# Question #5efd9

##### 1 Answer

#### Answer:

#### Explanation:

To get the reaction's percent yield, you must divide the actual yield by the theoretical yield and multiply the result by

#"% yield" = "actual yield"/"theoretical yield" xx 100%#

In your case, you will have

#"% yield" = (4.5 color(red)(cancel(color(black)("g"))))/(10.7color(red)(cancel(color(black)("g")))) xx 100% = 42%#

The answer is rounded to two **sig figs**, the number of sig figs you have for the actual yield of the reaction.

The idea here is that the reaction's percent yield tells you the number of grams of product you get for every *theoretically* get.

In this example, you get

#100 color(red)(cancel(color(black)("g"))) * "4.5 g"/(10.7color(red)(cancel(color(black)("g")))) = "42 g"#

Therefore, the reaction's percent yield is