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Why should you not measure more than 100% product? a. Measuring more than 100% yield indicates...

Question:

Why should you not measure more than 100% product?

a. Measuring more than 100% yield indicates impurities.

b. Measuring more than 100% yield indicates mathematical or experimental errors.

c. The conservation of matter states matter cannot be created.

d. All of the above.

Calculating Yields:

The yield of a reaction is often communicated as a percent to tell us how much of the expected product was actually produced. The theoretical yield is calculated using stoichiometry, while the experimental yield is measured experimentally. The formula is:

{eq}\rm \%\:yield = \frac{experimental\:yield}{theoretical\:yield}\times 100\%{/eq}

Answer and Explanation:

Option a is correct because to get a yield higher than 100% means that your product likely gained mass from other materials being mixed with the product. These other materials can be referred to as impurities.

Option b is also correct as mathematical mistakes can lead to the error. Experimental errors like not completely drying a product before massing it or not using a sufficiently valid separation method to isolate the desired product can lead to yields that are higher than 100%.

Option c is also correct as obtaining a yield above 100% means more product was produced than was possible from the amount of reactants. Thus yields above 100% imply that new matter was created. This violates the law of conservation of matter, which states matter cannot be created nor destroyed in chemical reactions.

Therefore Option D is the correct answer.


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