125 G Of Aluminum Bromide Reacts With Potassium Sulfate According To The Equation Below, Generating 45.6 G Of Potassium Bromide. What Is The Percent Yield For The Reaction?$\[ \begin{array}{c} 2 \text{AlBr}_3 + 3 \text{K}_2\text{SO}_4 \rightarrow 6
Understanding Percent Yield
Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield of a product to its theoretical yield, multiplied by 100. In other words, it is a measure of how much of the product is actually obtained compared to the maximum amount that could be obtained if the reaction were 100% efficient.
Theoretical Yield
To calculate the percent yield, we first need to calculate the theoretical yield of the product. The theoretical yield is the maximum amount of product that could be obtained if the reaction were 100% efficient. We can calculate the theoretical yield by using the molar masses of the reactants and products.
Calculating Molar Masses
The molar mass of aluminum bromide (AlBr3) is 266.25 g/mol. The molar mass of potassium sulfate (K2SO4) is 174.26 g/mol. The molar mass of potassium bromide (KBr) is 119.00 g/mol.
Balancing the Equation
The balanced equation for the reaction is:
2AlBr3 + 3K2SO4 → 6KBr + Al2(SO4)3
Calculating Theoretical Yield
To calculate the theoretical yield of potassium bromide, we need to know the number of moles of aluminum bromide that reacted. We can calculate the number of moles of aluminum bromide by dividing the given mass (125 g) by its molar mass (266.25 g/mol).
moles AlBr3 = mass AlBr3 / molar mass AlBr3 moles AlBr3 = 125 g / 266.25 g/mol moles AlBr3 = 0.469 mol
Since the balanced equation shows that 2 moles of AlBr3 produce 6 moles of KBr, we can calculate the number of moles of KBr that should be produced.
moles KBr = 6 × moles AlBr3 moles KBr = 6 × 0.469 mol moles KBr = 2.814 mol
Now, we can calculate the theoretical yield of KBr by multiplying the number of moles of KBr by its molar mass.
theoretical yield KBr = moles KBr × molar mass KBr theoretical yield KBr = 2.814 mol × 119.00 g/mol theoretical yield KBr = 334.06 g
Calculating Percent Yield
Now that we have the theoretical yield, we can calculate the percent yield by dividing the actual yield (45.6 g) by the theoretical yield (334.06 g) and multiplying by 100.
percent yield = (actual yield / theoretical yield) × 100 percent yield = (45.6 g / 334.06 g) × 100 percent yield = 13.67%
Therefore, the percent yield of the reaction is 13.67%.
Conclusion
In conclusion, the percent yield of the reaction between aluminum bromide and potassium sulfate is 13.67%. This means that only 13.67% of the maximum amount of potassium bromide that could be obtained was actually produced. This is a relatively low percent yield, indicating that the reaction is not very efficient.
Discussion
The low percent yield of this reaction can be attributed to several factors, including the formation of byproducts, the presence of impurities, and the incomplete reaction. To improve the percent yield, it may be necessary to optimize the reaction conditions, such as the temperature, pressure, and concentration of the reactants.
References
- "Chemical Reactions and Equations" by OpenStax
- "General Chemistry" by Linus Pauling
Additional Resources
- Khan Academy: Percent Yield
- Chemistry LibreTexts: Percent Yield
Table of Contents
- Understanding Percent Yield
- Theoretical Yield
- Calculating Molar Masses
- Balancing the Equation
- Calculating Theoretical Yield
- Calculating Percent Yield
- Conclusion
- Discussion
- References
- Additional Resources
Percent Yield Q&A =====================
Q: What is percent yield?
A: Percent yield is a measure of the efficiency of a chemical reaction. It is defined as the ratio of the actual yield of a product to its theoretical yield, multiplied by 100.
Q: Why is percent yield important?
A: Percent yield is important because it helps us understand how efficient a chemical reaction is. A high percent yield indicates that the reaction is efficient and produces a lot of product, while a low percent yield indicates that the reaction is not very efficient and produces very little product.
Q: How do I calculate percent yield?
A: To calculate percent yield, you need to know the actual yield of the product and the theoretical yield of the product. The actual yield is the amount of product that is actually produced, while the theoretical yield is the maximum amount of product that could be produced if the reaction were 100% efficient. You can calculate percent yield by dividing the actual yield by the theoretical yield and multiplying by 100.
Q: What are some common reasons for low percent yield?
A: Some common reasons for low percent yield include:
- Formation of byproducts
- Presence of impurities
- Incomplete reaction
- Incorrect reaction conditions (such as temperature, pressure, or concentration of reactants)
Q: How can I improve percent yield?
A: To improve percent yield, you can try the following:
- Optimize reaction conditions (such as temperature, pressure, or concentration of reactants)
- Use a catalyst to speed up the reaction
- Use a solvent to improve the reaction rate
- Remove impurities from the reaction mixture
- Use a different reaction pathway or mechanism
Q: What is the difference between actual yield and theoretical yield?
