Question #0601d
1 Answer
Explanation:
If I understand your question correctly, the answer will be
The trick here is to realize that the combined mass of the reactants must be equal to the combined mass of the products
You know that you're mixing
#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
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
#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
#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
#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