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:
Explanation:
We have to start with the <u>reaction</u>:
We have the same amount of atoms on both sides, so, we can continue. The next step is to find the <u>number of moles</u> that we have in the 110.0 g of carbon dioxide, to this, we have to know the <u>atomic mass of each atom</u>:
C: 12 g/mol
O: 16 g/mol
Mg: 23.3 g/mol
If we take into account the number of atoms in the formula, we can calculate the <u>molar mass</u> of carbon dioxide:
In other words: . With this in mind, we can calculate the moles:
Now, the <u>molar ratio</u> between carbon dioxide and magnesium carbonate is 1:1, so:
With the molar mass of (
. With this in mind, we can calculate the <u>grams of magnesium carbonate</u>:
I hope it helps!