# Question #2b111

Nov 20, 2015

$\text{Actual Yield"/"Theoretical Yield}$

#### 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.

$\text{Actual yield"/"Theoretical yield}$ x $100$ = $\text{Percent yield}$