Calculating the Number of Moles of Sodium Metal

Oct 13, 2025 by magicalceylontours.com 12 views

Introduction

In chemistry, experiments often involve the reaction of two or more substances to form a new compound. One such experiment involves the reaction of sodium metal with chlorine gas to form sodium chloride. In this article, we will explore the chemical reaction that occurs when 57.50 grams of sodium metal is reacted with an excess amount of chlorine gas, and calculate the percentage yield of the reaction.

The Chemical Reaction

The chemical reaction that occurs when sodium metal is reacted with chlorine gas is shown below:

${ 2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl} \}$

In this reaction, two moles of sodium metal react with one mole of chlorine gas to form two moles of sodium chloride.

Calculating the Number of Moles of Sodium Metal

To calculate the number of moles of sodium metal, we need to know the molar mass of sodium. The molar mass of sodium is 22.99 g/mol.

We can calculate the number of moles of sodium metal as follows:

${ \text{Number of moles of Na} = \frac{\text{Mass of Na}}{\text{Molar mass of Na}} \}$

${ \text{Number of moles of Na} = \frac{57.50 \text{ g}}{22.99 \text{ g/mol}} \}$

${ \text{Number of moles of Na} = 2.50 \text{ mol} \}$

Calculating the Number of Moles of Sodium Chloride

Since the reaction is a 1:1 ratio, the number of moles of sodium chloride produced will be equal to the number of moles of sodium metal reacted.

${ \text{Number of moles of NaCl} = \text{Number of moles of Na} \}$

${ \text{Number of moles of NaCl} = 2.50 \text{ mol} \}$

Calculating the Mass of Sodium Chloride Produced

To calculate the mass of sodium chloride produced, we need to know the molar mass of sodium chloride. The molar mass of sodium chloride is 58.44 g/mol.

We can calculate the mass of sodium chloride produced as follows:

${ \text{Mass of NaCl} = \text{Number of moles of NaCl} \times \text{Molar mass of NaCl} \}$

${ \text{Mass of NaCl} = 2.50 \text{ mol} \times 58.44 \text{ g/mol} \}$

${ \text{Mass of NaCl} = 145.60 \text{ g} \}$

Calculating the Theoretical Yield

The theoretical yield is the maximum amount of product that can be obtained from a given amount of reactant. In this case, the theoretical yield is the mass of sodium chloride that would be produced if the reaction were 100% efficient.

${ \text{Theoretical yield} = \text{Mass of NaCl} \}$

${ \text{Theoretical yield} = 145.60 \text{ g} \}$

Calculating the Percentage Yield

The percentage yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage.

${ \text{Percentage yield} = \frac{\text{Actual yield}}{\text{Theoretical yield}} \times 100\% \}$

${ \text{Percentage yield} = \frac{145.60 \text{ g}}{145.60 \text{ g}} \times 100\% \}$

${ \text{Percentage yield} = 100\% \}$

However, we are given that the percentage yield is 86%. This means that the actual yield is 86% of the theoretical yield.

${ \text{Actual yield} = \text{Percentage yield} \times \text{Theoretical yield} \}$

${ \text{Actual yield} = 0.86 \times 145.60 \text{ g} \}$

${ \text{Actual yield} = 125.19 \text{ g} \}$

Conclusion

In this article, we have calculated the percentage yield of the reaction between sodium metal and chlorine gas to form sodium chloride. We have found that the actual yield is 86% of the theoretical yield, which is 125.19 g. This means that the chemist was able to obtain 86% of the maximum amount of sodium chloride that could be produced from the given amount of reactants.

Discussion

The percentage yield of a reaction is an important factor to consider in chemistry. It can affect the outcome of an experiment and the accuracy of the results. In this case, the percentage yield of 86% indicates that the chemist was able to obtain a significant amount of sodium chloride from the reaction.

However, it is also possible that the percentage yield could be lower due to various factors such as impurities, contamination, or incomplete reaction. In such cases, the chemist may need to re-run the experiment or adjust the conditions to improve the yield.

References

CRC Handbook of Chemistry and Physics, 97th ed.
Chemical Equilibrium, 2nd ed. by J. W. Moore and R. G. Pearson.

Keywords

Sodium metal
Chlorine gas
Sodium chloride
Percentage yield
Theoretical yield
Actual yield
Chemical reaction
Chemistry experiment
A Chemist's Experiment: Q&A =============================

Introduction

In our previous article, we explored the chemical reaction between sodium metal and chlorine gas to form sodium chloride, and calculated the percentage yield of the reaction. In this article, we will answer some frequently asked questions related to the experiment.

Q: What is the purpose of calculating the percentage yield of a reaction?

A: The purpose of calculating the percentage yield of a reaction is to determine the efficiency of the reaction. It helps to identify any factors that may be affecting the yield, such as impurities, contamination, or incomplete reaction.

Q: How do I calculate the percentage yield of a reaction?

A: To calculate the percentage yield of a reaction, you need to know the actual yield and the theoretical yield. The actual yield is the amount of product obtained from the reaction, while the theoretical yield is the maximum amount of product that can be obtained from a given amount of reactant. The percentage yield is then calculated as the ratio of the actual yield to the theoretical yield, expressed as a percentage.

Q: What are some common factors that can affect the percentage yield of a reaction?

A: Some common factors that can affect the percentage yield of a reaction include:

Impurities in the reactants or products
Contamination of the reaction mixture
Incomplete reaction
Unfavorable reaction conditions, such as temperature or pressure
Inadequate stirring or mixing of the reaction mixture

Q: How can I improve the percentage yield of a reaction?

A: To improve the percentage yield of a reaction, you can try the following:

Use high-purity reactants and products
Minimize contamination of the reaction mixture
Ensure that the reaction is complete
Optimize the reaction conditions, such as temperature or pressure
Use adequate stirring or mixing of the reaction mixture

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

A: The actual yield is the amount of product obtained from the reaction, while the theoretical yield is the maximum amount of product that can be obtained from a given amount of reactant. The actual yield is always less than or equal to the theoretical yield.

Q: How do I determine the actual yield of a reaction?

A: To determine the actual yield of a reaction, you need to measure the mass of the product obtained from the reaction. This can be done using a balance or other measuring device.

Q: What is the significance of the percentage yield in a chemical reaction?

A: The percentage yield is a measure of the efficiency of a chemical reaction. It indicates the amount of product obtained from the reaction relative to the maximum amount that can be obtained. A high percentage yield indicates that the reaction is efficient and that the product is obtained in high purity.

Q: Can the percentage yield of a reaction be affected by external factors?

A: Yes, the percentage yield of a reaction can be affected by external factors, such as temperature, pressure, and stirring or mixing of the reaction mixture. These factors can affect the rate of reaction, the yield of product, and the purity of the product.

Q: How can I use the percentage yield to optimize a chemical reaction?

A: To use the percentage yield to optimize a chemical reaction, you can try the following:

Measure the percentage yield of the reaction
Identify any factors that may be affecting the yield, such as impurities, contamination, or incomplete reaction
Optimize the reaction conditions, such as temperature or pressure
Use adequate stirring or mixing of the reaction mixture
Monitor the reaction closely to ensure that it is complete and that the product is obtained in high purity.

Conclusion

In this article, we have answered some frequently asked questions related to the experiment of calculating the percentage yield of a reaction. We have discussed the purpose of calculating the percentage yield, how to calculate it, and some common factors that can affect it. We have also provided some tips on how to improve the percentage yield of a reaction and how to use it to optimize a chemical reaction.