Question #0601d

1 Answer
Jul 20, 2017

#"197 g"#

Explanation:

If I understand your question correctly, the answer will be #"197 g"#.

The trick here is to realize that the combined mass of the reactants must be equal to the combined mass of the products #-># think the Law of conservation of mass here.

You know that you're mixing #"20 g"# of aluminium metal and #"200 g"# of bromine, but that the reaction only consumes

#overbrace("200 g")^(color(blue)("what is available")) - overbrace("23 g")^(color(blue)("what is left behind")) = "177 g"#

of bromine. This means that the combined mass of the reactants will be

#"20 g + 177 g = 197 g"#

Since the reaction will only produce aluminium bromide, you can say that the mass of the product must be equal to #"197 g"#.

CHECK THE RESULT USING MOLES

If you want, you can check the result by using the balanced chemical equation

#2"Al"_ ((s)) + 3"Br"_ (2(l)) -> "Al"_ 2"Br"_ (6(aq))#

Use the molar masses of the two reactants to calculate how many moles of each take part in the reaction--keep in mind that only #"177 g"# of bromine react!

#20 color(red)(cancel(color(black)("g"))) * "1 mole Al"/(27.0color(red)(cancel(color(black)("g")))) = "0.74 moles Al"#

#177 color(red)(cancel(color(black)("g"))) * "1 mole Br"_2/(159.8color(red)(cancel(color(black)("g")))) = "1.11 moles Br"_2#

Aluminium reacts with bromine in a #2:3# mole ratio

#0.74 color(red)(cancel(color(black)("moles Al"))) * "3 moles Br"_2/(2color(red)(cancel(color(black)("moles Al")))) = "1.11 moles Al"#

and produces aluminium bromide in a #2:1# mole ratio

#0.74 color(red)(cancel(color(black)("moles Al"))) * ("1 mole Al"_2"Br"_6)/(2color(red)(cancel(color(black)("moles Al")))) = "0.37 moles Al"_2"Br"_6#

Finally, to convert this to grams, use the molar mass of aluminium bromide

#0.37 color(red)(cancel(color(black)("moles Al"_2"Br"_6))) * "533.4 g"/(1color(red)(cancel(color(black)("mole Al"_2"Br"_6)))) ~~ "197 g"#

Without taking into account the number of sig figs you have for your values, you can say that th answer will once again be #"197 g"# of aluminium bromide.