react with 3 moles of copper, we can set up a proportion to determine the number of moles of copper that would form.

moles_Cu = (3/2) * moles_Fe
moles_Cu = (3/2) * 0.181 mol
moles_Cu = 0.272 mol

Step 3: Calculate the Mass of Copper

Finally, we can calculate the mass of copper that would form by multiplying the number of moles of copper by the molar mass of copper.

mass_Cu = moles_Cu * molar_mass_Cu
mass_Cu = 0.272 mol * 63.55 g/mol
mass_Cu = 17.3 g

Conclusion

In conclusion, if 10.1 g of Fe are reacted, the mass of copper that would form is 17.3 g.

Discussion

This problem demonstrates the importance of balancing chemical equations and using stoichiometry to determine the amounts of reactants and products in a chemical reaction. By following the steps outlined above, we can accurately calculate the mass of copper that would form in this reaction.

Additional Examples

This problem is a classic example of a stoichiometry problem. Here are a few additional examples:

  • If 5.0 g of CuSO4 are reacted, what mass of Fe would form?
  • If 2.0 g of Fe2(SO4)3 are formed, what mass of Cu would form?

These problems can be solved using the same steps outlined above.

References

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling

Keywords

  • Stoichiometry
  • Balancing chemical equations
  • Molar mass
  • Number of moles
  • Mass of copper
  • Iron(III) sulfate
  • Copper(II) sulfate
    Frequently Asked Questions (FAQs) on Stoichiometry and Balancing Chemical Equations =====================================================================================

Q: What is stoichiometry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves the use of mole ratios to determine the amounts of reactants and products in a chemical reaction.

Q: Why is balancing chemical equations important?

A: Balancing chemical equations is important because it allows us to determine the correct mole ratios between reactants and products in a chemical reaction. This is crucial in stoichiometry, as it enables us to calculate the amounts of reactants and products in a chemical reaction.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to ensure that the number of atoms of each element is the same on both the reactant and product sides of the equation. You can do this by adding coefficients (numbers in front of the formulas of reactants or products) to balance the equation.

Q: What is the difference between a balanced and unbalanced chemical equation?

A: A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides of the equation. An unbalanced chemical equation does not have the same number of atoms of each element on both sides of the equation.

Q: How do I determine the number of moles of a substance?

A: To determine the number of moles of a substance, you need to know the mass of the substance and its molar mass. You can calculate the number of moles by dividing the mass of the substance by its molar mass.

Q: What is the relationship between moles and mass?

A: The relationship between moles and mass is given by the formula: moles = mass / molar mass. This formula allows you to calculate the number of moles of a substance from its mass and molar mass.

Q: How do I calculate the mass of a substance from its number of moles?

A: To calculate the mass of a substance from its number of moles, you need to know the molar mass of the substance. You can calculate the mass by multiplying the number of moles by the molar mass.

Q: What is the significance of stoichiometry in real-life applications?

A: Stoichiometry has numerous real-life applications, including:

  • Calculating the amounts of reactants and products in chemical reactions
  • Determining the yields of chemical reactions
  • Calculating the amounts of substances required for a reaction
  • Predicting the outcomes of chemical reactions

Q: Can you provide examples of stoichiometry problems?

A: Yes, here are a few examples of stoichiometry problems:

  • If 5.0 g of CuSO4 are reacted, what mass of Fe would form?
  • If 2.0 g of Fe2(SO4)3 are formed, what mass of Cu would form?
  • If 10.1 g of Fe are reacted, what mass of Cu would form?

These problems can be solved using the steps outlined in the previous article.

Q: What are some common mistakes to avoid in stoichiometry?

A: Some common mistakes to avoid in stoichiometry include:

  • Not balancing the chemical equation
  • Not using the correct mole ratios
  • Not calculating the number of moles correctly
  • Not using the correct molar masses

By avoiding these mistakes, you can ensure accurate calculations and results in stoichiometry.

Q: Can you provide additional resources for learning stoichiometry?

A: Yes, here are some additional resources for learning stoichiometry:

  • Chemistry: An Atoms First Approach, by Steven S. Zumdahl
  • General Chemistry: Principles and Modern Applications, by Linus Pauling
  • Online tutorials and videos on stoichiometry
  • Practice problems and worksheets on stoichiometry

By using these resources, you can gain a deeper understanding of stoichiometry and improve your skills in solving problems.