Well, let me calculate it in the most hilarious way possible! Buckle up!
So, first things first. We have 13.5 grams of aluminum. Now, if aliens invaded Earth and turned all our aluminum into tin foil hats, we would be pretty screwed, don't you think? But lucky for us, this aluminum is doing something much more useful - reacting with oxygen to form Al2O3!
Now, let's convert the grams of aluminum into moles. Since molar mass of Al is 27 g/mol, we divide 13.5 g by 27 g/mol, and guess what? We get 0.5 moles of aluminum. It's like finding half a donut in your pocket - unexpected but delicious!
Now, in that balanced equation, we see that for every 4 moles of aluminum, we get 2 moles of Al2O3. So, for 0.5 moles of aluminum, we can expect (drumroll, please) 0.25 moles of Al2O3. It's like getting a quarter, but instead of putting it in a piggy bank, you make fancy aluminum oxide!
Finally, we convert those moles into grams. The molar mass of Al2O3 is 102 g/mol. Multiply 0.25 moles by 102 g/mol, and voila! We have about 25.5 grams of Al2O3. It's as if we suddenly found 25.5 grams of gold under our pillows. I guess dreams do come true!
So, to sum it up, if 13.5 grams of aluminum completely react with oxygen according to the balanced equation, we would expect to obtain approximately 25.5 grams of Al2O3. That's a lot of shiny oxide, my friend!