A: The actual yield is the amount of product that is actually produced, while the theoretical yield is the maximum amount of product that could be produced if the reaction were 100% efficient. The actual yield is always less than or equal to the theoretical yield.
Q: Can percent yield be greater than 100%?
A: No, percent yield cannot be greater than 100%. If the percent yield is greater than 100%, it means that more product is being produced than is possible, which is not physically possible.
Q: What is the significance of percent yield in real-world applications?
A: Percent yield is significant in real-world applications because it helps us understand how efficient a chemical reaction is. A high percent yield is important in industries such as pharmaceuticals, where high-purity products are required. A low percent yield can result in wasted resources and increased costs.
Q: Can percent yield be used to compare the efficiency of different reactions?
A: Yes, percent yield can be used to compare the efficiency of different reactions. By comparing the percent yield of different reactions, you can determine which reaction is more efficient and produces more product.
Q: What are some common applications of percent yield?
A: Some common applications of percent yield include:
- Pharmaceutical industry: to determine the efficiency of a reaction and produce high-purity products
- Chemical industry: to determine the efficiency of a reaction and produce high-purity products
- Biotechnology industry: to determine the efficiency of a reaction and produce high-purity products
- Environmental science: to determine the efficiency of a reaction and produce high-purity products
Q: Can percent yield be used to predict the outcome of a reaction?
A: Yes, percent yield can be used to predict the outcome of a reaction. By knowing the percent yield of a reaction, you can determine how much product will be produced and whether the reaction will be efficient.
Q: What are some common mistakes to avoid when calculating percent yield?
A: Some common mistakes to avoid when calculating percent yield include:
- Not knowing the actual yield and theoretical yield
- Not using the correct units (such as grams or moles)
- Not rounding correctly
- Not checking for errors in the calculation
Q: Can percent yield be used to compare the efficiency of different reactions with different reactants?
A: Yes, percent yield can be used to compare the efficiency of different reactions with different reactants. By comparing the percent yield of different reactions, you can determine which reaction is more efficient and produces more product.
Q: What are some common challenges when calculating percent yield?
A: Some common challenges when calculating percent yield include:
- Difficulty in determining the actual yield and theoretical yield
- Difficulty in using the correct units (such as grams or moles)
- Difficulty in rounding correctly
- Difficulty in checking for errors in the calculation
Q: Can percent yield be used to predict the yield of a reaction with a catalyst?
A: Yes, percent yield can be used to predict the yield of a reaction with a catalyst. By knowing the percent yield of a reaction with a catalyst, you can determine how much product will be produced and whether the reaction will be efficient.
Q: What are some common applications of percent yield in environmental science?
A: Some common applications of percent yield in environmental science include:
- Determining the efficiency of a reaction to produce high-purity products
- Determining the efficiency of a reaction to produce high-purity products in a sustainable manner
- Determining the efficiency of a reaction to produce high-purity products with minimal waste
Q: Can percent yield be used to compare the efficiency of different reactions with different solvents?
A: Yes, percent yield can be used to compare the efficiency of different reactions with different solvents. By comparing the percent yield of different reactions, you can determine which reaction is more efficient and produces more product.
Q: What are some common challenges when using percent yield in real-world applications?
A: Some common challenges when using percent yield in real-world applications include:
- Difficulty in determining the actual yield and theoretical yield
- Difficulty in using the correct units (such as grams or moles)
- Difficulty in rounding correctly
- Difficulty in checking for errors in the calculation
Q: Can percent yield be used to predict the yield of a reaction with a different reaction pathway?
A: Yes, percent yield can be used to predict the yield of a reaction with a different reaction pathway. By knowing the percent yield of a reaction with a different reaction pathway, you can determine how much product will be produced and whether the reaction will be efficient.
Q: What are some common applications of percent yield in the pharmaceutical industry?
A: Some common applications of percent yield in the pharmaceutical industry include:
- Determining the efficiency of a reaction to produce high-purity products
- Determining the efficiency of a reaction to produce high-purity products in a sustainable manner
- Determining the efficiency of a reaction to produce high-purity products with minimal waste
Q: Can percent yield be used to compare the efficiency of different reactions with different concentrations of reactants?
A: Yes, percent yield can be used to compare the efficiency of different reactions with different concentrations of reactants. By comparing the percent yield of different reactions, you can determine which reaction is more efficient and produces more product.
Q: What are some common challenges when using percent yield in the chemical industry?
A: Some common challenges when using percent yield in the chemical industry include:
- Difficulty in determining the actual yield and theoretical yield
- Difficulty in using the correct units (such as grams or moles)
- Difficulty in rounding correctly
- Difficulty in checking for errors in the calculation