can percent yield be more than 100%?

Question

my actual yield is more than my theoretical yield. is that possible??

Answer 1

IT MOST CERTAINLY CAN!!!!

It actually is possible to obtain an actual yield higher than your theoretical yield. One particular experiment comes to mind in which this happened was due to an excess of zinc in the mixture, but I don't recall what the exact experiment was. Suffice to say that it is possible.

However, I agree with rest of the answers that 999 times out of 1000, you will not have a percent yield higher than 100 and there is likely an error in your calculation.

Answer 2

Percent Yield Greater Than 100

Answer 3

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The ideal or theoretical yield of a chemical reaction would be 100%, a value that is impossible to achieve due to limitations in measurement accuracy. According to Vogel's Textbook of Practical Organic Chemistry, yields around 100% are called quantitative, yields above about 90% are called excellent, yields above about 80% very good, yields above about 70% are called good, yields below about 50% are called fair, yields below about 40% are called poor.[1] Yields may appear to be above 100% when products are impure. Purification steps always lower the yield and the reported yields usually refer to the yield of the final purified product.

Answer 4

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RE:
can percent yield be more than 100%?
my actual yield is more than my theoretical yield. is that possible??

Answer 5

you will not have a percent yield higher than 100

Answer 6

Not if you have been careful with every step of the synthesis. It means that there may be some leftover reactants in your final product, which may have been released as a gaseous byproduct, which would bring the weight of the yield up. Is the final product something that can be tested with a melting temperature? If so, test it, and I would be almost certain that it is not a pure product.

Answer 7

I canthin of a few ways that could be possible but they are unlikely. The reaction would have to somehow leech molecules from the enviroment that were unaccounted for. It is more likely tat you had less of your original reactant than you thought or you measured the product wrong.

Answer 8

Here are some possibilities:
1. You accidentally put more of the reagents in than you thought.

2. You've done your calculations wrong.

3. Your "product" is impure:
3a) You weighed it while it was "wet" and therefore included the weight of some of the solvent.
3b) Whatever method you used for purifying the product didn't go so well; if you're crystallizing the product, you've still included impurities and you should recrystallize.

Answer 9

yes

Answer 10

No. This is not possible.

There is an error in your calculations or measurements somewhere.

Do not worry. This happens all the time in scientific research. That's why we call it research. :) Bceuase you search for an answer, do not find it... then you re-search, and re-search, and re-search, etc... until you find a repeatable result. :)

Hope this helps ... and hope you enjoyed my geek humor, too. :)