How Many Grams Of $PbSO_4$ Would Be Produced From The Complete Reaction Of 23.6 G $PbO$?$[ \begin Array}{l} Pb + PbO_2 + 2H_2SO_4 \rightarrow 2PbSO_4 + 2H_2O \ PbO_2 239.2 , \text{g/mol \quad [?] , \text{g} , PbSO_4

Mar 7, 2025 by ADMIN 220 views

**How Many Grams of PbSO4 Would Be Produced from the Complete Reaction of 23.6 g PbO?**

Understanding the Chemical Reaction

The given chemical reaction involves the formation of lead sulfate (PbSO4) from the reaction of lead (Pb), lead dioxide (PbO2), and sulfuric acid (H2SO4). The balanced chemical equation for this reaction is:

Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O

In this reaction, lead (Pb) and lead dioxide (PbO2) react with sulfuric acid (H2SO4) to form lead sulfate (PbSO4) and water (H2O). The question asks us to determine the amount of lead sulfate (PbSO4) produced from the complete reaction of 23.6 g of lead oxide (PbO).

Calculating the Molar Mass of PbO2

To solve this problem, we need to calculate the molar mass of lead dioxide (PbO2). The atomic masses of lead (Pb) and oxygen (O) are 207.2 g/mol and 16.0 g/mol, respectively. Therefore, the molar mass of PbO2 is:

Molar mass of PbO2 = atomic mass of Pb + 2 × atomic mass of O = 207.2 g/mol + 2 × 16.0 g/mol = 239.2 g/mol

Calculating the Number of Moles of PbO2

Since the question asks us to determine the amount of lead sulfate (PbSO4) produced from the complete reaction of 23.6 g of lead oxide (PbO), we need to calculate the number of moles of PbO2 required for the reaction. However, the given reaction equation shows that PbO2 is not directly involved in the reaction. Instead, the reaction involves the formation of PbSO4 from Pb and H2SO4. Therefore, we need to calculate the number of moles of PbO required for the reaction.

The molar mass of PbO is:

Molar mass of PbO = atomic mass of Pb + atomic mass of O = 207.2 g/mol + 16.0 g/mol = 223.2 g/mol

Now, we can calculate the number of moles of PbO:

Number of moles of PbO = mass of PbO / molar mass of PbO = 23.6 g / 223.2 g/mol = 0.106 mol

Calculating the Number of Moles of PbSO4 Produced

Since the reaction equation shows that 1 mole of Pb produces 1 mole of PbSO4, the number of moles of PbSO4 produced is equal to the number of moles of PbO required for the reaction:

Number of moles of PbSO4 = number of moles of PbO = 0.106 mol

Calculating the Mass of PbSO4 Produced

Now, we can calculate the mass of PbSO4 produced:

Molar mass of PbSO4 = atomic mass of Pb + atomic mass of S + 4 × atomic mass of O = 207.2 g/mol + 32.1 g/mol + 4 × 16.0 g/mol = 303.9 g/mol

Mass of PbSO4 = number of moles of PbSO4 × molar mass of PbSO4 = 0.106 mol × 303.9 g/mol = 32.2 g

Therefore, the amount of lead sulfate (PbSO4) produced from the complete reaction of 23.6 g of lead oxide (PbO) is 32.2 g.

Conclusion

In this problem, we calculated the amount of lead sulfate (PbSO4) produced from the complete reaction of 23.6 g of lead oxide (PbO). We first calculated the number of moles of PbO required for the reaction, and then used the balanced chemical equation to determine the number of moles of PbSO4 produced. Finally, we calculated the mass of PbSO4 produced using the molar mass of PbSO4. The result shows that the amount of PbSO4 produced is 32.2 g.

References

CRC Handbook of Chemistry and Physics, 97th Edition
Lide, D. R. (2016). CRC Handbook of Chemistry and Physics. CRC Press.
Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2016). General Chemistry: Principles and Modern Applications. Pearson Education.

Discussion

This problem requires a good understanding of chemical reactions, stoichiometry, and molar masses. The student should be able to balance chemical equations, calculate the number of moles of reactants and products, and use molar masses to calculate the mass of products. This problem is relevant to chemistry students who are studying chemical reactions and stoichiometry.

Additional Problems

Calculate the amount of lead (Pb) required to produce 32.2 g of lead sulfate (PbSO4).
Calculate the amount of sulfuric acid (H2SO4) required to produce 32.2 g of lead sulfate (PbSO4).
Calculate the amount of water (H2O) produced in the reaction.

These problems require the student to apply the concepts learned in this problem to new situations, and to think critically about the chemical reactions involved.

Q: What is the balanced chemical equation for the reaction?

A: The balanced chemical equation for the reaction is:

Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O

Q: What is the molar mass of PbO2?

A: The molar mass of PbO2 is 239.2 g/mol.

Q: How many moles of PbO are required for the reaction?

A: To calculate the number of moles of PbO required for the reaction, we need to calculate the mass of PbO required for the reaction. The molar mass of PbO is 223.2 g/mol. Therefore, the number of moles of PbO required for the reaction is:

Number of moles of PbO = mass of PbO / molar mass of PbO = 23.6 g / 223.2 g/mol = 0.106 mol

Q: How many moles of PbSO4 are produced in the reaction?

A: Since the reaction equation shows that 1 mole of Pb produces 1 mole of PbSO4, the number of moles of PbSO4 produced is equal to the number of moles of PbO required for the reaction:

Number of moles of PbSO4 = number of moles of PbO = 0.106 mol

Q: What is the molar mass of PbSO4?

A: The molar mass of PbSO4 is 303.9 g/mol.

Q: How many grams of PbSO4 are produced in the reaction?

A: To calculate the mass of PbSO4 produced, we need to multiply the number of moles of PbSO4 by the molar mass of PbSO4:

Mass of PbSO4 = number of moles of PbSO4 × molar mass of PbSO4 = 0.106 mol × 303.9 g/mol = 32.2 g

Q: What is the relationship between the amount of PbO and the amount of PbSO4 produced?

A: The amount of PbSO4 produced is directly proportional to the amount of PbO required for the reaction.

Q: What is the significance of the balanced chemical equation in this reaction?

A: The balanced chemical equation shows the stoichiometric relationship between the reactants and products in the reaction. It allows us to calculate the amount of products produced from a given amount of reactants.

Q: How can we use this reaction to produce PbSO4?

A: We can use this reaction to produce PbSO4 by reacting PbO with H2SO4 in the presence of Pb. The reaction is:

Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O

Q: What are some potential applications of PbSO4?

A: PbSO4 has several potential applications, including:

As a pigment in paints and coatings
As a component in batteries and other electrochemical devices
As a catalyst in chemical reactions
As a component in pharmaceuticals and other medical applications

These are just a few examples of the potential applications of PbSO4. The actual applications will depend on the specific properties and characteristics of the PbSO4 produced.