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anonymous
 one year ago
Aluminum oxide can be formed from its elements. How many grams of aluminum will react with 12.0 L of oxygen at STP?
anonymous
 one year ago
Aluminum oxide can be formed from its elements. How many grams of aluminum will react with 12.0 L of oxygen at STP?

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0This has a formula right?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I can help you, but just making sure

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0No the problem does not include a equation

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Oh okay thank you, do you want me to upload the problem?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Well first tell me, what's the atomic weight of Al?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0This is the problem and the attempt I have done for it.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Okay, so this problem involves stoicheomitry

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yeah I think so, but I'm not sure if what I did was right

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0You're on the right track about the Oxygen part but you got to convert the moles of oxygen into moles Al

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0yeah I used the ratio of 2/3 as the conversion since no conversion was given. I used 2/3 because of Al2O3

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0so I multiplied 2/3 by the moles of O2 (.54) in order to get the moles of Al

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0You don't need to convert the number into moles of Al, Al is simply 1 mol on the denominator if numerator.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0and multiply this by the MW of Al

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0so multiply .54 by the molar mass of Al?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yeah, but you can solve this problem using one whole stoicheiomectric uhh setup.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0oh okay, thanks. If you don't mind, could I ask you 2 more equations?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0sorry I meant to say questions

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0hould look like this. But sure!

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0yeah I did learn it like that too, but my professor wants us to write it out like the way I showed you.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Ah alright. Well are you in Chemistry Honors or AP CHem. ?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0But you wrote it correctly also!

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0I'm actually in college right now and I'm talking chem

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0That's awesome. Well I'll help either way! I'm going to college this fall. Anyways, your qestions?

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Cool!!! Did I write these two question right? I feel like I did not.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0first one is right. And 2nd one, you go to balance the equation first which you're doing.. and hold on lemme do the equation

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Okay, yeah cause I was getting confused on how to balance the second equation

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0ugh now I'm stuck on the balancing ..

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0yeah... thats where I got stuck too. I can do the rest of the problem easily but the balancing part is really messing me up

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Umm could you ask your professor though and let me know too? Ugh sorry about that :C

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Yeah I tried doing that and he as not emailed me back yet. And plus my exam is tomorrow, so idk when he's going to email me back. But thank you soo much for you help!!! (:

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0And don't worry about it, you've helped me a lot!!!!!

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0wait, maybe no balancing is required. There's 2.5 M of potassium ssulfite

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0Or maybe oh crap .. but you're welcome though!
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