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anonymous

  • one year ago

Molar conversion help please!

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  1. anonymous
    • one year ago
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    The NaHCO3 is the limiting reactant and the HCl is the excess reactant in this experiment. Determine the theoretical yield of the NaCl product, showing all of your work in the space below. (5 points) So far I have 12.71 g NaHCO3 / 83.96 g per mole NaHCO3 = 0.151

  2. sweetburger
    • one year ago
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    Whats your question to be exact?

  3. anonymous
    • one year ago
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    What is the theoretical yield of NaCl with the mass of NaHCO3 being 12.71 g and HCl being in excess. NaHCO3 +HCl → NaCl + CO2+ H2O

  4. anonymous
    • one year ago
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    Some direction or correction would be helpful

  5. sweetburger
    • one year ago
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    Alright so you found the number of moles of NaHCO3. Im assuming your math is correct (it looks correct). So from here we can find the number of moles of NaCl produced. |dw:1440617996106:dw|

  6. anonymous
    • one year ago
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    .151 x 1 = .151, but could you mind checking my work of converting grams to moles? (like the process/formula)

  7. sweetburger
    • one year ago
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    sure

  8. anonymous
    • one year ago
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    thank you

  9. sweetburger
    • one year ago
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    your math is correct but if you want the correct number of significant digits it should be .1514

  10. anonymous
    • one year ago
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    Oh thank you, I appreciate it. So, we don't have to mess with HCl conversion because it's in excess, right? I only really have to convert .1514 mole NaCl to grams?

  11. sweetburger
    • one year ago
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    yea because HCl is in excess it would never be the limiting reagent this means that we are limited by the amount of NaHCO3 present and therefor whatever amount of NaHCO3 we have will directly affect the amount of products we will have when the reaction is completed

  12. sweetburger
    • one year ago
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    lemme know if you have any other questions

  13. anonymous
    • one year ago
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    It does. So all that's left is NaCl mole -> gram conversion to find it's theoretical yield?

  14. sweetburger
    • one year ago
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    yes if you need to find the mass of NaCl produced that would be the only thing left to do in this situation

  15. anonymous
    • one year ago
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    Ok thank you. I'll be back in like 30 seconds.

  16. sweetburger
    • one year ago
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    aight

  17. anonymous
    • one year ago
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    OK. I'm resubmitting this and I was checking to see if I made any of the same mistakes. Well, all looks in order, you've been a great help thanks.

  18. sweetburger
    • one year ago
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    Alright glad to help :).

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