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Lena772

  • one year ago

Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the volume and molarity of Sulfuric Acid. Calculate the theoretical mass (in grams) of Sodium Sulfate produced using only the mass of Sodium Carbonate. What is the theoretical yield (in grams) of Sodium Sulfate? What mass (in grams) of the excess reactant is left over after the reaction?

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  1. Lena772
    • one year ago
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    \[H_{2}SO_{4}+Na_{2}CO_{3} \rightarrow H_{2}CO_{3} + Na_{2}SO_{4}\]

  2. anonymous
    • one year ago
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    Alright this is molarity question

  3. anonymous
    • one year ago
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    First off this is a double displacement question and I assume you know it.

  4. Lena772
    • one year ago
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    M= moles solute/L of solution moles solute= M*L m=4.9M*0.00698L =0.034202*105.99 g/ 1 mol = 3.6 mol However, I get that this is incorrect

  5. Lena772
    • one year ago
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    That should say 3.6g not mol.

  6. anonymous
    • one year ago
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    This is a very simple question. You ask your periodic table "hey what's up man tell me what your molar mass label has to say and I'll add them up happy to the kingdom come"

  7. anonymous
    • one year ago
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    Oh shiz I didn't note "using only the mass for the reactant" ok

  8. anonymous
    • one year ago
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    You do the happy stoichometry

  9. Lena772
    • one year ago
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    Do you see where I went wrong?

  10. anonymous
    • one year ago
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    Why don't you just use the stoichiometry ratio?

  11. anonymous
    • one year ago
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    I recommend stoichoimetry for the sake of simplicity because it's easier

  12. anonymous
    • one year ago
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    @Nnesha what's your take on this?

  13. Lena772
    • one year ago
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    I don't know what you mean by the stoichiometry ratio.

  14. anonymous
    • one year ago
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    I am gonna give you the kingdom come so the ratio between sulfuric acid used and sodium sulfate used is 1:1 meaning that every mole of sulfuric acid results in one mole of sodium sulfate. So find the overall gram of sodium sulfate by looking at periodic table and add them together.

  15. anonymous
    • one year ago
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    for 1 mole of reactant results in 1 mole of product.

  16. anonymous
    • one year ago
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    pretty simple isn't it?

  17. anonymous
    • one year ago
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    @empty if you could elaborate what I mean that's great

  18. anonymous
    • one year ago
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    that dude got scared off

  19. anonymous
    • one year ago
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    ok I am here with you no worries

  20. anonymous
    • one year ago
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    but I am really sleepy right now vote on my thread

  21. Lena772
    • one year ago
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    Add what together? I don't understand.

  22. anonymous
    • one year ago
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    @empty pitch in dude don't be the spectator ion

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