In class, students were given the following problem: "Aluminum satellite dishes resist corrosion because aluminum reacts with ox
ygen gas to form a coating of aluminum oxide (Al2O3). What is the mass of Al2O3?"
a) Sally solved the problem by first finding the molar mass of aluminum oxide. She calculated the molar mass of Al2O3 as 43.0 g/mol. This is not the correct molar mass however. What did sally do wrong?
b) After finding the molar mass of Al2O3, Jacob set up the following conversion. (I'll add a pic)
Is this the correct set up for the problem?
a) Sally solved the problem by first finding the molar mass of aluminum oxide. She calculated the molar mass of Al2O3 as 43.0 g/mol. This is not the correct molar mass however. What did sally do wrong?
b) After finding the molar mass of Al2O3, Jacob set up the following conversion. (I'll add a pic)
Is this the correct set up for the problem?
1 answer:
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Answer:
a) Limiting: sulfur. Excess: aluminium.
b) 1.56g Al₂S₃.
c) 0.72g Al
Explanation:
Hello,
In this case, the initial mass of both aluminium and sulfur are missing, therefore, one could assume they are 1.00 g for each one. Thus, by considering the undergoing chemical reaction turns out:
a) Thus, considering the assumed mass (which could be changed based on the one you are given), the limiting reagent is identified as shown below:
Thereby, since there 1.00g of aluminium will consume 0.0554 mol of sulfur but there are just 0.0156 mol available, the limiting reagent is sulfur and the excess reagent is aluminium.
b) By stoichiometry, the produced grams of aluminium sulfide are:
c) The leftover is computed as follows:
NOTE: Remember I assumed the quantities, they could change based on those you are given, so the results might be different, but the procedure is quite the same.
Best regards.