The theoretical yield of a reaction is 82.5 grams, but the reaction actually yields 12.3 grams less than expected. What is the percent yield for this reaction?
Percent yield is defined as the ratio between the actual yield and the theoretical yield of the reaction, multiplied by
#color(blue)(|bar(ul(color(white)(a/a)"% yield" = "what you actually get"/"what you should theoretically get" xx 100 color(white)(a/a)|)))#
So, you know that your reaction has a theoretical yield of
In other words, the theoretical yield tells you how much product is produced for a
Now, the reaction is said to produce
#"actual yield" = "82.5 g" - "12.3 g" = "70.2 g"#
The reaction's percent yield will thus be
#"% yield" = (70.2 color(red)(cancel(color(black)("g"))))/(82.5color(red)(cancel(color(black)("g")))) xx 100 = color(green)(|bar(ul(color(white)(a/a)"85.1%"color(white)(a/a)|)))#
The answer is rounded to three sig figs.