Question

If you were to perform this reaction in a lab, you would make far less than the theoretical yield of product due to a wide range of outside factors. We can compare the actual yield to the theoretical yield to calculate the percent yield: percent yield=actual yieldtheoretical yield×100% Keep in mind that the percent yield can be calculated using any unit of mass or moles, so long as they are the same. For example, you can divide moles by moles, or grams by grams, but you cannot divide moles by grams or vice versa. Part D

Answer 1

In a reaction,

percent yield is a term which is represented in percent "%" only.

It does not have any other unit

So If we to find percent yield of say a Raction A forming Product B

Theoretical yield of product B from A = x g

From the experiment carried out in the lab,

we get product A yield = y g

Then,

percent yield for product B by this reaction = (y g/x g) x 100

So here, unit "g" gets cancelled out and we end up with "%" unit for the percent yield.

Similarly, one may do this calculations, with say x moles of Product B (theoretical yield) and y moles of product B by experimental calculation.

Again,

percent yield = (y moles/x moles) x 100

Here, moles in numerator vets cancelled by moles in the denominator. Thus the net unit for percent yield remained as "%".

If instead one uses combinaton say x moles and y g, then the units does not cancelled out and the percent yield is incorrect by this method.