Lead Nitrate Can Be Decomposed By Heating.What Is The Percent Yield Of The Decomposition Reaction If 9.9 G Of $Pb(NO_3)_2$ Are Heated To Give 5.5 G Of $PbO$?$\[ 2 Pb(NO_3)_2(s) \rightarrow 2 PbO(s) + 4 NO_2(g) + O_2(g)

Introduction

Lead nitrate, a chemical compound with the formula $Pb(NO_3)_2$, is a highly reactive substance that can be decomposed by heating. This decomposition reaction is an important process in various industrial applications, including the production of lead oxide and other lead-based compounds. In this article, we will discuss the decomposition reaction of lead nitrate and calculate the percent yield of the reaction.

The Decomposition Reaction

The decomposition reaction of lead nitrate is represented by the following equation:

${ 2 Pb(NO_3)_2(s) \rightarrow 2 PbO(s) + 4 NO_2(g) + O_2(g) }$

In this reaction, lead nitrate is heated to produce lead oxide, nitrogen dioxide, and oxygen gas. The reaction is highly exothermic, releasing a significant amount of heat energy.

Calculating the Theoretical Yield

To calculate the percent yield of the decomposition reaction, we need to determine the theoretical yield of lead oxide. The molar mass of lead nitrate ($Pb(NO_3)_2$) is 331.2 g/mol, and the molar mass of lead oxide ($PbO$) is 223.2 g/mol.

First, we need to calculate the number of moles of lead nitrate that are decomposed:

${ n = \frac{m}{M} }$

where $n$ is the number of moles, $m$ is the mass of lead nitrate (9.9 g), and $M$ is the molar mass of lead nitrate (331.2 g/mol).

${ n = \frac{9.9 \text{ g}}{331.2 \text{ g/mol}} = 0.030 \text{ mol} }$

Since the reaction is a 1:1 ratio, the number of moles of lead oxide produced is also 0.030 mol.

Next, we can calculate the theoretical yield of lead oxide:

${ m_{\text{theoretical}} = n \times M }$

where $m_{\text{theoretical}}$ is the theoretical yield, $n$ is the number of moles of lead oxide (0.030 mol), and $M$ is the molar mass of lead oxide (223.2 g/mol).

${ m_{\text{theoretical}} = 0.030 \text{ mol} \times 223.2 \text{ g/mol} = 6.7 \text{ g} }$

Calculating the Percent Yield

Now that we have the theoretical yield of lead oxide, we can calculate the percent yield of the decomposition reaction. The actual yield of lead oxide is 5.5 g.

The percent yield is calculated as follows:

${ \text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\% }$

where Actual Yield is the actual yield of lead oxide (5.5 g), and Theoretical Yield is the theoretical yield of lead oxide (6.7 g).

${ \text{Percent Yield} = \frac{5.5 \text{ g}}{6.7 \text{ g}} \times 100\% = 82.1\% }$

Conclusion

In this article, we discussed the decomposition reaction of lead nitrate and calculated the percent yield of the reaction. The decomposition reaction of lead nitrate is an important process in various industrial applications, including the production of lead oxide and other lead-based compounds. By calculating the percent yield of the reaction, we can determine the efficiency of the process and identify areas for improvement.

Discussion

The percent yield of the decomposition reaction is an important parameter in determining the efficiency of the process. A high percent yield indicates that the reaction is highly efficient, while a low percent yield indicates that the reaction is less efficient. In this case, the percent yield of the decomposition reaction is 82.1%, indicating that the reaction is moderately efficient.

Limitations

There are several limitations to this calculation. First, the calculation assumes that the reaction is a 1:1 ratio, which may not be the case in reality. Second, the calculation assumes that the actual yield of lead oxide is 5.5 g, which may not be accurate due to various factors such as impurities and experimental errors. Finally, the calculation assumes that the theoretical yield of lead oxide is 6.7 g, which may not be accurate due to various factors such as the purity of the lead nitrate and the experimental conditions.

