Question

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?

Answer 1

`86.2%`

Explanation:

A reaction's percent yield is simply the number of grams of a product that you actually get for every `"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 `"65.3 g"` and an actual yield of `"56.3 g"`.

Since your goal is to determine the number of grams produced for every `"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

`color(darkgreen)(ul(color(black)("% yield = 86.2%")))`

For every `"100 g"` of product that could be produced, the reaction produces `"86.2 g"` of product.

The answer is rounded to the sig figs.