8.7 Two products are formed in the following reaction in a 50:50 mixture. Would the resulting solution be optically active
1 answer:
Answer:
Yes. The solution would be optically active.
Explanation:
Diastereomer are defined as the image that is non mirror and non -identical. It is made up of two stereoisomers. They are formed when the two stereoisomers or more than two stereoisomers of the compound have the same configuration at the equivalent stereocenters.
In the given context, as the product given is a diastereomeric mixture, the product would have an optical activity in total.
So the answer is Yes.
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Answer:
BaBr2
Explanation:
Halide ions are the ions of the elements of group 17 (or 7A), which have 7 electrons in their valence shell, so they need to gain one electron to be stable. If we noted as X the halide, the ion must be .
Barium is a metal of group 2 (or 2A) and has 2 electrons in its valence shell, so it must lose these 2 electrons to be stable, and it will form the anion . These elements will form an ionic bond, with formula BaX2.
Sulfuric acid has formula H2SO4, and the reaction is:
BaX2 + H2SO4 --> BaSO4 + 2HX
So, for the stoichiometry between BaX2 and BaSO4, and denoting by <em>y</em> the molar mass of the halide, and the molar mass of BaSO4 = 137.33 g of Ba + 32.06 g of S + 4x16 g of O = 233.39
1 mol of BaX2 ------------- 1 mol of BaSO4
(137.33 + 2y) g of BaX2 ------------ 233.39 g of BaSO4
0.158 g of BaX2 --------------------- 0.124 g of BaSO4
By a simple direct three rule:
0.124x(137.33 + 2y) = 0.158x233.39
17.02892 + 0.248y = 36.87562
0.248y = 19.8467
y = 19.8467/0.248
y = 80.03 g/mol
By consulting the periodic table, the halide element that has a molar mass close to 80.03 g/mol is Bromide (Br), which has molar mass 79.9 g/mol. So the salt has formula BaBr2.