Question #2b111

1 Answer
Slangus · Grace
Nov 20, 2015

#"Actual Yield"/"Theoretical Yield"#

Explanation:

From the two reactants that are to be used in a reaction, it can be determined what the limiting reactant will be. Using the mass of the limiting reactant -the theoretical yield can be determined.

The theoretical yield represents the mass of product that can be made if the reaction reaches 100% completion.

This will not happen, mostly due to thermodynamics, equilibrium, and impure reactants. Therefore the actual yield will be a little less than the theoretical yield.

#"Actual yield"/"Theoretical yield"# x #100# = #"Percent yield"#

Related questions
See all questions in Percent Yield
Impact of this question
1979 views around the world
You can reuse this answer
Creative Commons License