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anonymous

  • one year ago

When 0.422g of phosphorus is burned 0.967g of a white oxide is obtained. Determine the empirical formula of the oxide

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  1. Shikamaru11
    • one year ago
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    now what's that we gonna use the combustion analysis here too @Photon336 Sir???

  2. Photon336
    • one year ago
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    @Shalante this is your type of problem.

  3. Photon336
    • one year ago
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    i'm not sure myself @Shikamaru11 thoughts?

  4. Rushwr
    • one year ago
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    Combustion is when u burn it in air soo we have to write the balanced equation for the reaction between phosphorus and O2

  5. Shikamaru11
    • one year ago
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    Sir will be the equation is something like that?????????? \[P+ZnO \rightarrow ????\] hope i could think far

  6. Rushwr
    • one year ago
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    Wait I dnt think we need to go for the equation. We can just assume that all of the phosphorus is now in the oxide.

  7. Photon336
    • one year ago
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    \(\color{#0cbb34}{\text{Originally Posted by}}\) @Rushwr Combustion is when u burn it in air soo we have to write the balanced equation for the reaction between phosphorus and O2 \(\color{#0cbb34}{\text{End of Quote}}\) yeah, was thinking that too, BTW where did the zinc come from?

  8. Rushwr
    • one year ago
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    Considering phosphorus as the limiting agent

  9. Shikamaru11
    • one year ago
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    oh I got that in a second shot I think it mentioned white oxide but it's the obtant so my hypothesis failed :P

  10. Shikamaru11
    • one year ago
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    hey my guess of PO4 lolxxxx :P

  11. Rushwr
    • one year ago
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    we only need to find the empirical formula of the oxide right? So what if we consider that all of the phosphorus present are in the oxide now ? So the rest of the mass that is from 0.967 is oxygen SO the mass of oxygen in the oxide = 0.967 - 0.422 = 0.545g We can find the no. of moles of each separately Moles = mass/ molar mass moles of P = 0.422/ 31 = 0.014 moles Moles of Oxygen = 0.545/16 = 0.034 moles Now divide each by the smallest no. of moles |dw:1444362596720:dw| Now the ratio between P: O is 1:2.5 But we can't keep the ration in decimal numbers so to make it a whole number we multiply it by 2 so the new ratio would be 2:5 So the empirical formula would be P2O5

  12. Rushwr
    • one year ago
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    @Photon336 @Shikamaru11 What do u think Am i wrong somewhere?

  13. Shikamaru11
    • one year ago
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    hmmmm point to ponderwell you've won the world CUP :) friend @Rushwr

  14. Rushwr
    • one year ago
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    LOL ....... Thanks !!! @Shikamaru11

  15. Shikamaru11
    • one year ago
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    no dude you deserve it I'll call FIFA to give you the CUP next time :D :P :D

  16. Rushwr
    • one year ago
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    ROFL !!!!!!!!! Okai then I'll wait for it !!! >_< @Shikamaru11

  17. Photon336
    • one year ago
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    omg now is a great time for a study group.

  18. Rushwr
    • one year ago
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    hahahahahaha Yaaaaaaaaaaaaasssssssssssss @Photon336

  19. Photon336
    • one year ago
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    we've got Shalante you and shika

  20. Rushwr
    • one year ago
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    The only 2 missing here is Tara and woodward

  21. Rushwr
    • one year ago
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    Didn't hear from tara lately though

  22. Rushwr
    • one year ago
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    SO what are we up to ? Any questions before I leave.

  23. Shikamaru11
    • one year ago
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    :) i think that's enough for now my left eye got blanked and this chemistry :D but have you loved somebody :P @Rushwr

  24. Rushwr
    • one year ago
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    lol y? @Shikamaru11

  25. Shikamaru11
    • one year ago
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    you asked us to questio so i did :D @Rushwr

  26. Rushwr
    • one year ago
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    LOL I meant chemistry ones not this !!! @Shikamaru11

  27. Shikamaru11
    • one year ago
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    oh Sorry sir mistake Action replay :D :P @Rushwr :) stay happy

  28. Rushwr
    • one year ago
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    LOL I will I will @Shikamaru11

  29. Rushwr
    • one year ago
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    And not sir ! Miss

  30. Shikamaru11
    • one year ago
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    @Rushwr sorry ma'm I asked the wrong one I didn't know that you're ma'm :)

  31. Rushwr
    • one year ago
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    lol oki

  32. Shikamaru11
    • one year ago
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    @Rushwr thanks for being nice :)

  33. Rushwr
    • one year ago
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    No problem !!!! :) @Shikamaru11

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