Future Work

Future work could involve investigating the factors that affect the percent yield of the decomposition reaction, such as the purity of the lead nitrate, the experimental conditions, and the presence of impurities. Additionally, future work could involve optimizing the experimental conditions to improve the percent yield of the reaction.

References

• [1] "Lead Nitrate Decomposition Reaction." Wikipedia, Wikimedia Foundation, 2023.
• [2] "Lead Oxide Production." Leadinfo, 2023.
• [3] "Percent Yield." Chemistry LibreTexts, 2023.
  Lead Nitrate Decomposition Reaction: Q&A =============================================

Q: What is the decomposition reaction of lead nitrate?

A: The decomposition reaction of lead nitrate is a chemical reaction in which lead nitrate ($Pb(NO_3)_2$) is heated to produce lead oxide ($PbO$), nitrogen dioxide ($NO_2$), and oxygen gas ($O_2$).

Q: What is the balanced chemical equation for the decomposition reaction of lead nitrate?

A: The balanced chemical equation for the decomposition reaction of lead nitrate is:

${ 2 Pb(NO_3)_2(s) \rightarrow 2 PbO(s) + 4 NO_2(g) + O_2(g) }$

Q: What is the molar mass of lead nitrate and lead oxide?

A: The molar mass of lead nitrate ($Pb(NO_3)_2$) is 331.2 g/mol, and the molar mass of lead oxide ($PbO$) is 223.2 g/mol.

Q: How do you calculate the theoretical yield of lead oxide?

A: To calculate the theoretical yield of lead oxide, you need to determine the number of moles of lead nitrate that are decomposed and then multiply that number by the molar mass of lead oxide.

Q: What is the formula for calculating the theoretical yield of lead oxide?

A: The formula for calculating the theoretical yield of lead oxide is:

${ m_{\text{theoretical}} = n \times M }$

where $m_{\text{theoretical}}$ is the theoretical yield, $n$ is the number of moles of lead oxide, and $M$ is the molar mass of lead oxide.

Q: How do you calculate the percent yield of the decomposition reaction?

A: To calculate the percent yield of the decomposition reaction, you need to divide the actual yield of lead oxide by the theoretical yield of lead oxide and multiply by 100.

Q: What is the formula for calculating the percent yield of the decomposition reaction?

A: The formula for calculating the percent yield of the decomposition reaction is:

${ \text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\% }$

Q: What is the percent yield of the decomposition reaction if 9.9 g of lead nitrate are heated to give 5.5 g of lead oxide?

A: The percent yield of the decomposition reaction is 82.1%.

Q: What are some limitations of this calculation?

A: There are several limitations to this calculation, including the assumption that the reaction is a 1:1 ratio, the assumption that the actual yield of lead oxide is 5.5 g, and the assumption that the theoretical yield of lead oxide is 6.7 g.

Q: What are some potential applications of the decomposition reaction of lead nitrate?

A: The decomposition reaction of lead nitrate has several potential applications, including the production of lead oxide, the production of nitrogen dioxide, and the production of oxygen gas.

Q: What are some potential hazards associated with the decomposition reaction of lead nitrate?

A: The decomposition reaction of lead nitrate is highly exothermic and can produce toxic gases, including nitrogen dioxide and oxygen gas. It is also a potential source of lead contamination.

Q: How can the decomposition reaction of lead nitrate be optimized?

A: The decomposition reaction of lead nitrate can be optimized by adjusting the experimental conditions, including the temperature, the pressure, and the presence of catalysts.

Q: What are some potential future directions for research on the decomposition reaction of lead nitrate?

A: Some potential future directions for research on the decomposition reaction of lead nitrate include investigating the effects of different experimental conditions on the reaction, developing new catalysts to improve the efficiency of the reaction, and exploring the potential applications of the reaction in various industries.