What Is the Percent Yield from Aluminum to Potassium Alum?

You are getting in your own way with this.In summary, the question is asking for the percent yield of potassium alum when 5.00 g of aluminum is used to obtain 75.0 g of potassium alum. To solve this, the reaction equation for the formation of potassium alum (KAl(SO4)2) needs to be written. Then, the theoretical yield can be calculated using stoichiometry, but it is not clear if this is the correct approach since the actual yield is much greater than the theoretical yield. More information is needed to determine if any errors were made in the calculation. Additionally, it is important to use the appropriate number of significant figures in the calculation.
  • #1
Lili123
6
0
Please post this type of questions in HW section using the template.
Here is the question: If 75.0 g of potassium alum is obtained from 5.00 g of aluminum, what is the percent yield?

This is what I've done so far, but I'm not sure if it is fully correct:
5.00g Al x (1/26.98156) x (1/1) x 258.207 = 47.84882537g potassium alum

Wouldn't this then be the theoretical yield? But then that wouldn't work because the actual yield of 75.0g is much greater... is there something I did wrong here?
 
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  • #2
Lili123 said:
5.00g Al x (1/26.98156) x (1/1) x 258.207 = 47.84882537g potassium alum

And you expect us to guess what these numbers mean?

Please start by writing the reaction equation. What is the formula of the alum? Hint: it is not just KAl(SO4)2.
 
  • #3
Another hint: You've been given a three significant figure problem. Piling on significant figures is neither useful nor impressive.
 
Last edited:

1. What is percent yield and why is it important?

Percent yield is a measure of the efficiency of a chemical reaction, indicating how much of the desired product was obtained compared to the theoretical yield. It is important because it allows scientists to assess the success of a reaction and make adjustments for future experiments.

2. How is percent yield calculated?

Percent yield is calculated by dividing the actual yield (the amount of product obtained in a reaction) by the theoretical yield (the amount of product that should have been obtained based on stoichiometric calculations) and multiplying by 100%.

3. What factors can affect the percent yield of a reaction?

Several factors can affect the percent yield of a reaction, including impurities in the reactants, side reactions, incomplete reactions, and errors in the measuring or handling of the reactants.

4. How can the percent yield be improved?

To improve the percent yield of a reaction, scientists can use high-quality and pure reactants, optimize reaction conditions such as temperature and pressure, and carefully measure and handle the reactants to minimize errors.

5. What is a good percent yield?

A good percent yield is typically around 90-95%, although it can vary depending on the reaction and the specific goals of the experiment. A percent yield of 100% is not always achievable due to practical limitations.

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