In an experiment to prepare a particular compound, the theoretical yield s 65.3 g and the actual yield is 56.3 g. What is the percent yield?

Mar 5, 2017

86.2%

Explanation:

A reaction's percent yield is simply the number of grams of a product that you actually get for every $\text{100 g}$ of said product that you could theoretically get.

The number of grams of a product that can theoretically be obtained by a reaction is called the theoretical yield. This value is calculated using stoichimetry and assuming that the raction has a 100% yield.

The number of grams of a product that are actually produced by a reaction is called the actual yield. This value is detemined experimentally, i.e. by actually doing the reaction.

In your case, the reaction has a theoretical yield of $\text{65.3 g}$ and an actual yield of $\text{56.3 g}$.

Since your goal is to determine the number of grams produced for every $\text{100 g}$ that could theoretically be produced, you can use this ratio as a conversion factor

100 color(red)(cancel(color(black)("g theoretically"))) * "56.3 g actually"/(65.3color(red)(cancel(color(black)("g theoretically")))) = "86.2 g actually"

Thsi means that the reaction has a percent yield of

$\textcolor{\mathrm{da} r k g r e e n}{\underline{\textcolor{b l a c k}{\text{% yield = 86.2%}}}}$

For every $\text{100 g}$ of product that could be produced, the reaction produces $\text{86.2 g}$ of product.

The answer is rounded to the sig figs.