What possible reasons could be advanced that Jim recovered #82*g# of product that yielded #95*g#?

1 Answer
Nov 16, 2016

Answer:

Clearly, Jim is a duffer in the lab.

Explanation:

In every chemical reaction ever performed, mass is conserved. If you start with #100*g# of reactants, at most you can get #100*g# of product. In practice you are not even going to get that. Reactions seldom proceed with #100%# yield, and even if they do, some losses are going to occur on handling, i.e. getting your product out of the reaction vessel, purifying it, getting it into a tared bottle; mass loss occurs down the line.

Here, Jim lost #(95-82)=13*g#. Jim was apparently a bit lax in scraping his product out of the reaction vessel; or maybe it didn't crystallize out of solution completely. If the product were pure, the loss may be acceptable.