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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?

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  1. anonymous
    • one year ago
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    This has a formula right?

  2. anonymous
    • one year ago
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    I can help you, but just making sure

  3. anonymous
    • one year ago
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    No the problem does not include a equation

  4. anonymous
    • one year ago
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    Oh okay thank you, do you want me to upload the problem?

  5. anonymous
    • one year ago
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    Yeah that's fine :3

  6. anonymous
    • one year ago
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    Well first tell me, what's the atomic weight of Al?

  7. anonymous
    • one year ago
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    26.98

  8. anonymous
    • one year ago
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    This is the problem and the attempt I have done for it.

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  9. anonymous
    • one year ago
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    Okay, so this problem involves stoicheomitry

  10. anonymous
    • one year ago
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    Yeah I think so, but I'm not sure if what I did was right

  11. anonymous
    • one year ago
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    You're on the right track about the Oxygen part but you got to convert the moles of oxygen into moles Al

  12. anonymous
    • one year ago
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    yeah I used the ratio of 2/3 as the conversion since no conversion was given. I used 2/3 because of Al2O3

  13. anonymous
    • one year ago
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    so I multiplied 2/3 by the moles of O2 (.54) in order to get the moles of Al

  14. anonymous
    • one year ago
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    You don't need to convert the number into moles of Al, Al is simply 1 mol- on the denominator if numerator.

  15. anonymous
    • one year ago
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    and multiply this by the MW of Al

  16. anonymous
    • one year ago
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    so multiply .54 by the molar mass of Al?

  17. anonymous
    • one year ago
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    Yeah, but you can solve this problem using one whole stoicheiomectric uhh setup.

  18. anonymous
    • one year ago
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    oh okay, thanks. If you don't mind, could I ask you 2 more equations?

  19. anonymous
    • one year ago
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    sorry I meant to say questions

  20. anonymous
    • one year ago
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    hould look like this. But sure!

  21. anonymous
    • one year ago
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    Should*

  22. anonymous
    • one year ago
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    yeah I did learn it like that too, but my professor wants us to write it out like the way I showed you.

  23. anonymous
    • one year ago
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    Ah alright. Well are you in Chemistry Honors or AP CHem. ?

  24. anonymous
    • one year ago
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    But you wrote it correctly also!

  25. anonymous
    • one year ago
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    I'm actually in college right now and I'm talking chem

  26. anonymous
    • one year ago
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    That's awesome. Well I'll help either way! I'm going to college this fall. Anyways, your qestions?

  27. anonymous
    • one year ago
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    Cool!!! Did I write these two question right? I feel like I did not.

  28. anonymous
    • one year ago
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    first one is right. And 2nd one, you go to balance the equation first which you're doing.. and hold on lemme do the equation

  29. anonymous
    • one year ago
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    Okay, yeah cause I was getting confused on how to balance the second equation

  30. anonymous
    • one year ago
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    ugh now I'm stuck on the balancing .-.

  31. anonymous
    • one year ago
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    yeah... thats where I got stuck too. I can do the rest of the problem easily but the balancing part is really messing me up

  32. anonymous
    • one year ago
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    Umm could you ask your professor though and let me know too? Ugh sorry about that :C

  33. anonymous
    • one year ago
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    Yeah 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!!! (:

  34. anonymous
    • one year ago
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    And don't worry about it, you've helped me a lot!!!!!

  35. anonymous
    • one year ago
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    wait, maybe no balancing is required. There's 2.5 M of potassium ssulfite

  36. anonymous
    • one year ago
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    Or maybe oh crap .-. but you're welcome though!

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spraguer (Moderator)
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