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?
1 Answer
Explanation:
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.