Question #d2807
1 Answer
Explanation:
The idea here is that you need to convert the volumes to moles by using the densities and the molar masses of the three chemical species of interest.
You will have
- acetic acid
#4.40 color(red)(cancel(color(black)("mL"))) * "1.05 g"/(1color(red)(cancel(color(black)("mL")))) = "4.62 g"#
#4.62 color(red)(cancel(color(black)("g"))) * "1 mole acetic acid"/(60.0color(red)(cancel(color(black)("g")))) = "0.0770 moles"#
- isopentyl alcohol
#3.35color(red)(cancel(color(black)("mL"))) * "0.81 g"/(1color(red)(cancel(color(black)("mL")))) = "2.7135 g"#
#2.7135 color(red)(cancel(color(black)("g"))) * "1 mole isopentyl alcohol"/(88.2color(red)(cancel(color(black)("g")))) = "0.03077 moles"#
- isopentyl acetate
#3.25 color(red)(cancel(color(black)("mL"))) * "0.867 g"/(1color(red)(cancel(color(black)("mL")))) = "2.818 g"#
#2.818color(red)(cancel(color(black)("g"))) * "1 mole isopentyl acetate"/(130.2 color(red)(cancel(color(black)("g")))) = "0.02164 moles"#
Now, acetic acid and isopentyl alcohol react in a
In this case, isopentyl alcohol will be the limiting reagent, since
#"0.03077 moles " < " 0.0770 moles"#
Therefore, the reaction will consume
Consequently, the reaction should theoretically produce
However, you calculated that the reaction produced only
The percent yield for this reaction, which basically tells you how much product you should expect to see for every
#color(purple)(bar(ul(|color(white)(a/a)color(black)("% yield" = "what you actually get"/"what you should theoretically get" xx 100)color(white)(a/a)|)))#
will be equal to
#"% yield" = (0.02164 color(red)(cancel(color(black)("moles"))))/(0.03077color(red)(cancel(color(black)("moles")))) xx 100 = color(green)(bar(ul(|color(white)(a/a)color(black)(70.3%)color(white)(a/a)|)))#
The answer is rounded to three sig figs.