Question #1c575
1 Answer
Yes, the percent yield is indeed
Explanation:
You know that the balanced chemical equation that describes this reaction looks like this
#2"X" + 3"Y" + 4"Z" -> 5"W"#
As you can see, for every
In your case, you start with
Right from the start, you should be able to tell that
Since you only have
Consequently, you can say that at
#1 color(red)(cancel(color(black)("mole X"))) * overbrace("5 moles W"/(2color(red)(cancel(color(black)("moles X")))))^(color(blue)("given by the balanced chemical equation")) = "2.5 moles W"#
However, you know that the reaction actually produced
#"% yield" = "what you actually get"/"what you could theoretically get" * 100%#
will be equal to
#"% yield" = (1.25 color(red)(cancel(color(black)("moles W"))))/(2.5color(red)(cancel(color(black)("moles W")))) * 100% = color(darkgreen)(ul(color(black)(50%)))#