Lilac M.
asked • 05/30/21Please answer this asap!!!
write a balanced chemical equation for this reaction: In an experiment group of students produced 63.5 grams of aluminum bromide from the reaction of 113 g aluminum chromate and excess magnesium bromide
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1 Expert Answer
Sidney P. answered • 05/31/21
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Given substance is Al2(CrO4)3 because Al is 3+ and CrO4 is 2-; molar mass = 401.94g. Wanted substance is AlBr3 with molar mass = 266.69g. Balanced reaction: Al2(CrO4)3 + 3 MgBr2 --> 2 AlBr3 + 3 MgCrO4.
Stoichiometry: [113g Al2(CrO4)3] * [1 mole Al2(CrO4)3 /401.94g Al2(CrO4)3] * [2 mole AlBr3 /1 mole Al2(CrO4)3] * [266.69g AlBr3 /1 mole AlBr3] = 150 g AlBr3 theoretical yield.
Percent yield = 100 actual/theoretical = 100 (63.5 / 150) = 42.3%.
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Lilac M.
Also please: Identify the given substance by chemical formula and calculate its molar mass. Identify the wanted substance by chemical formula and calculate its molar mass. What is the theoretical amount of aluminum bromide that calculations indicate should have been produced? Show all work What was the percent yield from this experiment? Show the formula and all your work.05/30/21