Question #5efd9

1 Answer
May 5, 2017

Answer:

#42%#

Explanation:

To get the reaction's percent yield, you must divide the actual yield by the theoretical yield and multiply the result by #100%#.

#"% 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 #"100 g"# of product that you could theoretically get.

In this example, you get #"4.5 g"# of beryllium chloride for #"10.7 g"# of beryllium chloride that you could theoretically get, which means that for #'100 g"# of beryllium chloride that you could theoretically get, you will actually have

#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 #42%#.